thermal energy and heat
DESCRIPTION
Thermal Energy and Heat. Temperature. Particle level kinetic energy A measure of the average kinetic energy of the atoms or molecules of a substance Temperature increases if the motion of the particles increases. Thermal Energy (Q). Particle level Mechanical (total) Energy - PowerPoint PPT PresentationTRANSCRIPT
Thermal Energy and Heat
TemperaturebullParticle level kinetic energy
bullA measure of the average kinetic energy of the atoms or molecules of a substance
bullTemperature increases if the motion of the particles increases
Thermal Energy (Q)bullParticle level Mechanical (total) Energy
bullTotal kinetic and potential energy of a systemrsquos particles
HeatbullParticle level WORK
bullThe transfer of thermal energy
Methods of Heat TransferConductionbullHeat transfer through a material by collision
of atoms bullParticles in flame gain kinetic energy and
start moving faster ndash they collide with neighbouring atoms making them move more rapidly and heat spreads
bullOccurs well in metals
Methods of Heat TransferConvectionbullthe process of transferring heat by a circulating path of fluid particles ndash called a convection current
bullHot fluid spreads out and moves upwards cooler fluid takes its place creating a current
Methods of Heat TransferRadiationbullEnergy transfer by electromagnetic waves ndash no particles are necessary
bullie visible radio micro UV infrared X-rays
Calculating HeatbullWe use Specific Heat Capacity (c) Unit J(kg oC)
bullA measure of the amount of energy needed to raise the temperature of 10kg of a substance by 10oC
bullDifferent for every substancecwater ndash 418 x 103 J(kg oC)
Calculating Heat
Q = mcΔtbullQ = heat (J)bullm = mass (kg)bullc ndash specific heat capacity J(kg oC)
bullΔt ndash change in temp ndash Δt = tf - ti
Ex 1 What is the mass of a bucket of water that requires 84 x 104 J of heat to increase its temperature from 12oC to 22oC
Ans m = 20 kg
Latent Heat
What has more energyWater at 10oC or water at 50oC
Cooler particles move slower (less kinetic energy)
Hotter particles move faster (more kinetic energy)
What has more energyIce at 0oC or water at 0oC
Solid ndash Highly structured particles are trapped little motion
Liquid ndash Less structured particles can move more motion
Liquids are higher energy
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
TemperaturebullParticle level kinetic energy
bullA measure of the average kinetic energy of the atoms or molecules of a substance
bullTemperature increases if the motion of the particles increases
Thermal Energy (Q)bullParticle level Mechanical (total) Energy
bullTotal kinetic and potential energy of a systemrsquos particles
HeatbullParticle level WORK
bullThe transfer of thermal energy
Methods of Heat TransferConductionbullHeat transfer through a material by collision
of atoms bullParticles in flame gain kinetic energy and
start moving faster ndash they collide with neighbouring atoms making them move more rapidly and heat spreads
bullOccurs well in metals
Methods of Heat TransferConvectionbullthe process of transferring heat by a circulating path of fluid particles ndash called a convection current
bullHot fluid spreads out and moves upwards cooler fluid takes its place creating a current
Methods of Heat TransferRadiationbullEnergy transfer by electromagnetic waves ndash no particles are necessary
bullie visible radio micro UV infrared X-rays
Calculating HeatbullWe use Specific Heat Capacity (c) Unit J(kg oC)
bullA measure of the amount of energy needed to raise the temperature of 10kg of a substance by 10oC
bullDifferent for every substancecwater ndash 418 x 103 J(kg oC)
Calculating Heat
Q = mcΔtbullQ = heat (J)bullm = mass (kg)bullc ndash specific heat capacity J(kg oC)
bullΔt ndash change in temp ndash Δt = tf - ti
Ex 1 What is the mass of a bucket of water that requires 84 x 104 J of heat to increase its temperature from 12oC to 22oC
Ans m = 20 kg
Latent Heat
What has more energyWater at 10oC or water at 50oC
Cooler particles move slower (less kinetic energy)
Hotter particles move faster (more kinetic energy)
What has more energyIce at 0oC or water at 0oC
Solid ndash Highly structured particles are trapped little motion
Liquid ndash Less structured particles can move more motion
Liquids are higher energy
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Thermal Energy (Q)bullParticle level Mechanical (total) Energy
bullTotal kinetic and potential energy of a systemrsquos particles
HeatbullParticle level WORK
bullThe transfer of thermal energy
Methods of Heat TransferConductionbullHeat transfer through a material by collision
of atoms bullParticles in flame gain kinetic energy and
start moving faster ndash they collide with neighbouring atoms making them move more rapidly and heat spreads
bullOccurs well in metals
Methods of Heat TransferConvectionbullthe process of transferring heat by a circulating path of fluid particles ndash called a convection current
bullHot fluid spreads out and moves upwards cooler fluid takes its place creating a current
Methods of Heat TransferRadiationbullEnergy transfer by electromagnetic waves ndash no particles are necessary
bullie visible radio micro UV infrared X-rays
Calculating HeatbullWe use Specific Heat Capacity (c) Unit J(kg oC)
bullA measure of the amount of energy needed to raise the temperature of 10kg of a substance by 10oC
bullDifferent for every substancecwater ndash 418 x 103 J(kg oC)
Calculating Heat
Q = mcΔtbullQ = heat (J)bullm = mass (kg)bullc ndash specific heat capacity J(kg oC)
bullΔt ndash change in temp ndash Δt = tf - ti
Ex 1 What is the mass of a bucket of water that requires 84 x 104 J of heat to increase its temperature from 12oC to 22oC
Ans m = 20 kg
Latent Heat
What has more energyWater at 10oC or water at 50oC
Cooler particles move slower (less kinetic energy)
Hotter particles move faster (more kinetic energy)
What has more energyIce at 0oC or water at 0oC
Solid ndash Highly structured particles are trapped little motion
Liquid ndash Less structured particles can move more motion
Liquids are higher energy
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
HeatbullParticle level WORK
bullThe transfer of thermal energy
Methods of Heat TransferConductionbullHeat transfer through a material by collision
of atoms bullParticles in flame gain kinetic energy and
start moving faster ndash they collide with neighbouring atoms making them move more rapidly and heat spreads
bullOccurs well in metals
Methods of Heat TransferConvectionbullthe process of transferring heat by a circulating path of fluid particles ndash called a convection current
bullHot fluid spreads out and moves upwards cooler fluid takes its place creating a current
Methods of Heat TransferRadiationbullEnergy transfer by electromagnetic waves ndash no particles are necessary
bullie visible radio micro UV infrared X-rays
Calculating HeatbullWe use Specific Heat Capacity (c) Unit J(kg oC)
bullA measure of the amount of energy needed to raise the temperature of 10kg of a substance by 10oC
bullDifferent for every substancecwater ndash 418 x 103 J(kg oC)
Calculating Heat
Q = mcΔtbullQ = heat (J)bullm = mass (kg)bullc ndash specific heat capacity J(kg oC)
bullΔt ndash change in temp ndash Δt = tf - ti
Ex 1 What is the mass of a bucket of water that requires 84 x 104 J of heat to increase its temperature from 12oC to 22oC
Ans m = 20 kg
Latent Heat
What has more energyWater at 10oC or water at 50oC
Cooler particles move slower (less kinetic energy)
Hotter particles move faster (more kinetic energy)
What has more energyIce at 0oC or water at 0oC
Solid ndash Highly structured particles are trapped little motion
Liquid ndash Less structured particles can move more motion
Liquids are higher energy
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Methods of Heat TransferConductionbullHeat transfer through a material by collision
of atoms bullParticles in flame gain kinetic energy and
start moving faster ndash they collide with neighbouring atoms making them move more rapidly and heat spreads
bullOccurs well in metals
Methods of Heat TransferConvectionbullthe process of transferring heat by a circulating path of fluid particles ndash called a convection current
bullHot fluid spreads out and moves upwards cooler fluid takes its place creating a current
Methods of Heat TransferRadiationbullEnergy transfer by electromagnetic waves ndash no particles are necessary
bullie visible radio micro UV infrared X-rays
Calculating HeatbullWe use Specific Heat Capacity (c) Unit J(kg oC)
bullA measure of the amount of energy needed to raise the temperature of 10kg of a substance by 10oC
bullDifferent for every substancecwater ndash 418 x 103 J(kg oC)
Calculating Heat
Q = mcΔtbullQ = heat (J)bullm = mass (kg)bullc ndash specific heat capacity J(kg oC)
bullΔt ndash change in temp ndash Δt = tf - ti
Ex 1 What is the mass of a bucket of water that requires 84 x 104 J of heat to increase its temperature from 12oC to 22oC
Ans m = 20 kg
Latent Heat
What has more energyWater at 10oC or water at 50oC
Cooler particles move slower (less kinetic energy)
Hotter particles move faster (more kinetic energy)
What has more energyIce at 0oC or water at 0oC
Solid ndash Highly structured particles are trapped little motion
Liquid ndash Less structured particles can move more motion
Liquids are higher energy
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Methods of Heat TransferConvectionbullthe process of transferring heat by a circulating path of fluid particles ndash called a convection current
bullHot fluid spreads out and moves upwards cooler fluid takes its place creating a current
Methods of Heat TransferRadiationbullEnergy transfer by electromagnetic waves ndash no particles are necessary
bullie visible radio micro UV infrared X-rays
Calculating HeatbullWe use Specific Heat Capacity (c) Unit J(kg oC)
bullA measure of the amount of energy needed to raise the temperature of 10kg of a substance by 10oC
bullDifferent for every substancecwater ndash 418 x 103 J(kg oC)
Calculating Heat
Q = mcΔtbullQ = heat (J)bullm = mass (kg)bullc ndash specific heat capacity J(kg oC)
bullΔt ndash change in temp ndash Δt = tf - ti
Ex 1 What is the mass of a bucket of water that requires 84 x 104 J of heat to increase its temperature from 12oC to 22oC
Ans m = 20 kg
Latent Heat
What has more energyWater at 10oC or water at 50oC
Cooler particles move slower (less kinetic energy)
Hotter particles move faster (more kinetic energy)
What has more energyIce at 0oC or water at 0oC
Solid ndash Highly structured particles are trapped little motion
Liquid ndash Less structured particles can move more motion
Liquids are higher energy
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Methods of Heat TransferRadiationbullEnergy transfer by electromagnetic waves ndash no particles are necessary
bullie visible radio micro UV infrared X-rays
Calculating HeatbullWe use Specific Heat Capacity (c) Unit J(kg oC)
bullA measure of the amount of energy needed to raise the temperature of 10kg of a substance by 10oC
bullDifferent for every substancecwater ndash 418 x 103 J(kg oC)
Calculating Heat
Q = mcΔtbullQ = heat (J)bullm = mass (kg)bullc ndash specific heat capacity J(kg oC)
bullΔt ndash change in temp ndash Δt = tf - ti
Ex 1 What is the mass of a bucket of water that requires 84 x 104 J of heat to increase its temperature from 12oC to 22oC
Ans m = 20 kg
Latent Heat
What has more energyWater at 10oC or water at 50oC
Cooler particles move slower (less kinetic energy)
Hotter particles move faster (more kinetic energy)
What has more energyIce at 0oC or water at 0oC
Solid ndash Highly structured particles are trapped little motion
Liquid ndash Less structured particles can move more motion
Liquids are higher energy
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Calculating HeatbullWe use Specific Heat Capacity (c) Unit J(kg oC)
bullA measure of the amount of energy needed to raise the temperature of 10kg of a substance by 10oC
bullDifferent for every substancecwater ndash 418 x 103 J(kg oC)
Calculating Heat
Q = mcΔtbullQ = heat (J)bullm = mass (kg)bullc ndash specific heat capacity J(kg oC)
bullΔt ndash change in temp ndash Δt = tf - ti
Ex 1 What is the mass of a bucket of water that requires 84 x 104 J of heat to increase its temperature from 12oC to 22oC
Ans m = 20 kg
Latent Heat
What has more energyWater at 10oC or water at 50oC
Cooler particles move slower (less kinetic energy)
Hotter particles move faster (more kinetic energy)
What has more energyIce at 0oC or water at 0oC
Solid ndash Highly structured particles are trapped little motion
Liquid ndash Less structured particles can move more motion
Liquids are higher energy
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Calculating Heat
Q = mcΔtbullQ = heat (J)bullm = mass (kg)bullc ndash specific heat capacity J(kg oC)
bullΔt ndash change in temp ndash Δt = tf - ti
Ex 1 What is the mass of a bucket of water that requires 84 x 104 J of heat to increase its temperature from 12oC to 22oC
Ans m = 20 kg
Latent Heat
What has more energyWater at 10oC or water at 50oC
Cooler particles move slower (less kinetic energy)
Hotter particles move faster (more kinetic energy)
What has more energyIce at 0oC or water at 0oC
Solid ndash Highly structured particles are trapped little motion
Liquid ndash Less structured particles can move more motion
Liquids are higher energy
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Ex 1 What is the mass of a bucket of water that requires 84 x 104 J of heat to increase its temperature from 12oC to 22oC
Ans m = 20 kg
Latent Heat
What has more energyWater at 10oC or water at 50oC
Cooler particles move slower (less kinetic energy)
Hotter particles move faster (more kinetic energy)
What has more energyIce at 0oC or water at 0oC
Solid ndash Highly structured particles are trapped little motion
Liquid ndash Less structured particles can move more motion
Liquids are higher energy
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Latent Heat
What has more energyWater at 10oC or water at 50oC
Cooler particles move slower (less kinetic energy)
Hotter particles move faster (more kinetic energy)
What has more energyIce at 0oC or water at 0oC
Solid ndash Highly structured particles are trapped little motion
Liquid ndash Less structured particles can move more motion
Liquids are higher energy
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
What has more energyWater at 10oC or water at 50oC
Cooler particles move slower (less kinetic energy)
Hotter particles move faster (more kinetic energy)
What has more energyIce at 0oC or water at 0oC
Solid ndash Highly structured particles are trapped little motion
Liquid ndash Less structured particles can move more motion
Liquids are higher energy
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
What has more energyIce at 0oC or water at 0oC
Solid ndash Highly structured particles are trapped little motion
Liquid ndash Less structured particles can move more motion
Liquids are higher energy
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Latent Heatbullthe energy released or absorbed during a change in state
bullldquolatentrdquo means ldquohiddenrdquo ndash the energy is hidden in the bonds between molecules
bullthere is no temperature change during a change in state
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Specific Latent Heat ndash the heat required for a particular mass of substance to change state
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Q = mlQ = heat energy (Jkg)m = mass (kg)l = specific latent heat (J)
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Specific Heat of Fusionbullthe quantity of heat required to meltfreeze 1kg of a substance without changing the temperature
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Specific Heat of Vaporizationbullthe quantity of heat required to vaporizecondense 1kg of a substance without changing the temperature
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Using the latent heat values from your sheetHow much energy is required to turn 290g of solid oxygen at -219oC into liquid oxygen at -219oC
Ans Q = 403J
How much energy is required to turn a 50g 0oC ice cube into 0oC water
Ans Q = 17x104J
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Consider an ice cube meltingbullBelow 0oC the ice is solid heat energy
from the surroundings increases the temperature of the ice
bullAs the ice melts the heat energy is used to break the forces of attraction that hold the ice in a solid crystal lattice (no temperature change)
bullOnce the ice is melted the heat energy from the surroundings can be used to increase the temperature of the water
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
0C Ice Add Latent Heat 0 C Water
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Consider an ice cube meltingbullAs the water reaches 100oC the heat energy will stop raising the temperature and be used to break the forces of attraction in order to turn the liquid into a gas
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
0C Ice Add Latent Heat 0 C Water
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Applications of the Latent Heat of WaterWater has one of the largest specific latent heats
of fusion (melting) of all substances 333kJkgbullthis means that 333 kJ of heat must be
absorbed to melt 1kg of icebullthis makes ice a good refrigerant in coolers When water freezes it releases energy into the
surroundings (333kJ for every kg)bullfarmers use this to protect their crops from
frost they water the plants and as the water freezes it gives 333kJkg worth of heat E to the plant to warm it up
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Applications of the Latent Heat of Water
A burn from steam is worse than a burn from boiling water
bullwhen water condense on a persons skin 2268 J of energy is transferred to the skin
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Sample ProblembullHow much energy is required to turn 60 g
of -15oC ice into 50oC water
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Principle of Heat Exchange
When heat is transferred from one body to another the amount of heat lost by the hot body equals the amount of heat gained by the cool body
Qlost + Qgained = 0 OR
m1c1Δt1 (heat lost) + m2c2Δt2 (heat gained) = 0
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Principle of Heat Exchange
bullWhen heat is transferred from one object to another it usually flows from the hotter object to the cooler one
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
A gunsmith is making homemade bullets of melted lead After he creates the 23kg bullet it has a temperature of 1680oC He submerges it into 25kg of 20oC water to cool it down and let it harden What is the final temperature of both the lead and the water
Ans Tf =26oCHeat Transfer
cwater ndash 418 x 103 J(kg oC) clead ndash 160 x 102 J(kg oC)
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Solution
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
More on latent heat
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
Graph of Temperature vs Heat absorbed to melt an ice cube
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-
bullA Heat is absorbed by the surroundings to raise the temp of the ice
bullB Temperature doesnt change ndash energy is used to break forces of attraction within the solid to turn it into a liquid
bullC Heat is absorbed by the surroundings to raise the temp of the water
bullD Temperature doesnt change ndash energy is used to break forces of attraction within the liquid to turn it into a gas
bullE Heat is absorbed by the surroundings to raise the temperature of the gas
- Thermal Energy and Heat
- Temperature
- Thermal Energy (Q)
- Heat
- Methods of Heat Transfer
- Methods of Heat Transfer (2)
- Methods of Heat Transfer (3)
- Calculating Heat
- Calculating Heat (2)
- Slide 10
- Latent Heat
- What has more energy
- What has more energy (2)
- Latent Heat
- Slide 15
- Slide 16
- Specific Heat of Fusion
- Specific Heat of Vaporization
- Using the latent heat values from your sheet
- Consider an ice cube melting
- Slide 21
- Consider an ice cube melting (2)
- Slide 23
- Applications of the Latent Heat of Water
- Applications of the Latent Heat of Water (2)
- Sample Problem
- Principle of Heat Exchange
- Principle of Heat Exchange (2)
- Slide 29
- Solution
- More on latent heat
- Graph of Temperature vs Heat absorbed to melt an ice cube
- Slide 33
-