conceptual physics hewitt, 1999 bloom high school chapter 21 temperature, heat and expansion
TRANSCRIPT
21.1 Temperature
Temperature- a measure of how hot or cold something is Demonstrated by the expansion or contraction of a liquid
Red thermometer- colored alcohol Silver thermometer- mercury
Celsius scale- 100 degrees difference between freezing and boiling of pure water 0°C corresponds to the freezing point of pure water 100°C corresponds to the boiling point of pure water
Fahrenheit scale- 180 degrees difference between freezing and boiling of pure water 0°F corresponds to a mixture of ice, water, ammonium chloride and
salt 100°F corresponds to human body temperature
Kelvin
Kelvin- 100 degrees difference between freezing and boiling of pure water 273K corresponds to the freezing point of pure water 373K corresponds to the boiling point of pure water 0K (absolute zero) represents zero kinetic energy of a
substance
Fahrenheit is an English unitCelsius is not SI, but a derived unitKelvin is SI (metric)
We don’t use “degrees” with Kelvin
Temperature & Kinetic Energy
Temperature is related to the motion of molecules Proportional to the average kinetic
energy Not a measure of the total KE of the
molecules
Example: There is twice as much energy in 2L of 90°C H2O as 1L of 90°C H2O Even though the temperature is the
same, there is twice as much mass
21.2 Heat
Heat- the energy transfer that takes place because of the temperature difference between two objects Energy always flows from high to low Matter does not contain heat
Thermal energy- energy resulting from heat flow Chapter 8 Internal energy- term used in this
chapter for the same thingThermal contact- when heat flows
due to direct contact
21.3 Thermal Equilibrium
Thermal equilibrium- when objects in contact reach the same temperature No heat flows from one to the other any more
A thermometer is read at thermal equilibrium When the alcohol or mercury stops moving The glass of the thermometer is too small to affect the
temperature
21.4 Internal Energy
Internal energy- grand total of all of the energies in the substance Translational energy (moving in a straight line) Rotational energy of the molecule Kinetic energy within the molecule Potential energy due to forces within molecule
As a substance absorbs energy, the temperature increases
As a substance gives off energy, temperature decreases and one or more of the energies decrease
21.5 Measurement of Heat
Temperature- a measure of heat transfer, not heat content
Calorie (cal)- amount of heat required to increase 1g of H2O by 1°C Metric, derived unit of heat energy kilocalorie (kcal or Cal)- 1000
calories Found on food wrappers
Joule (J)- 4.18J are required to increase 1g of H2O by 1°C Standard SI unit of heat energy
Hungry Man Classic Fried Chicken Dinner
21.6 Specific Heat Capacity
Specific heat capacity (or just specific heat)- the quantity of heat required to raise the temperature of 1g by 1°C Ability to store internal energy
A measured value for each substance (see table)
Using Specific Heat (chemistry review)
Label Symbol Unit
Specific Heat c cal/(g°C) or J/(g°C)
Heat Q cal or J
Mass m g
Change in temp.
DT °C
q=mcDT cal=(g)(cal/(g°C))(°C)J=(g)(J/(g°C))(°C)
21.7 The High Specific Heat Capacity of H2O
Absorbs more than would be expectedSlow to gain heatSlow to lose heatAir near water areas are cooler than far inland
because water resists a change in temperature
21.8 Thermal Expansion
As temperature increases, kinetic energy of the molecules increase and they “wiggle” further apart
Gases expand the most when heated Liquids expand less than gases Solids expand less than liquids
Your Thermostat & You
Bimetallic strip- a strip made of two metals that expand at different rates Brass & iron, typically One side expands at a different rate than the other
Thermostat- practical application of bimetallic strip to turn on and off your furnace/AC In the diagram, closing the circuit (touching) turns the
furnace on
21.9 Expansion of Water
All liquids expand when heated
Ice cold (0°C) H2O does the opposite!
As H2O warms from 0°C to 4°C, it contracts H2O is more dense at 4°C
than 0°C, therefore sinks to the bottom of the container
Solid versus Liquid H2O
In liquid H2O, some of the O’s are attracted to the H’s H2O molecules are able to slide past
each other with minimal interaction
In solid H2O, each O is attracted to two H’s This causes large, fixed gaps, which
decreases density Ice floats because of this decreased
density Lakes/ponds freeze from the top
down