esci 215 chapter 5. in 1714 a german-dutch scientist named gabriel fahrenheit developed the first...
TRANSCRIPT
In 1714 a German-Dutch scientist named Gabriel Fahrenheit developed the first scale to be used frequently◦ Scale included: boiling, freezing, and zero points◦ He selected an arbitrary “zero” point (32°F) so
that winter temperatures would still read as positive values
◦ He selected the boiling point to be represented by 212°F, which was 180 degrees above the boiling point
Historical Background: Fahrenheit Scale
In 1742, Anders Celsius, a Swedish astronomer invented the Celsius scale
Temperature scale with:◦ Freezing point of water is the zero point (0°C)
100 degrees between the freezing and boiling points
Works well with decimal systems, so was easy for scientists to use
Historical Background:Centigrade (or Celsius) Scale
Lord Kelvin of England developed this scale Absolute zero = the lowest possible
temperature (0K) There are 273 degrees between absolute
zero and the freezing point (273K) There are 100 degrees between the freezing
and boiling points (373K) Using 0K to represent absolute zero meant
that no temperature could go below “zero” using this scale
Historical background:Kelvin Scale
Heat and temperature are different◦ Temperature scales measure temperature (not
heat)◦ Event 5-A shows the difference between
temperature and heat The nail and bolt have the same temperature, but
the bolt has more temperature See diagram page 72
Temperature – how hot or cold something; measured in degrees (F, C, K)
Heat – a quantity of energy something has
Heat and Temperature
Measuring Heat and Temperature Heat
◦ The energy a substance has due to motion of its molecules Increased heat = increased molecular motion Decreased heat = decreased molecular motion
◦ Absolute zero = the point where all molecular motion stops and a substance has no heat Scientists have never been able to get a substance
to this point Heat is measured in calories, British thermal
units (Btu), or joules
Calorie – amount of heat needed to raise the temperature of 1 gram of water by 1 degree Celsius◦ Common measurement
Btu – heat needed to raise 1 pound of water by 1 degree Fahrenheit◦ Used sometimes (i.e. furnace)
Joule –work done by 1 newton of force or weight moving a body through 1 meter◦ Used by scientists
Calories, Btu, Joules
1 gram of ice at 0°C or 1 gram of water at 0°C◦ Water
1 gram of water at 100°C or 1 gram of steam at 100°C◦ Steam
Why?◦ When matter changes from a state of slower
molecular movement to a state of higher molecular movement, heat is required
Change from solid to liquid requires heat Heat is needed to melt ice or to change water to
steam Heat of fusion and heat of vaporization are needed
Which Contains More Heat?
1 calorie of heat increases temperature of 1 gram of ice by 1 degree
If ice is -10C:◦ How many calories are needed to get to 0C?
10 calories melting point - but more heat is needed to change state
Heat of Fusion - change of state from solid to liquid takes 80 calories
How many calories are needed to get to 100C? 100 calories Vaporization point – but more heat is needed to change
state Heat of Vaporization – change of state from liquid to gas
takes 540 calories
Heat of Fusion and Vaporization
Where does the heat come from to change the state of matter?◦ It can come from anywhere
Air Your body Stove Hot plate
◦ When you hold an ice cube, heat is taken from your hand and used to melt the ice – leaving your hand feeling cold
◦ When you step out of a shower, heat is taken from your body and used to turn water into steam – leaving you feeling cool
Heat of Fusion and Vaporization
Event 5-B shows that there is no temperature change unless there is a change in the amount of heat present
Event 5-C demonstrates that heat of fusion is what causes the ice to melt by taking heat from the salt and using it to melt the ice◦ This causes the temperature of the salt water to
drop below freezing◦ This cooled water evaporates and forms frost on
the beaker
Heat of Fusion and Vaporization
There are many sources of heat Grouped into 4 categories:
Sources of Heat
Mechanical Chemical Electrical Nuclear
Friction Rearranging molecules
Lights Sun and stars
Bending Flame Toasters Atomic fission
Hammering Water and plaster
Heaters Atomic fusion
Pressure Sulfuric acid and sugar
Stoves Nuclear power reactor
Table 5.2 page 77 of text
Event 5-D Shake heat into a Bottle◦ Demonstrates a mechanical source of heat◦ Sand hits top and bottom of bottle and this friction
causes heat◦ Insulation around bottle is to make sure that the
heat is not coming from your hands Event 5-E Wire Heater
◦ Demonstrates a mechanical source of heat◦ Bending the wire causes heat to build at the bend
Some nails have adhesive on the shaft. This adhesive does not do anything at room temperature, but it melts when nailed into wood. Why?
Sources of Heat
Conduction Convection Radiation
Definition Transfer of heat from one molecule to another
Transfer of heat by movement of fluids
Transfer of energy by waves through space
Examples Silver spoonClothesIronCookware
Winds (weather)Chimney draftBoiling water
Sun’s heatHeat lampElectric heater
Heat Travels in 3 Ways:
Table 5.3 page 79 in text
Transfer of heat from 1 molecule to another Event 5-G Ice Preservation Race
◦ Purpose – learn about movement of heat by conduction Could be used after learning about conduction to show their
understanding of the concept Could be used before learning about conduction to have them
explore ways to slow heat transfer◦ 2 important rules:
No refrigerators, ice, or outdoors Do not let ice touch anything that will soak up water – water
needs to be measured to find the winner
◦ Best results achieved when: Size of container is small – reduces the area to be protected
from heat Conductivity is decreased – tin conducts heat well so need to
insulate the ice cube from the tin
Conduction
Good conductors◦ Metals are usually the best conductors of heat
(especially copper, silver, aluminum) Poor conductors
◦ Called insulators◦ Glass, paper, wood, plastic rubber
Event 5-H Two toned paper shows the effects of good and poor conductors◦ Wood is a poor conductor of heat so the paper scorches
more than copper which conducts the heat away Event 5-I Candle Snuffer shows a good conductor
◦ The candle goes out because the copper carries the heat away from the candle, not because of oxygen loss
Conduction
Transfer of heat by movement of fluids (gas or liquid)
Convection current - Liquids expand and become lighter when heated
Event 5-J The Mixed-Up Bottles shows a convection current ◦ Hot water is less dense and rises◦ Cold water is denser and sinks
Event 5-K The Circling Sawdust shows the movement of water
Convection
Figure 3.7 page 80 in text
Event 5-L Does Air Move In or Out shows the convection currents in air◦ One window is open on the bottom and another is
open at the top to show the air movement in the room Cold air enters the room through the lower opening
and hot air leaves the room through the higher opening
Event 5-M Convection Tester #1 shows that air rises when heated◦ Air is heated by the bulb and rises, causing the
coil to spin (see figure 5.9 on page 81)
Convection
Energy travels, at the speed of sound, from a source to an object; it travels through space◦ Ex: heat from the sun
This energy is only converted to heat when it hits a non-transparent object◦ On a cold day the sun’s light heats up a window sill,
but the window’s glass is still cold Substances vary in their ability to reflect and
absorb radiation◦ Event 5-N Which is the “warmer” colour? and Event 5-
O Hot Car show that black absorbs heat well and white reflects most of the heat energy that hits it
Radiation
All objects whose temperature is above absolute zero radiate (give off) some heat◦ The temperature must be very hot before we can feel
it Event 5-P Heat from Light shows the radiation
that a light bulb gives off◦ The heat below the light bulb is from radiation◦ The heat above the light bulb is from radiation and
convection If you had a fire in a fireplace, where would
you feel the radiant heat? Where would you feel the convection heat?
Radiation
Almost all substances expand when heated and contract when cooled◦ Index of expansion - the amount of expansion
or contraction ◦ When heated, molecules vibrate more and take
up more space Water is an exception
◦ It expands and contracts like other substances only when it is above 4°C
◦ Below 4°C it expands when cooled◦ This allows ice to form on top of water instead of
at the bottom
Expansion and Contraction
Interesting facts:◦ Sears Tower in Chicago is about 15 centimeters
taller on a hot summer day than on a cold winter day
◦ A 2km bridge can expand and contract about 1m between summer and winter
◦ Concrete highways and sidewalks have separation or joints to allow them to expand and contract without breaking
Expansion and Contraction
Event 5-Q Dancing Dimes shows how air expands when heated, rises up and pushes past the coin◦ When will the coin stop “dancing”?
When the air inside the bottle reaches room temperature
Note: the coin must have an airtight seal – wet the rim on the bottle with water
Event 5-R Jumping Juice (see safety note)◦ Hot water on outside of beaker causes the
coloured water to rise in the tube. Why?◦ Cold water on the outside of beaker causes the
coloured water to drop in the tube. Why?
Expansion and Contraction
Event 5-S The Sagging Solid shows that different metals have different expansion rates◦ Metal strip is bimetal (iron side and brass side)◦ The metal that expands more will be on the
outside of the curve◦ Which metal expands more?
Similar to 2 humans running a track. The outer lane is longer, so the runner has to run farther and faster to keep up with the runner in the inner lane
Expansion and Contraction
Event 5-T Expansion Meter shows how heat causes metal to expand◦ What happens to the weight as the wire is
heated?
Expansion and Contraction
Fig 5.12 page 85 in text
See Safety
Caution
Event 5-U Expansion of Gases shows how much air expands when heated◦ Air expands as it heats, rises and travels along
the tube and into the inverted bottle
Expansion and Contraction
Fig 5.13 page 86 in text
Fire is a chemical source of energy It releases energy by rearranging the atoms
of the object that is burning◦ A candle is a hydrocarbon – made of hydrogen (H)
and carbon (C) atoms◦ When it burns, oxygen (O) is bonded with the
hydrogen and carbon atoms◦ Carbon dioxide (CO2) and water (H2O) are produced◦ Event 5-V Water from Fire shows how fire
releases water Hydrogen atoms of candle combine with oxygen
atoms in air to produce water which condenses on the cold glass
Fire
Fire Triangle – the 3 things fire needs in order to burn:
1. Fuel2. Oxygen3. Kindling temperature – the temperature that
something will ignite at (different for different materials)
Fire will go out when 1 of these 3 things is missing
Fire is a form of rapid oxidation because it uses oxygen quickly
Fire
Event 5-W Boil Water in a Paper Cup shows how flame is extinguished when the kindling temperature is missing◦ The water in the paper cup takes the heat away
from the paper quickly, so the paper never reaches the kindling temperature
◦ The paper cup never burns, but the water boils
◦ Caution: Do not use plastic or Styrofoam cups. Why? Plastic will melt Styrofoam is a good insulator so water cannot take
the heat away fast enough and the styrofoam will burn, releasing fumes
Fire
Event 5-X Kindling Temperatures shows that different substances have different kindling temperatures◦ Some substances will ignite quickly at low
temperatures◦ Some substances will take more time and higher
temperature to ignite
◦ Caution: Do this in an area with lots of ventilation due to fumes and odours
Fire
When oxygen combines with other materials, it produces heat
Slow oxidation occurs when the heat is so little that you cannot detect it◦ When iron combines with oxygen to produce rust, it
produces heat that is not noticeable Event 5-Y Heat from Grass is a demonstration of
slow oxidation◦ Heat is produced in the moist grass as microorganisms
use the moisture to break down grass Moist grass breaks down in 1-2 days Dried hay (a type of grass) has no moisture, so can
be stored by farmers in a barn for years
Slow Oxidation