1. Physics Unit 5: Heat and Temperature

2. Chapter 13
Bellringer
We use words like hot and cold, long and short, and heavy and light every day to describe the differences between things. In science, however, this is often not accurate enough and leads to confusion.
In drawing 1, which bowl would feel warm to your hands? Which bowl would feel cool?

3. Bellringer, continued Chapter 13
In drawing 2, which bowl would feel warm to your hands? Which would feel cool?
3. A person from Seattle tells his friend from Florida that the weather in Seattle is somewhat warm. When the friend arrives for a visit, he finds that he is uncomfortably cool wearing the shorts he packed. What would be a more effective way for the person from Seattle to explain the weather?

4. Temperature What does temperature indicate?
Measurement of the average Kinetic Energy of the molecules
NOT A MEASURE OF HEAT

5. Measuring Temperature
We use a Thermometer to measure temperature
Thermometers rely on expansion
Most objects expand when their temperature increases
Alcohol or Mercury Thermometers use expansion and contraction to measure temperature.

6. Digital thermometers use electrical current to measure temperature.
The warmer a liquid is, the more the particles move and thus the liquid expands (takes up more space) and rises up through the tube
Liquid thermometers can only be used between certain temperatures, why?
Because the liquid will freeze at low temps
Because the liquid will boil at high temps
So, some thermometers use a solid metal to measure temperature through expansion
Like a metal coil used in refrigerators
Digital thermometers use electrical current to measure temperature.

7. Temperature Scales There are three temperature scales
1) Fahrenheit Scale: water boils at 212 oF and freezes at 32 oF, normal body temp is 98.6 oF.
2) Celsius Scale or Centigrade: like the metric system, it is bases on powers of 10.
- water boils at 100 oC and freezes at 0 oC.
3) Kelvin Scale (Science): water boils at 373 K and freezes at 273 K. (no degree symbol)
- absolute zero (0 K): motion stops…the lowest possible temperature you can go. (-273 oC)
The size of each temperature unit or degree for the Celsius and Kelvin unit is the same. The difference between the boiling point and freezing point for both is 100.
The size of the Fahrenheit degree is smaller that the Celsius degree. The diff between the boiling point and the freezing point ( ) is 180 degrees, not 100 like Celsius or Kelvin.
The zero points are all different on all three scales.

8. Since the Celsius and Fahrenheit Scales can go below their zero mark, they have negative values.
This is why they are reported in degrees
Since KELVIN starts at zero, and cannot go below that absolute zero, then you cannot have negative Kelvin
This is why Kelvin is not reported in degrees
Kelvin is always positive

9. Converting Temperature
Celsius to Kelvin: tK = t oC
Ex: 23 oC to K
Kelvin to Celsius: t oC = tK
Ex: 338 K to oC
Celsius to Fahrenheit: t oF = 1.8 (t oC) + 32
Ex: 33.5 oC to oF
Fahrenheit to Celsius: t oC = (t oF – 32) Ex: 147 oF to oC
The size of each temperature unit or degree for the Celsius and Kelvin unit is the same. The difference between the boiling point and freezing point for both is 100.
The size of the Fahrenheit degree is smaller that the Celsius degree. The diff between the boiling point and the freezing point ( ) is 180 degrees, not 100 like Celsius or Kelvin.
The zero points are all different on all three scales.

10. Chapter 13
Bellringer
Why is it a bad idea to drink hot cocoa out of a tin cup? Explain the energy transfers on the atomic level.

11. Bellringer, continued Chapter 13
2. What happens to your hand when you place it above a lighted candle? (Assume you are not touching the flame. Explain the energy transfers on the atomic level. Hint: Remember that warm air rises.)
3. When you sit near a fire, you can feel its warmth on your skin, even if you are in cool air. Does this sensation depend upon the fact that warm air rises?

12. Temperature and Energy Transfer
When you hold an ice cube, the ice melts because of the energy transfer.
The particles of your hand are moving faster than those of the ice cube
The particles of your hand collide with the particles of the ice cube and cause the particles of the ice cube to move faster
When the ice cube particles move faster (higher kinetic energy) from this collision, the temperature of the ice cube rises and thus it melts.

13. This happens until equilibrium is reached!
The energy transfer between particles of two objects due to a temperature difference between the two objects is called heat.
The transfer of heat ALWAYS goes from higher temperature (faster moving) to lower temperature (slower moving)
This happens until equilibrium is reached!
A seat may feel cool at first, but your body will warm it up until they reach the same temperature (equal temp equilibrium)
Heat gained = heat lost
Law of conservation of energy

14. Methods of Energy Transfer
Conduction: involves objects in direct contact
Fast moving molecule will collide with slow moving molecule, transferring energy
Works for all 3 phases of matter
But gases are very poor conductors because the particles are so far apart
Liquids are okay
Solids are best insulators, but vary by substance
Heat Conductor: Substance that moves heat more effectively (like metal skillets used to cook)
Insulator: Substance that will not conduct heat well (like fiber glass insulation, wood on skillet handle)

15. Conductors and Insulators
Chapter 13
Conductors and Insulators
Any material through which energy can be easily transferred as heat is called a conductor.
Poor conductors are called insulators.
Gases are extremely poor conductors.
Liquids are also poor conductors.
Some solids, such as rubber and wood, are good insulators.
Most metals are good conductors.

16. Methods of Energy Transfer, continued
Chapter 13
Methods of Energy Transfer, continued
Thermal Conduction
Conduction involves objects in direct contact.
Conduction takes place when two objects that are in contact are at unequal temperatures.

17. 2. Convection: movement of warm fluids
The fluid (air) transfers the heat
Molecules move in currents
Only in a fluid: (Liquid or Gas)
Heated portion speeds up and becomes less dense, creating a current of heat
Air currents are a result of convection

18. Methods of Energy Transfer, continued
Chapter 13
Methods of Energy Transfer, continued
Convection
Convection results from the movement of warm fluids.
During convection, energy is carried away by a heated fluid that expands and rises above cooler, denser fluids.
A convection current is the vertical movement of air currents due to temperature variations.

19. 3. Radiation: does not require direct contact
Heat is transferred through space
Does not involve the movement of matter
Travels as waves
Electromagnetic radiation (Gamma, UV, Visible, X-rays, Microwaves, Radio, Infrared,)

20. Measuring Heat calories (cal) or joules (j) are used to measure heat
calorie: Amount of heat needed to raise the temperature of one gram of liquid one degree Celsius
Since heat is related to kinetic energy, the unit of joules is often used
1 cal = 4.2 joules
Convert 350 cal to kJ

21. What Are Food Calories? Calories are really kilocalories
2000 Cal diet is really 2,000,000 calories
We use capital C (kilo) because it is easier

22. Specific Heat (s) :
Specific Heat (s) : amount of energy required to change the temperature of one gram of a substance 1 oC
How well a substance conducts heat
Varies from one substance to another
Heat always travels from high concentration to low concentration!!
Heat lost = Heat gained

23. Water has a specific heat = 1 cal/goC or 4.184 J/goC
Water has the second highest specific heat capacity of all known substances. So it requires high amounts of heat energy to raise water temperature.
water also has a high energy/heat requirement for evaporation
SIRON = J/goC
Which would heat up faster, 5.00 grams of iron or 5.00 grams of water?
  Which would cool down faster, 5.00 grams of iron or 5.00 grams of water?
 Which is a better thermal conductor?
 Which is a better insulator?

24. Q = s x m x DT Q = energy (heat) required (J) or (cal)
s = specific heat capacity (J/goC) or (cal/goC)
m = mass of the sample in grams
DT = change in temperature in oC
A 2.8 g sample of a pure metal requires 10.1 J of energy to change its temperature from 21 oC to 36 oC. What is the specific heat of the metal?
s = Q = J = J/goC m x DT (2.8 g x 15oC)

25. Chapter 13
Bellringer
One extremely cold winter day, the thermostat in the science classroom was set too low and the room was cold. The science teacher did not have the right tool to reset the thermostat, so she made a thin cloth cover for the thermostat, wet it, and placed it over the thermostat. Soon the room was comfortably warm.
You have learned that there is an energy change when a liquid evaporates. Will the area near the liquid get hotter or cooler as evaporation occurs? (Hint: Compare and contrast the molecular motion of particles as liquids and as gases.)

26. Bellringer, continued
Imagine a different situation in the same class, during the week before summer vacation. This time, it is very hot outside, but the thermostat is set so high that the air conditioner does not come on. Which of the following might help the thermostat trigger the air conditioner more frequently?
a. use another wet cloth on the thermostat
b. point a fan at the thermostat
c. wrap the thermostat in a dark cloth that has been sitting by the windowsill
d. wrap the thermostat in a dark cloth that has been kept in the refrigerator
e. redirect air from the air conditioner vent away from the thermostat

27. Applications Heating Systems:
Work can increase ave kinetic energy, like when lighting a fire by using the friction of two sticks
Our bodies act like a heating system to regulate our body temp to stay at 37 oC or 98.6 oF, we burn stored calories and nutrients to provide the energy we need to raise our temp in the cold.
The sun can be used to heat a system
by cold-blooded animals to help maintain their temp

28. Chapter 13
Heating Systems
Most heating systems use a source of energy to raise the temperature of a substance such as air or water.
The human body is a heating system. Some of the energy from food is transferred as heat to blood moving throughout the human body to maintain a temperature of about 37°C (98.6°F).
In central heating systems, heated water or air transfers energy as heat.
Solar heating systems also use warmed air or water.

29. Heating Systems, continued
Chapter 13
Heating Systems, continued
In the solar system shown here, a solar collector uses panels to gather energy radiated by the sun.
This energy is used to heat water that is then moved throughout the house.
This is an active solar heating system because it uses energy from another source, such as electricity, to move the heated water.

30. Heating Systems, continued
Chapter 13
Heating Systems, continued
In a passive solar heating system, energy transfer is accomplished by radiation and convection.
In this example, energy from sunlight is absorbed in a rooftop panel.
Pipes carry the hot fluid that exchanges heat energy with the air in each room.

31. Heating Systems, continued
Chapter 13
Heating Systems, continued
When energy can be easily transformed and transferred to accomplish a task, such as heating a room, we say that the energy is in a usable form.
After this transfer, the same amount of energy is present, according to the law of conservation of energy. Yet less of it is in a form that can be used.
In general, the amount of usable energy always decreases whenever energy is transferred or transformed.
Insulation minimizes undesirable energy transfers.

32. Cooling systems:
Liquids can be evaporated or condensed to allow for transfer of energy in either direction so as to cool or heat a system.
Evaporation causes a cooling effect because gases are farther apart and thus cannot transfer energy as well through physical contact. Also particles gain energy as they evaporate, removing it from surroundings.

33. Air Conditioner Chapter 13
One example is an air conditioner. An air conditioner does work to remove energy as heat from the warm air inside a room and then transfers the energy to the warmer air outside the room.

34. Cooling Systems Chapter 13
In all cooling systems, energy is transferred as heat from one substance to another, leaving the first substance with less energy and thus a lower temperature.
A refrigerant is a material used to cool an area or an object to a temperature that is lower than the temperature of the environment. During each operating cycle, the refrigerant evaporates into a gas and then condenses back into a liquid.

35. Heat Engines
A heat engine is a machine that transforms heat into mechanical energy, or work.
Internal combustion engines burn fuel inside the engine.
An automobile engine is a four-stroke engine, because four strokes take place for each cycle of the piston.
The four strokes are called intake, compression, power, and exhaust strokes.
Internal combustion engines vary in number of pistons.

36. Internal Combustion Engine