1. Chapter 6: Thermal Energy
RECALL: Temperature is a measure of the average kinetic energy of the particles in the object.
As temperature increases, the average speed (and thus the average kinetic energy) of the particles increases.
Thermal energy is the sum of the kinetic energy and the potential energy of the particles in the object.
Note: potential energy is made up of chemical, electrical and nuclear potential energy and any other potential energy due to interactions between the particles.

2. 50 g 100 g Thermal energy, Temperature and Mass T = 25 °C T = 25 °C
More thermal E!
50 g
100 g
Q: Is the thermal energy of both beakers the same?
A: No. While both beakers have the same average kinetic energy (same T), there are more particles in the 100 g sample of water so it must have more thermal energy.

3. Heat: thermal energy that flows FROM a region of higher temperature TO a region of lower temperature.
As the temperature difference increases, the amount of heat transferred increases.
Hot
Cool
Very
Cold
HEAT
MORE
DT1
DT2
DT2
>
DT1
DT = difference in temperature

4. Specific Heat: The amount of heat needed to raise 1 kg of a substance by 1°C
Water is often used as a coolant because of its high specific heat.

5. Q: What will heat up faster, water or iron?
Iron: it has a lower specific heat
Q: What will stay hot longer, copper or silver?
Copper: it has a higher specific heat

6. Q = mCDT Calculating changes in thermal energy
Q = heat energy, units are Joules (J)
m = mass, units are kg
C = specific heat, units are J/(kg°C)
DT = change in temperature (Tf - Ti)
Q = mCDT
EX: A room containing 72 kg of air with a specific heat of 1010 J/kg°C is heated from 20°C to 25°C. How much thermal energy was used?
m = 72 kg
C = 1010 J/kg°C
DT = 25°C - 20°C = 5°C
Q = mCDT
= (72 kg)(1010 J/kg°C)(5°C)
= 363,600 J

7. Calorimetry: A technique used to measure the amount of heat transferred between substances.
Air
Water
Metal pieces
Thermometer
Stirrer
0.025 kg of metal is heated to 100°C and then put into 0.1 kg of water that is at 20°C.
The excess heat in the metal is transferred to the water warming it up to 23°C.
1. How much heat was transferred?
QH2O = mCDT
QH2O =(0.1 kg)(4184 J/kg°C)(3°C)
QH2O = 1255 J

8. 2. What is the specific heat of the 0.025 kg of metal?
If 1255 J of heat was gained by the water, that means that 1255 J of heat was lost by the metal (Conservation of Energy).
Qmetal = 1255 J
What is DT?
Metal started out at 100°C and ended up at the same temperature as the water, 23°C.
DT = 100°C - 23°C = 77°C
Substitute the values into Qmetal = mCDT and solve for C.
Qmetal = mCDT
1255 J = (0.025 kg) C (77°C)
1255 J = (1.93) C
C = 650 J/kg°C

9. Thermodynamics: describe the inter-relationship between heat, thermal energy and work.
First law of thermodynamics: The increase in thermal energy (DU) of a system is the sum of the work done on the system and the heat transferred to the system
DU = Q + W
In closed systems, heat cannot enter or leave the system.
DU = 0
In open systems, heat can be exchanged with the environment
DU  0

10. Second law of thermodynamics: It is impossible for heat to flow from a cool object to a warm object unless work is done on the system.
NO WORK = NO HEAT TRANSFER
HOT
COLD
HEAT

11. Section 2: Transferring Thermal Energy Heat
Conduction: heat is transferred through a material (glass, wood, metal etc.)
Rate of heat transfer depends upon the material.
Metals: FAST, good conductors
Gases: SLOW, good insulators

12. Convection: transfer of thermal energy in liquids and gases by movement of warmer and cooler regions from place to place.
The warm water is less dense than the cooler water around it so it rises.
The warm water cools (through conduction) as it rises.
The cooled water sinks back to the bottom.

13. Radiation: transfer of energy by electromagnetic radiation
Radiation: transfer of energy by electromagnetic radiation. No matter is needed for transfer to occur.
When solar radiation strikes a light colored object, most of the radiation is reflected. The small amount that is absorbed causes a small temperature increase.
When solar radiation strikes a dark colored object, most of the radiation is absorbed. This causes a larger temperature increase.
Because the molecules are far apart, gases do not absorb much solar radiation.

14. Heating systems
Forced-Air
Steam/hot water Radiators
Electric Heating

15. Passive Solar Heating
Limitations for both types:
Doesn’t work at night
Doesn’t work well on cloudy days
Active Solar Heating

16. Heat Engine: a device that converts heat into work
Example: An internal combustion engine
Chemical energy of gasoline is converted into heat, which causes gases to expand and push (a force) against the piston heads. When the pistons move under the force of the expanding gases, work is being done.
Only about 25% of the heat generated by the engine is converted into work. The rest is transferred out to the surroundings.
Q: Is an internal combustion engine a closed or open system?
A: Heat is transferred to the surroundings, so it is an OPEN system.

17. Heat movers: do work in order to move heat from a COLD area to a WARMER area.
Example: A refrigerator
Electrical energy is used to compress the coolant into a liquid.
The liquid coolant absorbs some of the the thermal energy from the inside of the refrigerator so it can expand into a gas. This causes the inside of the refrigerator to cool. B A
Air conditioners and heat pumps are also heat movers.