1. Energy
EQ: What is the relationship between heat energy and temperature?

2. Eureka: Temperature

3. A. Definitions
1. Energy (light, heat, electric) The capacity to do work or supply heat.

4. A. Definitions
2. Law of conservation of energy: In any reaction, energy can be converted from one form to another, but cannot be created or destroyed.

5. A. Definitions 3. Heat (q) is the energy transferred
always flows from Hot  Cold
Measured in Joules or calories
4. Temperature (T) :measure of the avg. kinetic energy measured in Kelvin or degrees Celcius.

6. Thermal energy can be transferred from object to object through direct contact
Molecules collide, transferring energy from molecule to molecule

7. Thermal energy can be transferred from object to object through direct contact
Molecules collide, transferring energy from molecule to molecule

8. Thermal energy can be transferred from object to object through direct contact
Molecules collide, transferring energy from molecule to molecule

9. Thermal energy can be transferred from object to object through direct contact
Molecules collide, transferring energy from molecule to molecule

10. Thermal energy can be transferred from object to object through direct contact
Molecules collide, transferring energy from molecule to molecule

11. Thermal energy can be transferred from object to object through direct contact
Molecules collide, transferring energy from molecule to molecule

12. Thermal energy can be transferred from object to object through direct contact
Molecules collide, transferring energy from molecule to molecule

13. Thermal energy can be transferred from object to object through direct contact
Molecules collide, transferring energy from molecule to molecule

14. Thermal energy can be transferred from object to object through direct contact
Molecules collide, transferring energy from molecule to molecule

15. Thermal energy can be transferred from object to object through direct contact
Molecules collide, transferring energy from molecule to molecule

16. Thermal energy can be transferred from object to object through direct contact
Molecules collide, transferring energy from molecule to molecule
AKA: HEAT

17. Eureka: Temp Vs. Heat

18. B. Unit conversions 1 cal = 4.184 J 1Cal = 1000 cal
Convert 8.5 Joule to calories
= 2.0 cal
1 cal
8.5 J x
4.184 J

19. C. Specific Heat (C)
The amount of heat needed to raise the temperature of 1 gram of a substance by 1°C.
Objects with low specific heats, heat up faster than objects with high specific heats.
Which object heats up faster?
Water: j/gC
Pot: j/gC

20. ∆T= Tfinal- Tinitial q = m x c x DT A. Specific Heat specific heat
change in
temperature
Heat =
mass X X
q = m x c x DT
∆T= Tfinal- Tinitial

21. C for Fe = 0.444 J/g • 0C Given: q = ? Work: m = 869 g q=mcT
Ex: How much heat is given off when an 869 g iron bar cools from 940C to 50C?
C for Fe = J/g • 0C
Given:
q = ?
m = 869 g
c = J/goC
ΔT = tfinal – tinitial
= 50C – 940C
= -890C
Work:
q=mcT
q=869 g x J/g0C x –890C
q=-34,000 J

22. q_ c= ΔT =350C – 250C m∆T = 10.0C Given: Work: C= ? q=mcT  m= 25.0 g
Ex: Calculate the specific heat of an object with a mass of 25.0 g whose temperature changes from 250C to 350C when 16,500 J are added.
Given:
C= ?
m= 25.0 g
ΔT =350C – 250C
q = 16,500J
Work:
q=mcT 
C = _16,500 J
(25.0g) (10.0C)
C = 66 q_ c=
m∆T
= 10.0C
J/goC