1. Specific Heat
Capacity

2. Temperature vs. Heat
• Temperature is the
measurement of the avg. KE
of the particles in matter.
• Heat energy that flows
from a warmer object to a
cooler object.

4. 4
A. When you touch ice, heat is transferred
from
1) your hand to the ice
2) the ice to your hand
B. When you drink a hot cup of coffee, heat
is transferred from
1) your mouth to the coffee
2) the coffee to your mouth
Learning Check

5. Have you ever noticed that on a
hot summer day the pool is
cooler than the hot cement?
OR maybe that the ocean is
cooler than the hot sand?

8. Specific Heat Capacity
1 calorie = 4.184 J
1,000 J = 1 KJ
4,184 J = 1 Kcal = 1 Calorie
Specific Heat: The amount of heat required to
raise the temperature of 1 gram of a substance
1 degree Celsius.

9. Substance Specific
Heat
J/(g°C)
Water 4.184
Ethanol 2.44
Aluminum 0.897
Granite 0.803
Iron 0.449

10. LecturePLUS Timberlake 99 10
Learning Check
A. A substance with a large specific heat
1) heats up quickly 2) heats up slowly
B. When ocean water cools, the surrounding air
1) cools 2) warms 3) stays the same
C. Sand in the desert is hot in the day, and cool
at night. Sand must have a
1) high specific heat 2) low specific heat

11. Equation:
q = c x m x ΔT
ΔT = Tfinal – Tinitial
q = the heat absorbed or released
c = the specific heat of the substance
m = the mass of the sample in grams
ΔT = change in temperature

13. 1.) Copper metal has a specific heat (Cp) of
0.385 J/g⁰C. Calculate the amount of heat (J)
required to raise the temperature of 22.8 g of
copper from 20.0⁰C to 875⁰C.

14. 2) What is the specific heat of a 25.0 g
substance that absorbs 493.4 J,
and raises the temperature from 12.0⁰C to
34⁰C?

15. 3) It takes 1,250 J of energy to heat a certain
sample of pure silver from 12.0 0C to 15.2 0C.
Calculate the mass of the sample of silver.