1. [Final temp-Initial temp]
energy (J)
mass (g) Q
= m
s ∆T
temp. change (oC)
[Final temp-Initial temp]
specific
heat
(J/goC)

2. A werewolf hunter cools her newly handmade silver bullet from 952 oC to oC in a bucket of water. Calculate the energy change in kcal for the bullet if it has a mass of 35.2 grams.
Q = s ∙ m ∙ ∆T Q = (0.240 J/goC) (35.2g) (22oC - 952oC) Q = J
J x 1 cal x 1 kcal = kcal
4.184 J cal

3. A 2. 6 g sample of a metal requires 15
A 2.6 g sample of a metal requires 15.2 J of energy to change its temperature from 21oC to 34oC. Use the table to determine the identity of metal.
s = Q .
m∆T
s = J
(2.6g) (34oC - 21oC)
s = J/goC

4. A sample of gold loses 3.1 J of energy when it cools from 27 oC to 19oC. What is the mass of this sample of gold?
m = Q
s∆T
m = J
(0.129 J/goC ) (19oC - 27oC)
m = 3 g Au

5. If 294 J of heat is transferred to a 10
If 294 J of heat is transferred to a 10.0 g sample of silver at 25oC, what is the final temperature of the silver? (sAg = 0.24 J/goC)
∆T = Q . sm
Tfinal - 25oC = J
(0.24 J/goC ) (10.0g)
Tfinal = 150oC