Name____________________________________Date________________Period____________
Heat & Its Measurements
Q = m Cp (ΔT)
ΔT = Tf - Ti
Use the above formulas to solve the problems below. SHOW YOUR WORK to get credit!!
1.) What must be the specific heat of a sample of an unknown material of 36.359g, when 59.912 J of heat
are applied raising the temperature 152.0°C?
Q=
m=
Cp=
ΔT=
2.) How many Joules are required to raise the temperature of a 29.352g sample of water by 52.0°C?
(Note the specific heat of water is 4.18J/g °C)
Q=
m=
Cp=
ΔT=
3.) How many Joules of heat are necessary to raise the temperature of 350ml of water from 1.00 °C to
5.00°C? (Cp of water is 4.18 J/g°C)
Q=
m=
Cp=
ΔT=
4.) Find the mass of a piece of copper when 8000.0 J of heat are applied, causing a 45 °C increase in
temperature. (Cp of copper is 0.385 J/g °C)
Q=
m=
Cp=
ΔT=
5.) Find the specific heat of an unknown metal with an initial temperature of 16.0 °C, when 3500 Joules
are applied to a 40.0g sample and the final temperature is 81.0 °C.
Q=
m=
Cp=
ΔT=
6.) A 250 g sample of water with an initial temperature of 98.8 °C loses 7500 joules of heat. What is the
final temperature of the water?
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m=
Cp=
ΔT=
7.) How much heat is lost when a 15.34 g piece of copper’s temperature drops from 90.0 °C to 81.0 °C?
Q=
m=
Cp=
ΔT=
8.) Copper has a specific heat of 0.385 J/g °C. How much change in temperature would the addition of 35
000 Joules of heat have on a 538.0 gram sample of copper?
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m=
Cp=
ΔT=
9.) 4786 Joules of heat are transferred to a 89.0 gram sample of an unknown material, with an initial
temperature of 23.0 °C. What is the specific heat of the material if the final temperature is 89.5 °C?
Q=
m=
Cp=
ΔT=
10.) 8750 J of heat is applied to a piece of aluminum, causing a 56 °C increase in its temperature. The
specific heat of aluminum is 0.902 J/g°C. What is the mass of the aluminum?
Q=
m=
Cp=
ΔT=
11.) The temperature of a 55 gram sample of a certain metal drops by 113 °C as it loses 3500 Joules of
heat. What is the specific heat of the metal?
Q=
m=
Cp=
ΔT=