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# Specific Heat (Grades 11-12)

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## Specific Heat

1.
According to Joule's Law, the internal energy of a gas is a function of the                      energy of its molecules.
2.
When working gas law problems, all temperatures must be converted to the
1. Celsius scale.
2. Fahrenheit scale.
3. Boyle scale.
4. Kelvin scale.
3.
What is the term used for the amount of heat per unit mass required to raise the temperature of a substance by one degree Celsius?
1. temperature capacity
2. latent heat
3. specific heat
4. relative heat
4.
What is the formulaic relationship between Q, C, m and $Delta$T, where

Q is the amount of heat transferred to an object
C is the specific heat of that object
m is the mass of the object and
$Delta$T is the change in temperature?
1. Q = Cm$Delta$T
2. Q = Cm/$Delta$T
3. C = $Delta$T/mQ
4. C = Qm$Delta$T
5.
The SI unit for specific heat is 1                     .
6.
Which of these substances has the highest specific heat, requiring the most amount of heat energy to raise its temperature by $1degC$?
1. iron
2. wood
3. oil
4. water
7.
What is the specific heat of water?
1. 4.186 J/g•°C
2. 10 J/g•°C
3. 1 kcal/g•°C
4. 1 cal/kg•°C
8.
The specific heats of gases are generally expressed as molar specific heats because the number of moles is a more convenient measure of an amount of gas.
1. True
2. False
9.
A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron.

$C=Q/(m*DeltaT)$

10.
If 335 g of water at 65.5 °C loses 9750 J of heat, what is the final temperature of the water? Liquid water has a specific heat of 4.18 J/(g•°C).

$DeltaT=Q/(m*C)$

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