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Study Quiz Section 10.2
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1

How much heat would be required to warm 1000 kg of pure water from 5°C to 37°C?
A)134 080 kJ
B)7 637.2 kJ
C)134.1 kJ
D)32 000 kJ
2

What would be the temperature change of a mass of 15 g of pure water if 2.75 kJ of heat were applied?
A)183°C
B)172.8°C
C)43.76°C
D)0.043°C
3

The fact that water has a high specific heat capacity means that:
A)More heat is required to raise the temperature of 1 g of water than 1 g of many other substances.
B)Less heat is required to raise the temperature of 1 g of water than 1 g of many other substances.
C)Water absorbs heat slowly and releases it quickly.
D)Water absorbs heat quickly and releases it slowly.
4

The heat of vaporization of water is:
A)60.53 kJ/mol
B)40.65 kJ/mol
C)6.01 kJ/mol
D)4.19 kJ/mol
5

The term "heat of vaporization" refers to:
A)The amount of energy required to melt one mole of a substance.
B)The amount of energy released when one mole of a substance changes from a solid to a liquid.
C)The amount of energy released when one mole of a substance is changed from a solid to a gas.
D)The amount of energy required to convert one mole of a substance from a liquid to a gas.
6

If the heat of fusion of nitrogen is 0.71 J/mol and the heat of vaporization is 5.57 kJ/mol, calculate the energy required to completely melt 125.5 g? (The molar mass of Nitrogen is 28.02 g/mol)
A)156.1 kJ
B)24.95 kJ
C)19.89 J
D)3.18 J
7

Water is constantly changing state in the environment. One such change of state is frost forming on cold surfaces. This phase change is called:
A)Freezing
B)Sublimation
C)Condensation
D)Vaporization





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