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Chapter 6
1. Define kinetic energy, potential energy, chemical energy and state function(6.2, 6.3)
Energy that is associated with the relative positions of electrons and nuclei in atoms and
molecules is called
A) kinetic energy
B) thermal energy
C) potential energy
D) chemical energy
2. Describe the first law of thermodynamics and use it to model energy changes (6.3)
The law of ________ states that energy that can be neither created or destroyed.
A) kinetic energy
B) the consecration of energy
C) potential energy
D) the conservation of energy
E) thermochemistry
3. Relate internal energy to heat and work (6.4)
(1) Which of the following signs on q and w represent a system that is doing work on the
surroundings, as well as gaining heat from the surroundings?
A) q = +, w = ‒
B) q = ‒, w = +
C) q = +, w = +
D) q = ‒, w = ‒
E) None of these represent the system referenced above.
(2) For ΔEsys to always be -, what must be true?
A) q = w
B) +q > ‒w
C) +w > ‒q
D) ‒w > +q
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4. Given two of the three: work, pressure and change in volume, or a means to solve two
of the three, determine the value for the missing variable (6.4)
Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and is
changing from 12.00 L to 6.00 L in volume at 1.50 atm pressure. (Remember that 101.3 J = 1
L·atm)
A) +25.9 kJ
B) ‒16.0 kJ
C) ‒25.9 kJ
D) ‒24.1 kJ
E) 937 kJ
5. Given three of the four: energy, mass, specific heat and change in temperature, or a
means to solve three of the four, determine the value for the missing variable (6.4)
Determine the final temperature of a gold nugget (mass = 376 g) that starts at 398 K and loses
4.85 kJ of heat to a snowbank when it is lost. The specific heat capacity of gold is 0.128 J/g°C.
A) 133 K
B) 398 K
C) 187 K
D) 297 K
E) 377 K
6. Define the concept heat capacity and relate it to specific heat capacity and molar heat
capacity (6.4)
Which of the following (with specific heat capacity provided) would show the smallest
temperature change upon gaining 200.0 J of heat?
A) 50.0 g Al, CAl = 0.903 J/g°C
B) 50.0 g Cu, CCu = 0.385 J/g°C
C) 25.0 g granite, Cgranite = 0.79 J/g°C
D) 25.0 g Au, CAu = 0.128 J/g°C
E) 25.0 g Ag, CAg = 0.235 J/g°C
7. Define enthalpy, exothermic reaction and endothermic reaction (6.6)
Which statement is FALSE?
A) An exothermic reaction gives heat off heat to the surroundings.
B) Enthalpy is the sum of a system's internal energy and the product of pressure and volume.
C) ΔErxn is a measure of heat.
D) ΔHrxn is the heat of reaction.
E) Endothermic has a positive ΔH.
Chapter 6
1. Define kinetic energy, potential energy, chemical energy and state function(6.2, 6.3)
Energy that is associated with the relative positions of electrons and nuclei in atoms and
molecules is called
A) kinetic energy
B) thermal energy
C) potential energy
D) chemical energy
2. Describe the first law of thermodynamics and use it to model energy changes (6.3)
The law of ________ states that energy that can be neither created or destroyed.
A) kinetic energy
B) the consecration of energy
C) potential energy
D) the conservation of energy
E) thermochemistry
3. Relate internal energy to heat and work (6.4)
(1) Which of the following signs on q and w represent a system that is doing work on the
surroundings, as well as gaining heat from the surroundings?
A) q = +, w = ‒
B) q = ‒, w = +
C) q = +, w = +
D) q = ‒, w = ‒
E) None of these represent the system referenced above.
(2) For ΔEsys to always be -, what must be true?
A) q = w
B) +q > ‒w
C) +w > ‒q
D) ‒w > +q
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4. Given two of the three: work, pressure and change in volume, or a means to solve two
of the three, determine the value for the missing variable (6.4)
Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and is
changing from 12.00 L to 6.00 L in volume at 1.50 atm pressure. (Remember that 101.3 J = 1
L·atm)
A) +25.9 kJ
B) ‒16.0 kJ
C) ‒25.9 kJ
D) ‒24.1 kJ
E) 937 kJ
5. Given three of the four: energy, mass, specific heat and change in temperature, or a
means to solve three of the four, determine the value for the missing variable (6.4)
Determine the final temperature of a gold nugget (mass = 376 g) that starts at 398 K and loses
4.85 kJ of heat to a snowbank when it is lost. The specific heat capacity of gold is 0.128 J/g°C.
A) 133 K
B) 398 K
C) 187 K
D) 297 K
E) 377 K
6. Define the concept heat capacity and relate it to specific heat capacity and molar heat
capacity (6.4)
Which of the following (with specific heat capacity provided) would show the smallest
temperature change upon gaining 200.0 J of heat?
A) 50.0 g Al, CAl = 0.903 J/g°C
B) 50.0 g Cu, CCu = 0.385 J/g°C
C) 25.0 g granite, Cgranite = 0.79 J/g°C
D) 25.0 g Au, CAu = 0.128 J/g°C
E) 25.0 g Ag, CAg = 0.235 J/g°C
7. Define enthalpy, exothermic reaction and endothermic reaction (6.6)
Which statement is FALSE?
A) An exothermic reaction gives heat off heat to the surroundings.
B) Enthalpy is the sum of a system's internal energy and the product of pressure and volume.
C) ΔErxn is a measure of heat.
D) ΔHrxn is the heat of reaction.
E) Endothermic has a positive ΔH.
