Q. In a closed system, if the internal energy increases, what can be said about the work done on the system?
A.
Work is done by the system.
B.
Work is done on the system.
C.
No work is done.
D.
Work is irrelevant.
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Solution
If the internal energy of a closed system increases, it indicates that work is done on the system.
Correct Answer:
B
— Work is done on the system.
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Q. In a constant pressure process, the work done by the system is given by which equation?
A.
W = PΔV
B.
W = ΔH
C.
W = ΔU
D.
W = Q + ΔH
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Solution
The work done by the system at constant pressure is given by W = PΔV, where P is pressure and ΔV is the change in volume.
Correct Answer:
A
— W = PΔV
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Q. In a reaction at equilibrium, what happens to the enthalpy change (ΔH) if the temperature is increased?
A.
ΔH increases.
B.
ΔH decreases.
C.
ΔH remains constant.
D.
ΔH becomes negative.
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Solution
According to Le Chatelier's principle, increasing temperature shifts the equilibrium position, which can affect the enthalpy change (ΔH) depending on the reaction.
Correct Answer:
A
— ΔH increases.
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Q. In a reversible isothermal expansion of an ideal gas, what is the work done by the gas?
A.
W = nRT ln(Vf/Vi)
B.
W = nRT (Vf - Vi)
C.
W = -PΔV
D.
W = 0
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Solution
The work done by the gas during a reversible isothermal expansion is given by W = nRT ln(Vf/Vi).
Correct Answer:
A
— W = nRT ln(Vf/Vi)
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Q. What is the effect of increasing pressure on the equilibrium of an exothermic reaction with fewer moles of gas on the product side?
A.
Shifts to the left.
B.
Shifts to the right.
C.
No effect.
D.
Increases temperature.
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Solution
Increasing pressure shifts the equilibrium to the side with fewer moles of gas, which is the product side in this case.
Correct Answer:
B
— Shifts to the right.
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Q. What is the enthalpy change for the reaction: N2(g) + 3H2(g) → 2NH3(g) if ΔHf° for NH3 is -45.9 kJ/mol?
A.
-137.7 kJ
B.
-91.8 kJ
C.
0 kJ
D.
45.9 kJ
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Solution
The enthalpy change for the reaction is calculated as ΔH = 2 * ΔHf°(NH3) = 2 * (-45.9 kJ) = -91.8 kJ.
Correct Answer:
A
— -137.7 kJ
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Q. What is the relationship between Gibbs free energy (G) and spontaneity of a reaction?
A.
G < 0 indicates non-spontaneous reaction
B.
G > 0 indicates spontaneous reaction
C.
G = 0 indicates spontaneous reaction
D.
G < 0 indicates spontaneous reaction
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Solution
A negative Gibbs free energy change (G < 0) indicates that a reaction is spontaneous.
Correct Answer:
D
— G < 0 indicates spontaneous reaction
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Q. Which of the following statements is true about the first law of thermodynamics?
A.
Energy can be created or destroyed.
B.
Energy can only be transformed from one form to another.
C.
The total energy of a closed system decreases.
D.
Heat and work are the same.
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Solution
The first law of thermodynamics states that energy cannot be created or destroyed, only transformed.
Correct Answer:
B
— Energy can only be transformed from one form to another.
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