During a reversible adiabatic expansion of an ideal gas, which of the following is NOT true?
B) pV = nRT
D) W = -$\int$ pdV
E) pV = constant

Question

During a reversible adiabatic expansion of an ideal gas, which of the following is NOT true?
B) pV = nRT 
D) W = -$\int$ pdV 
E) pV = constant

Quizplus · Accepted Answer

During a reversible adiabatic expansion, the gas expands without any transfer of heat and the process is reversible. Therefore, the internal energy remains constant (since there is no change in temperature) and work done by the gas equals the decrease in internal energy. From the first law of thermodynamics, we have dU = -W, where dU is the change in internal energy and W is the work done by the gas. Since dU = 0, we have W = 0. Therefore, the gas does not perform any work on the surroundings and its volume increases without any external pressure being applied. Thus, the product pV remains constant during an adiabatic expansion of an ideal gas. Therefore, option E is not true.

During a Reversible Adiabatic Expansion of an Ideal Gas, Which ∫\int∫

During a Reversible Adiabatic Expansion of an Ideal Gas, Which $\int$