Consider a Carnot cycle as shown in the figure. The ideal gas expanded from volume \(V_{1}\) to \(V_{2}\) along the path AB. During this process, the temperature \(T_{1}\) is constant and the entropy changes from \(S_{1}\) to \(S_{2}\). \(T_{2}\) is the temperature of the cold bath.

Which of the following statements is correct?
IIT JAM - 2026,
Answer: A
The correct statement is \(W_{AB} = -NRT_1 \ln\frac{V_2}{V_1}\), with \(W\) taken as the work done on the gas.
On a T-S diagram, horizontal lines are isotherms and vertical lines are adiabats (constant entropy). AB is the isothermal expansion at \(T_1\). For \(N\) moles of ideal gas the work done by the gas is \(\int P\,dV = NRT_1\ln\frac{V_2}{V_1}\), so the work done on it is
\[ W_{AB} = -\int_{V_1}^{V_2} P\,dV = -NRT_1 \ln\frac{V_2}{V_1} \]
The key follows this sign convention, so the expansion work is negative.
BC and DA are adiabats on which the temperature changes, so \(W = \Delta U \neq 0\) on both. CD is an isothermal compression at the cold temperature \(T_2\), so its work involves \(T_2\), not \(T_1\).
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