Which of the following statements or relation | vedclass

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(C) For an isothermal reversible expansion of an ideal gas,the work done is given by the formula $w = - nRT \ln \frac{V_2}{V_1}$.Option $A$ is correct

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$w = nRT \ln \frac{V_2}{V_1}$ (isothermal reversible expansion of an ideal gas)

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(C) For an isothermal reversible expansion of an ideal gas,the work done is given by the formula $w = - nRT \ln \frac{V_2}{V_1}$.Option $A$ is correct because for an ideal gas,internal energy $U$ is a function of temperature only,so $\Delta U = 0$ for isothermal processes.Option $B$ is the correct formula for work done.Option $C$ is incorrect because it lacks the negative sign,which represents work done by the system.Option $D$ is correct because at constant volume,$w = 0$,so $\Delta U = q_v$.

Which of the following statements or relationships is not correct in thermodynamic changes?

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