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(C) From the ideal gas equation,$PV = nRT$,the molar volume $V_m = \frac{V}{n} = \frac{RT}{P}$.Thus,$V_m \propto \frac{T}{P}$.For maximum molar volume

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At $127\,^oC$ and $1\, atm$ pressure

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(C) From the ideal gas equation,$PV = nRT$,the molar volume $V_m = \frac{V}{n} = \frac{RT}{P}$.Thus,$V_m \propto \frac{T}{P}$.For maximum molar volume,we need the highest temperature $(T)$ and the lowest pressure $(P)$.Comparing the conditions:$A$: $T = 273.15\, K, P = 1\, atm \implies \frac{T}{P} = 273.15$$B$: $T = 273.15\, K, P = 2\, atm \implies \frac{T}{P} = 136.57$$C$: $T = 127 + 273 = 400\, K, P = 1\, atm \implies \frac{T}{P} = 400$$D$: $T = 273 + 273 = 546\, K, P = 2\, atm \implies \frac{T}{P} = 273$Comparing the values,the ratio $\frac{T}{P}$ is maximum for option $C$.

In which of the following conditions will the molar volume of $CO_2$ be maximum?

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