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(B) For an ideal gas,the entropy change $\Delta S$ is given by the general expression: $\Delta S = n C_p \ln \left( \frac{T_f}{T_i} \right) + n R \ln

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$\Delta S = nR \ln \left( \frac{p_i}{p_f} \right)$

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(B) For an ideal gas,the entropy change $\Delta S$ is given by the general expression: $\Delta S = n C_p \ln \left( \frac{T_f}{T_i} \right) + n R \ln \left( \frac{p_i}{p_f} \right)$ For an isothermal process,the temperature remains constant,so $T_i = T_f$. This implies $\ln \left( \frac{T_f}{T_i} \right) = \ln(1) = 0$. Therefore,the expression simplifies to: $\Delta S = n R \ln \left( \frac{p_i}{p_f} \right)$

For a sample of a perfect gas,when its pressure is changed isothermally from $p_i$ to $p_f$,the entropy change is given by:

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The entropy values (in $J K^{-1} mol^{-1}$) of $H_{2(g)} = 130.6$,$Cl_{2(g)} = 223.0$ and $HCl_{(g)} = 186.7$ at $298 \ K$ and $1 \ atm$ pressure. Then entropy change for the reaction $H_{2(g)} + Cl_{2(g)} \to 2HCl_{(g)}$ is :-

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