At $25\,^oC$ and $1\,atm$ pressure,mercury reacts with chlorine to form mercurous chloride: $2Hg + Cl_2 \to Hg_2Cl_2; \Delta H = -31.3\,kcal$. What is the entropy change of the reaction at $25\,^oC$?
- A$31300 / 298$
- B$-31300 / 298$
- C$31300 / 760$
- DNone of these
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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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