Chemistry · 2016
JEE Main · 9 April 2016, Shift 1 · Q37
For the reaction, A ( g )+ B ( g ) → C ( g )+ D ( g ), Δ H^° and Δ S^° are, respectively, -29.8 kJ mol^-1 and -0.100 kJ K^-1 mol^-1 at 298 K. The…
For the reaction, $\displaystyle \mathrm{A}(\mathrm{g})+\mathrm{B}(\mathrm{g}) \rightarrow \mathrm{C}(\mathrm{g})+\mathrm{D}(\mathrm{g}), \Delta H^{\circ}$ and $\displaystyle \Delta S^{\circ}$ are, respectively, $\displaystyle -29.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $\displaystyle -0.100 \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$ at $\displaystyle 298$ K. The equilibrium constant for the reaction at $\displaystyle 298$ K is :
Official answer
(4)
$\displaystyle 1$
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JEE Main 2016 Chemistry question, with the answer from NTA’s final answer key. Where our answers come from.