Calculate the equilibrium constant for the reaction \( P \) given below at \( 400 \mathrm{~K} \)....
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0Calculate the equilibrium constant for the reaction
\( P \)
given below at \( 400 \mathrm{~K} \), if \( \Delta \mathrm{H}^{\circ}=77.2 \mathrm{~kJ} \mathrm{~mol}^{-1} \) and \( \Delta \mathrm{S}^{\circ} \)
W
\( =122 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} \).
\( \mathrm{PCl}_{5(\mathrm{~s})} \rightleftharpoons \mathrm{PCl}_{3(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})} \)
(1) \( 2.135 \times 10^{-4} \)
(2) \( 1.958 \times 10^{-4} \)
(3) \( 4.524 \times 10^{-3} \)
(4) \( 1.001 \times 10^{-3} \)
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