Calculate the equilibrium constant for the reaction given below at \( 400 \mathrm{~K} \), if \( ....

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Calculate the equilibrium constant for the reaction
\( \mathrm{P} \)
given below at \( 400 \mathrm{~K} \), if \( \Delta \mathrm{H}^{\circ}=77.2 \mathrm{~kJ} \mathrm{~mol}^{-1} \) and \( \Delta \mathrm{S}^{\mathrm{o}}=122 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} \) \( \mathrm{PCl}_{5}(\mathrm{~g}) \rightarrow \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \)
(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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