Calculate equilibrium constant for the reaction given below at `400K`, if `DeltaH^(Theta) = 77.2 kJ mol^(-1)` and `DeltaS^(Theta) = 122 J K^(-1) mol^(-1)`
`PCI_(5)(g) rarr PCI_(3)(g) +CI_(2)(g)`

Explanation

To calculate the equilibrium constant \( K \) for the reaction

\[ \text{PCl}_5(g) \rightleftharpoons \text{PCl}_3(g) + \text{Cl}_2(g) \]

at \( 400 \, K \), given that \( \Delta H^\circ = 77.2 \, kJ \, mol^{-1} \) and \( \Delta S^\circ = 122 \, J \, K^{-1} \, mol^{-1} \), we will follow these steps:

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