What is the correct volume of equilibrium constant for the following reaction at 400 {K}, if the values of \\Delta {H}^\circ is 77.5 {kJ} {mol}^{-1} and \\Delta {S}^\circ=135 {JK}^{-1} {mol}^{-1} 2 {NOCl}({g}) \⇌ 2 {NO}({g})+{Cl}_{2}({g})

Correct Answer is : 8.545×10−4

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What is the correct volume of equilibrium constant for the following reaction at 400K, if the values of ΔH° is 77.5kJmol−1 and ΔS°=135JK−1mol−1
2NOCl(g)⇌2NO(g)+Cl2(g)

8.545×10−4
8.545×10−2
8.314
135

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