Calculate the equilibrium constant, K for the following reaction at 400 K ? 2NOCl(g) hArr 2NO(g) + Cl_(2)(g) Given thatDelta_(r) H^(@) = 80.0 kJ mol^(_1) and Delta_(r)S^(@)=120 J K^(-1) mol^(-1) at 400 K.

Calculate the equilibrium constant, K for the following reaction at 40

1.	Calculate the equilibrium constant, K for the following reaction at 400 K ? 2NOCl(g) hArr 2NO(g) + Cl_(2)(g) Given thatDelta_(r) H^(@) = 80.0 kJ mol^(_1) and Delta_(r)S^(@)=120 J K^(-1) mol^(-1) at 400 K.
Answer» SOLUTION :`Delta_(r) G^(@) = Delta_(r)H^(@) - TDelta_(r)S^(@) = 80000J - 400 xx 120 J = 32000 J` Now, `Delta_(r) G^(@) = -2.303 RT log K ` `:. 32000 = - 2.303 xx 8.314 xx 400 xx LOGK `or `log K = - 4.1782 = BAR(5).8218` `:.K = ` Antilog `bar(5).8218 = 6.634 xx 10^(-5)`