What is the equilibrium constant `K_(c)` for the following reaction at `400K`? `2NOCI(g) hArr 2NO(g) +CI_(2)(g)` `DeltaH^(Theta) = 77.2 kJ mol^(-1)` and `DeltaS^(Theta) = 122 J K^(-1) mol^(-1) at 400K`.

What is the equilibrium constant `K_(c)` for the following reaction at

1.	What is the equilibrium constant `K_(c)` for the following reaction at `400K`? `2NOCI(g) hArr 2NO(g) +CI_(2)(g)` `DeltaH^(Theta) = 77.2 kJ mol^(-1)` and `DeltaS^(Theta) = 122 J K^(-1) mol^(-1) at 400K`.
Answer» According to Gibbs-Helmhotz equation `DeltaG^(Theta) = DeltaH^(Theta) - T DletaS^(Theta)` `= 77.2 - 400 xx 122 xx 10^(-3)` `28.4 kJ = 28.4 xx 10^(3)J` We know `DeltaG^(Theta) =- 2.303 RT log_(10)K_(c)` `:. log_(10)K_(c) = (-DeltaG^(@))/(2.303RT)` `=(28.4xx10^(3))/(2.303xx8.314xx400) = - 3.7081` `K_(c) = antilog (-3.7081) = 1.958 xx 10^(-4)`

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What is the equilibrium constant `K_(c)` for the following reaction at `400K`? `2NOCI(g) hArr 2NO(g) +CI_(2)(g)` `DeltaH^(Theta) = 77.2 kJ mol^(-1)` and `DeltaS^(Theta) = 122 J K^(-1) mol^(-1) at 400K`.

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