ΔG^ o at 25^°C for the reaction 1/2N2(g) + 3/2H2(g) ⇋ 2NH3(g) is -11.392 kj mole^-1. Hence thermodynamics equilibrium constant is : he equilibrium constant for reaction is 10. (Use R=8.3 JK ^−1 mol ^−1)

Answer key : 10^2

The dissociation equilibrium of a gas AB2 can be represented as : 2AB2(g) ⇋ 2AB(g) + B2(g) The degree of dissociation is "x" and is small compared to 1. The expression relating the degree of dissociation (x) with equilibrium constant Kp and total pressure P is.

(A) (2KP/P)^1/2  

(B) (KP/P) 

(C) (2KP/P) 

(D) (2KP/P)^1/3

The equilibrium constant for reaction is 10. What will be the value of ΔG o (R=8.314JK −1 mol −1 & T=300K)

Relation between Kp and Kc:

When concentration are expressed in terms of mole fractions.

We know that partial pressure (P) = Mole fraction × Total pressure (Pt)

In Homogeneous gaseous equilibrium, M(g) + 3N(g)--> 4P(g). Initial concentration of M is equal to that of N. If equilibrium concentrations of M and P are equal then what will be the value of KC?