For a reaction at equilibrium

A(g) $$\rightleftharpoons$$ B(g) + $${1 \over 2}$$ C(g)

the relation between dissociation constant (K), degree of dissociation ($$\alpha$$) and equilibrium pressure (p) is given by :

The value of K_C is 64 at 800 K for the reaction

N₂(g) + 3H₂(g) ⇌ 2NH₃(g)

The value of K_C for the following reaction is :

NH₃(g) ⇌ $${1 \over 2}$$N₂(g) + $${3 \over 2}$$H₂(g)

The variation of equilibrium constant with temperature is given below :

Temperature	Equilibrium Constant
T1 = 25oC	K1 = 10
T2 = 100oC	K2 = 100

The values of $$\Delta $$H^o, $$\Delta $$G^o at
T₁ and $$\Delta $$G^o at T₂ (in kJ mol^–1) respectively, are close to :
[Use R = 8.314 J K^–1 mol^–1]

For the reaction

Fe₂N(s) + $${3 \over 2}$$H₂(g) ⇌ 2Fe(s) + NH₃(g)