For the reaction

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

Consider the following reaction:

N₂O₄(g) ⇌ 2NO₂(g); $$\Delta $$H^o = +58 kJ

For each of the following cases (a, b), the direction in which the equilibrium shifts is :
(a) Temperature is decreased.
(b) Pressure is increased by adding N₂ at constant T.

If the equilibrium constant for
A ⇌ B + C is $$K_{eq}^{(1)}$$ and that of
B + C ⇌ P is $$K_{eq}^{(2)}$$, the equilibrium
constant for A ⇌ P is :

For the equilibrium A ⇌ B , the variation of the rate of the forward (a) and reverse (b) reaction with time is given by :