5.1 g NH₄SH is introduced in 3.0 L evacuated flask at 327ºC. 30% of the solid NH₄SH decomposed to NH₃ and H₂S as gases . The Kp of the reaction at 327^oC is (R = 0.082 L atm mol^–1 K^–1, Molar mass of S = 32 g mol^–1 molar mass of N = 14 g mol^–1)

The values of K_p/K_c for the following reactions at 300 K are, respectively : (At 300 K, RT = 24.62 dm³ atm mol^–1)

N₂(g) + O₂(g)  $$\rightleftharpoons$$ 2 NO(g)

N₂O₄(g)  $$\rightleftharpoons$$   2 NO(g)

N₂(g) + 3H₂(g) $$\rightleftharpoons$$ 2 NH₃(g)

Consider the following reversible chemical reactions :



The relation between K₁ and K₂ is :

The gas phase reaction 2NO₂(g) $$ \to $$ N₂O₄(g) is an exothermic reaction. The decomposition of N₂O₄, in equilibrium mixture of NO₂(g) and N₂O₄(g), can be increased by :