In a chemical reaction,


the initial concentration of B was 1.5 times of the concentration of A, but the equilibrium concentrations of A and B were found to be equal. The equilibrium constant (K) for the aforesaid chemical reaction is -

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

The equilibrium constant of the above reaction is K_p. If pure ammonia is left to dissociate, the partial pressure of ammonia at equilibrium is given by (Assume that P_NH3 << P_total at equilibrium)

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)