K_p for the following reaction is 3.0 at 1000 K.

CO₂(g) + C(s) $$\rightleftharpoons$$ 2CO(g)

What will be the value of K_c for the reaction at the same temperature?

(Given : R = 0.083 L bar K^$$-$$1 mol^$$-$$1)

3O₂(g) $$\rightleftharpoons$$ 2O₃(g)

for the above reaction at 298 K, K_c is found to be 3.0 $$\times$$ 10^$$-$$59. If the concentration of O₂ at equilibrium is 0.040 M then concentration of O₃ in M is

Which one of the following conditions will favour maximum formation of the product in the reaction
A_2(g) + B_2(g) ⇌ X_2(g) , $$\Delta $$_rH = –X kJ ?

The equilibrium constants of the following are

N₂ + 3H₂ $$\rightleftharpoons$$ 2NH₃;     K₁

N₂ + O₂ $$\rightleftharpoons$$ 2NO;     K₂

H₂ + $${1 \over 2}$$O₂ $$\rightleftharpoons$$ H₂O;     K₃

The equilibrium constant (K) of the reaction :

2NH₃ + $${5 \over 2}$$ O₂ $$\rightleftharpoons$$ 2NO + 3H₂O will be