Factors affecting equilibria - Effect of Temperature Change

Assertion (A): For any chemical reaction at a particular temperature, the equilibrium constant is fixed and is a characteristic property.

Reason (R): Equilibrium constant is independent of temperature.

At 473 K, equilibrium constant K_c for decomposition of phosphorus pentachloride, PCl₅ is 8.3 ×10^-3. If decomposition is depicted as,

\[\ce{PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)}\]  Δ_rH° = 124.0 kJmol^–1

What would be the effect on K_c if

1. more PCl₅ is added
2. pressure is increased?
3. The temperature is increased?

Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per following endothermic reaction:

\[\ce{CH4 (g) + H2O (g) ⇌ CO (g) + 3H2 (g)}\]

How will the values of Kp and composition of equilibrium mixture be affected by

1. increasing the pressure
2. increasing the temperature
3. using a catalyst?

State the effect of the following on the reaction

\[\ce{2SO2_{(g)} + O2_{(g)} ⇌ 2SO3_{(g)} + 189.4}\]kJ at equilibrium:

(i) Temperature is increased.
(ii) The concentration of SO₂ is increased.
(iii) The pressure is decreased.
(iv) Helium is added at constant pressure.

At 473 K, equilibrium constant K_c for decomposition of phosphorus pentachloride, PCl₅is 8.3 ×10^-3. If decomposition is depicted as,

\[\ce{PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)}\]  Δ_rH° = 124.0 kJmol^–1

Write an expression for K_c for the reaction.

At 473 K, equilibrium constant K_c for decomposition of phosphorus pentachloride, PCl₅is 8.3 ×10^-3. If decomposition is depicted as,

\[\ce{PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)}\]  Δ_rH° = 124.0 kJmol^–1

What is the value of K_c for the reverse reaction at the same temperature?

Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per following endothermic reaction:

\[\ce{CH4 (g) + H2O (g) ⇌ CO (g) + 3H2 (g)}\]

Write as the expression for K_p for the above reaction.