Question

At 473 K, equilibrium constant $K_{c}$ for decomposition of phosphorus pentachloride, PCl₅ is 8.3 x 10⁻³. If decomposition is depicted as, PCl₅ (g) ⇆ PCl₃ (g) + Cl₂ (g); ΔHϴ 124.0 kJ mol⁻¹ . what is the value of $K_{c}$ for the reverse reaction at the same temperature?

Answer 1

From the given chemical reaction, PCL5(g)---PCL3 (g) + CL2 (g), the equilibrium constant Kc will be = [PCL3(g)] [Cl2(g)] / [PCl5(g)].

The equilibrium constant is the state which is obtained where the solids will be ignored, and the gaseous reactants will be taken into consideration.

This is the main ideology behind this principle and is applied to all the chemical reactions.