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 would be the effect on $K_{c}$ if (i) more PCl₅ is added(ii) pressure is increased(iii) the temperature is increased?

Answer 1

"At 473 K, number of reactants  $K_{c}$ for putrefaction of phosphorus pentachloride, PCl₅ is 8.3 x 10⁻³.

If putridity is depicted as, PCl₅ (g)  ⇆  PCl₃ (g) + Cl₂ (g); ΔHϴ 124.0 kJ mol⁻¹

a) Kc= (pcl3 x cl2)/pcl5 all in g

b) Kc = 120-48

c)

(i) Kc would remain the same because in this case, the temperature remains the same.  

(ii) Kc is constant at constant temperature. Thus, in this case, Kc would not change.  

(iii)In an endothermic reaction, the value of Kc increases with an increase in temperature. Since the given reaction in an endothermic reaction, the value of Kc will increase if the temperature is increased. "