Question

If the equilibrium constants for the two reactions 2 HCl(g) H_2 (g) + Cl_2 (g) and I_2 (g) + Cl_2 (g) 2 ICI(g) are denoted K_1 and K_2 respectively, then the equilibrium constant for the reaction 2 HCl(g) + I_2 (g) 2 ICI(g) + H_2 (g) equals

Answer 1

The equilibrium constant for the reaction 2 HCl(g) + I₂(g) ⇒ 2 ICl(g) + H₂(g) can be found by multiplying the given equilibrium constants K₁ and K₂ for the individual component reactions; K₃ = K₁ × K₂.

Step-by-step explanation:

The question asks for the equilibrium constant of the reaction 2 HCl(g) + I₂ (g) ⇒ 2 ICl(g) + H₂ (g) given the equilibrium constants for the reactions 2 HCl(g) ⇒ H₂ (g) + Cl₂ (g) and I₂ (g) + Cl₂ (g) ⇒ 2 ICl(g), denoted as K₁ and K₂ respectively.

Using the principle that the equilibrium constant for a reaction that is the sum of two or more reactions is equal to the product of the equilibrium constants for the individual reactions, the equilibrium constant K₃ for the given reaction is found by multiplying K₁ and K₂. Therefore, the equilibrium constant for 2 HCl(g) + I₂ (g) ⇒ 2 ICl(g) + H₂ (g) is K₃ = K₁ × K₂.