The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant.
2 HD(g) ⇌ H₂(g) + D₂(g) K_c = 0.28
6 H₂(g) + 6 D₂(g) ⇌ 12 HD(g) K_c = ?

Question

The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant. 2 HD(g)⇌ H₂(g)+ D₂(g)K_c = 0.28 6 H₂(g)+ 6 D₂(g)⇌ 12 HD(g)K_c = ?

Quizplus · Accepted Answer

To find the value of K_c for the second reaction, we can use the relationship between equilibrium constants for a reaction and its reverse reaction: K_reverse = 1/K_forward Thus, we can calculate the equilibrium constant for the reverse reaction: 2 HD(g) ⇌ H₂(g) + D₂(g) K_reverse = 1/0.28 K_reverse = 3.57 Now, we can use this reverse equilibrium constant to calculate the equilibrium constant for the second reaction: 6 H₂(g) + 6 D₂(g) ⇌ 12 HD(g) K_second = (K_reverse)^n, where n is the stoichiometric coefficient for the conversion from the reverse reaction to the second reaction K_second = (3.57)^2 = 12.75 Therefore, the missing equilibrium constant is K_second = 12.75, which corresponds to choice D.

The Equilibrium Constant Is Given for One of the Reactions