Question

The reaction 2 a → b c has a kc of 0.2. the reaction is commenced with initial concentrations [a] = 0.2 m, [b] = 0.2 m and [c] = 0.2 m. in what direction does the reaction occur?

Answer 1

Kc = [b]*[c]/([a]^2) = (0.2 M)^2/(0.2 M)^2 = 1.0
To achieve equilibrium, Kc must be equal to 0.2, therefore Kc must decrease, so the concentrations of b and c must decrease and the concentration of a must increase, meaning the reaction will proceed toward the formation of a.

Answer 2

the answer is 'the reaction shifts to the left to reach equilibrium' on ut, hope I helped! if you need an explanation, feel free to ask me:)

Step-by-step explanation: