Question

H2(g) + Br2(g) ⇄ 2HBr(g)

At a certain temperature, the value of the equilibrium constant, K, for the reaction represented above is 2.0 x 105. What is the value of K for the reverse reaction at the same temperature?

Answer 1

The value of K for the reverse reaction is 5 x 10^-6.

Step-by-step explanation:

The value of the equilibrium constant, K, for a given reaction is equal to the ratio of the product concentrations to the reactant concentrations, with each concentration raised to the power of its stoichiometric coefficient.

In the reaction represented by H2(g) + Br2(g) ⇄ 2HBr(g), the value of K is 2.0 x 10^5.

For the reverse reaction, the value of K is the reciprocal of the original K value, which is 1 divided by 2.0 x 10^5, or 5 x 10^-6.