Question

For the reversible reactionA(g)↽−−⇀B(g)A(g)↽−−⇀B(g)which K values would indicate that there is more B than A at equilibrium?a. K=7000Kb. K=0.3Kc. K=6×10^–5d. K=2×10^8

Answer 1

Answer : The correct options are, (a) and (d)

Explanation :

The given reversible reaction is:

`A(g)\rightleftharpoons B(g)`

Equilibrium constant : It is defined as the equilibrium constant. It is defined as the ratio of concentration of products to the concentration of reactants.

The equilibrium constant expression for the given reaction will be:

`K=([B])/([A])`

As per question, when the value of equilibrium constant is greater than 1 then concentration of B is greater than concentration of A at equilibrium.

In the given options, option (a) and option (d) K values would indicate that there is more B than A at equilibrium because value of equilibrium constant is greater than 1.

Hence, the correct options are, (a) and (d)