Question

Consider the reversible reaction

A(g)↽−−⇀B(g)

Which values would indicate that there is more B than A at equilibrium?

=1×10–5

=7000

=8×105

=0.2

Answer 1

=8×105

Step-by-step explanation:

This value represents the equilibrium constant, Kc, of the reaction. The equilibrium constant is a measure of the relative concentrations of reactants and products at equilibrium. If the value of Kc is greater than 1, it means that there is more product than reactant at equilibrium, and if the value of Kc is less than 1, it means that there is more reactant than product at equilibrium.

The value 8×105 is greater than 1, so it means that there is more B than A at equilibrium. =8×105.