Question

Which reaction is likely to be more exergonic, one with ${\mathbf{K}}_{\mathbf{eq}}$=1000 or one with ${\mathbf{K}}_{\mathbf{eq}}$= 0.001?

Short answer

The reaction in which ${\mathrm{K}}_{eq}$=1000 is more exergonic.

Step-by-step solution

Spontaneous reaction

Reactions that proceed without an external energy supply are called a spontaneous reaction.

For a reaction to be spontaneous, it needs to have a negative value of Gibbs free energy.

Also, for the reaction to be spontaneous, the value of needs to be positive

Relation between Keq and exergonic reaction

When${\mathrm{K}}_{\mathrm{eq}}$ greater than 1, the energy is out in the reaction,which means the reaction is exergonic.

When ${\mathrm{K}}_{\mathrm{eq}}$ is less than 1, the energy is out in the reaction,which means the reaction is endergonic.

The above reaction ${\mathrm{K}}_{\mathrm{eq}}$=1000, is more exergonic.