Question

If the \[\ce{E^{\circ}_{cell}}\] for a given reaction has a negative value, then which of the following gives the correct relationships for the values of ΔG° and K_eq?

Options

• ΔG° < 0; K_eq > 1

• ΔG° < 0; K_eq < 1

• ΔG° > 0; K_eq < 1

• ΔG° > 0; K_eq > 1

Answer 1

ΔG° > 0; K_eq < 1

Explanation:

If \[\ce{E{^{\circ}_{cell}}}\] is negative, then from the relation

\[\ce{\Delta G^\circ = -nFE{^{\circ}_{cell}}}\]

We get ΔG° > 0, meaning the reaction is non-spontaneous.

Also,

ΔG° = −RT ln K_eq​

∴ ΔG° > 0; K_eq < 1