The theoretical thermodynamic efficiency eta of a hydrogen-oxygen fuel cell operating at 298 K is defined as ( Delta G circ)/( Delta H circ). Given Delta G circ = -237.2 kJ/mol and Delta H circ = -285.8 kJ/mol, what is the efficiency?

The theoretical thermodynamic efficiency $η$ of a hydrogen-oxygen fuel cell operating at $298 K$ is defined as $\frac{Δ G ^{\circ}}{Δ H ^{\circ}}$ . Given $Δ G^{\circ} = - 237.2 kJ/mol$ and $Δ H^{\circ} = - 285.8 kJ/mol$ , what is the efficiency?

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