Quantity defined by $E^{\text{⚬}}=-\frac{{\mathrm{\Delta }}_{\text{r}}{G}^{\text{⚬}}}{nF}=\frac{RT}{nF}\ln K^{\text{⚬}}$, where ${\mathrm{\Delta }}_{\text{r}}{G}^{\text{⚬}}$ is the standard Gibbs energy of the cell reaction in the direction in which reduction occurs at the right-hand electrode in the diagram representing the cell ('reduction at right'), $K^{\text{⚬}}$ is the standard equilibrium constant for this reaction, $n$ its charge number, $F$ the Faraday constant, $R$ the gas constant and $T$ the thermodynamic temperature.