What is the value of the standard electrode potential, E° for a fuel cell that uses the following reaction? (Give the value in Volts to nearest integer) 1F=96500 C
${\mathrm{C}}_3{\mathrm{H}}_8\left(\mathrm{g}\right)+5{\mathrm{O}}_2\left(\mathrm{g}\right)\to 3{\mathrm{CO}}_2\left(\mathrm{g}\right)+4{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right),{\mathrm{\Delta G}}^0=-2.108\times {10}^3\mathrm{kJ}{\mathrm{mol}}^{-1}$