Electrochemistry · Fuel cell gibbs energy work

Consider the following two half-cell reactions along with the standard reduction potential given :

$\ce{CO2 + 6H+ + 6e- -> CH3OH + H2O}$    $E^\circ_\mathrm{red} = 0.02$ V

$\dfrac{1}{2}$ $\ce{O2 + 2H+ + 2e- -> H2O}$    $E^\circ_\mathrm{red} = 1.23$ V

The fuel cell was set up using the above two reactions such that the cell operates under the standard condition of 1 bar pressure and 298 K temperature. The fuel cell works with 80% efficiency. If the work derived from the cell using 1 mol of $\ce{CH3OH}$ is used to compress an ideal gas isothermally against a constant pressure of 1kPa, then the change in the volume of the gas, $\lvert\Delta V\rvert$ = m$^3$. (Nearest integer)

Given : $F = 96500$ C mol$^{-1}$