Batteries and corrosion

An electrochemical cell is fueled by the combustion of butane at 1 bar and 298 K. Its cell potential is $\dfrac{\boldsymbol{X}}{F}\times10^3$ volts, where $F$ is the Faraday constant. The value of $\boldsymbol{X}$ is _____.

Use: Standard Gibbs energies of formation at 298 K are: $\Delta_fG^\circ_{\ce{CO2}} = -394\ \mathrm{kJ\,mol^{-1}}$; $\Delta_fG^\circ_{\text{water}} = -237\ \mathrm{kJ\,mol^{-1}}$; $\Delta_fG^\circ_{\text{butane}} = -18\ \mathrm{kJ\,mol^{-1}}$

An aqueous solution of hydrazine ($\ce{N2H4}$) is electrochemically oxidized by $\ce{O2}$, thereby releasing chemical energy in the form of electrical energy. One of the products generated from the electrochemical reaction is $\ce{N2(g)}$.

Choose the correct statement(s) about the above process

Match List - I with List - II.

Choose the correct answer from the options given below :