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Methanol-oxygen fuel cell: cell and half-cell potentials

This type of question, asked 2 times: 3 Apr 2025, 2 Apr 2026 S2. All 2 questions below, oldest first.

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  1. Question 1

    3 Apr 2025

    109
    The standard cell potential (Ecell ⊖)\left( E_{\text{cell~}}^{\ominus} \right) of a fuel cell based on the oxidation of methanol in air that has been used to power television relay station is measured as 1.21 V . The standard half cell reduction potential for O2(EO2/H2Oo)O_{2}\left( E_{O_{2}/H_{2}O}^{o} \right) is 1.229 V . Choose the correct statement:

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  2. Question 2

    2 Apr 2026 S2

    48
    Consider the following two half-cell reactions along with the standard reduction potential given :
    CO2+6H++6e−→CH3OH+H2OEred o=0.02 V{CO}_{2} + 6H^{+} + 6e^{-} \rightarrow {CH}_{3}OH + H_{2}OE_{\text{red~}}^{o} = 0.02\text{ }V
    12O2+2H++2e−→H2OEred o=1.23 V\frac{1}{2}O_{2} + 2H^{+} + 2e^{-} \rightarrow H_{2}OE_{\text{red~}}^{o} = 1.23\text{ }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%80\% efficiency. If the work derived from the cell using 1 mol of CH3OH{CH}_{3}OH is used to compress an ideal gas isothermally against a constant pressure of 1 kPa , then the change in the volume of the gas, ΔV=\Delta V = ____\_\_\_\_ m3m^{3}. (Nearest integer) Given : F=96500Cmol−1F = 96500C{mol}^{- 1}