What would be the electrode potential for the given half cell reaction at pH = 5 ? 2H2O → O2 + 4H+ + 4e− ; E°red = 1.23 V (R = 8.314 J mol−1 K−1; Temp = 298 K; oxygen under std. atm. pressure of 1 bar)

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Accepted Answer

1.52. The electrode potential is adjusted using the Nernst equation, which accounts for the change in concentration of H+ ions due to the pH level. At pH 5, the concentration of H+ is lower than at standard conditions, resulting in a higher potential of 1.52 V.

What would be the electrode potential for the given half cell reaction at pH = 5 ? 2H2O → O2 + 4H+ + 4e− ; E°red = 1.23 V (R = 8.314 J mol−1 K−1; Temp = 298 K; oxygen under std. atm. pressure of 1 bar)

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