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Q.

What would be the electrode potential for the given half cell reaction at pH=5?2H2O→O2+4H⊕+4e−; Ered0=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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Detailed Solution

E=1.23+0.0594log1H+4=1.23+0.0594log110−54=1.23+0.0594×20 =1.23+0.295 =+1.525 V

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What would be the electrode potential for the given half cell reaction at pH=5?2H2O→O2+4H⊕+4e−; Ered0=1.23 V(R=8.314 J mol-1 K -1; Temp = 298 K; oxygen under std. atm. Pressure of 1 bar)