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Calculate the standard reduction potential for the reaction H_2O+ e to 1/2 H_2+OH^- using the Nernst equation and the fact that the standard reduction potential for the reaction H^+ + e to 1/2 H_2 is by definition equal to 0.00V at 25^@C |
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Answer» Solution :Given that `H_2O + e to 1/2 H_2 +OH^- , E^@=xV` (say) `THEREFORE` for the reaction, `H_2Oto H^+ +OH^- , E^@=xV` The Nernst EQUATION is `E_(cell)=E^@- 0.0591/1 LOG[H^+][OH^-]` At EQUILIBRIUM `E_(cell)=0 and [H^+][OH^-]=K_w=1 times 10^-14` `therefore 0=x-0.0591/1 log 10^-14` or `x=-0.8274 V` |
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