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Posted by on Tuesday, March 27, 2012 at 7:43pm.

Consider the cell: (Pt) H2/H+ || (Pt) H+/H2. In the anode half-cell, hydrogen gas at 1.0 atm is bubbled over a platinum electrode dipping into a solution that has a pH of 7.0. The other half-cell is identical to the first except that the solution around the platinum electrode has a pH of 0.0. What is the cell voltage?

  • chemistry - , Tuesday, March 27, 2012 at 10:10pm

    For the anode written as a reduction:
    E = Eo - (0.0592/n)log(pH2/H^+)
    Eo = 0, and H^+ = 1E-7, E then written as an oxidation will be the negative of that.

    E for the cathode written as a reduction:
    same equation with different numbers.
    Then E cell = Eoxdn + Eredn
    I think the answer is approximately 0.50v.

  • chemistry - , Tuesday, March 27, 2012 at 10:49pm

    nevermind i got it.. the answer is -.414
    thanks though

  • chemistry - , Wednesday, March 28, 2012 at 12:57am

    right. I dropped the - sign when I typed it in.

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