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Chemistry

Consider the following cell:
Pt|H2(g, 0.460 atm)|H (aq, ? M)||Ag (aq, 1.00 M)|Ag(s)

If the measured cell potential is 1.00 V at 25 °C and the standard reduction potential of the Ag /Ag half-reaction couple is 0.80 V, calculate the hydrogen ion concentration in the anode compartment

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Daisy

  1. H2 ==> 2H^+ + 2e Eo = 0
    2Ag^+ + 2e ==> Ag(s) Eo = 0.8
    -----------------------------
    H2 + 2Ag^+ ==> 2H^+ + 2Ag Ecell = 1.00

    Ecell = Eocell - (0.0592/2)log(H^+)^2/(pH2*(Ag^+)^2

    Ecell = 1.00v
    Eocell = 0.8v
    pH2 = 0.0460 atm
    (Ag^+) = 1.00M
    (H^+) = x
    Solve for x.

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    DrBob222

  2. Sapling???

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    Tulip

  4. .44

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    Anonymous

  5. Ecell = 1.00v
    Eocell = 0.8v
    pH2 = 0.0460 atm
    (Ag^+) = 1.00M
    (H^+) = x
    Q= [(H^+)^2 / (pH2* (Ag^+)^2)]
    R = 8.3145J/mol K
    T = 298K
    F = 96485J/V mol
    n = 2
    Ecell = Eocell - (RT/Fn)* lnQ

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    Sam

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