Question

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

Answer 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.

Answer 2

Sapling???

Answer 3

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