What is the voltage of the cell if [Cu2+] = .200 M and [Zn2+] = .0200M (Ecell = +1.10V)

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What is the voltage of the cell if [Cu2+] = .200 M and [Zn2+] = .0200M (Ecell = +1.10V)

[From: ] [author: ] [Date: 11-04-22] [Hit: ]

Ecell = +1.10 - 0.Ecell = +1.10 + 0.+1.10 + 0.......

it is a galvanic cell,

Zn(s) + Cu 2+ (aq) -> Cu (s) + Zn 2+ (aq)

-

it would be log [Zn++]/[Cu++] in eqn

Ecell = +1.10 - 0.0592/2 log(0.020/0.200)

Ecell = +1.10 - 0.0592/2 log(10^-1)

Ecell = +1.10 + 0.0592/2
+1.10 + 0.03 = 1.13

-

Ecell = Eocell - 0.0592/nlog[Q]

Q = products/reactants = [Cu++]/[Zn++]

The cell is a 2-electron process.

Ecell = +1.10 - 0.0592/2 log(0.200/0.0200)

Ecell = +1.07

1

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