Problem: The value of E°cell for the reaction Zn(s) + Cu2+(aq) <=> Zn2+(aq) + Cu(s) is 1.10 V. What is the value of E for a cell in which [Cu2+] = 1.0 x 10-3 M and [Zn2+] = 1.0 M?a. 1.01 Vb. 1.19 Vc. 0 Vd. -1.01 Ve. -1.19 V 

FREE Expert Solution

We are asked to calculate the value of E for a cell in which [Cu2+] = 1.0 x 10-3 M and [Zn2+] = 1.0 M

Zn(s) + Cu2+(aq) ⇌ Zn2+(aq) + Cu(s)      E°cell = 1.10 V


We will use the Nernst Equation to calculate the cell potential. The Nernst Equation relates the concentrations of compounds and cell potential.

 Ecell=E°cell-(0.0592 Vn) log Q

Ecell = cell potential under non-standard conditions
cell = standard cell potential
n = number of e- transferred
Q= reaction quotient = [products]/[reactants]


We're going to calculate the Ecell using the following steps:

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Problem Details

The value of E°cell for the reaction Zn(s) + Cu2+(aq) <=> Zn2+(aq) + Cu(s) is 1.10 V. What is the value of E for a cell in which [Cu2+] = 1.0 x 10-3 M and [Zn2+] = 1.0 M?

a. 1.01 V
b. 1.19 V
c. 0 V
d. -1.01 V
e. -1.19 V 

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