Problem: The value of E°cell for the reaction Zn(s) + Cu 2+(aq) <=> Zn 2+(aq) + Cu(s) is 1.10 V. What is the value of E for a cell in which [Cu 2+] = 1.0 x 10 -3 M and [Zn 2+] = 1.0 M? a. 0.63 Vb. 0.77 Vc. 1.01 Vd. 1.28 Ve. 1.77 V

FREE Expert Solution

We are asked to find the cell potential of the given reaction. We will use the Nernst Equation to calculate the cell potential with the given conditions. The Nernst Equation relates the concentrations of compounds and cell potential.

Ecell = E°cell - (0.0592n) log Q

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

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Problem Details

The value of E°cell for the reaction Zn(s) + Cu 2+(aq) <=> Zn 2+(aq) + Cu(s) is 1.10 V. What is the value of E for a cell in which [Cu 2+] = 1.0 x 10 -3 M and [Zn 2+] = 1.0 M? 

a. 0.63 V

b. 0.77 V

c. 1.01 V

d. 1.28 V

e. 1.77 V

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