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.

$\overline{){{\mathbf{E}}}_{{\mathbf{cell}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}{\mathbf{}}{\mathbf{-}}{\mathbf{}}\mathbf{\left(}\frac{\mathbf{0}\mathbf{.}\mathbf{0592}}{\mathbf{n}}\mathbf{\right)}{\mathbf{}}{\mathbf{log}}{\mathbf{}}{\mathbf{Q}}}$

E_{cell} = cell potential under non-standard conditions

E°_{cell} = standard cell potential

n = number of e^{-} transferred

Q= reaction quotient = [products]/[reactants]

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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