We are asked to find the **cell potential (E _{cell}) for the following **lead concentration cell given.

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

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

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

E°_{cell} = standard cell potential

n = number of e^{-} transferred

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

In the Nernst Equation, the **E****° _{cell} is needed** but only E

Calculate the cell potential (E_{cell}) for the following lead concentration cell at 298 K.

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