Use the Nernst equation to calculate the cell potential, \( E_{\text {cell, }} \) for a galvanic cell consisting of \( \mathrm{Fe} / \mathrm{Fe}^{2+} \) and \( \mathrm{Pb} / \mathrm{Pb}^{2+} \), if \( \left[\mathrm{Pb}^{2+}\right]=0.0018 \mathrm{M} \) and \( \left[\mathrm{Fe}^{2+}\right]=0.201 \mathrm{M} \) at \( 25^{\circ} \mathrm{C} \) The Faraday constant has a known value of \( 96500 \mathrm{~J} /(\mathrm{V} \cdot \) mol) , has a value of \( 8.314(\mathrm{~J} / \mathrm{K} \) - mol) The half-reactions and the reduction potentials for each are shown Half-Reaction \( \mathrm{Fe}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \longrightarrow \mathrm{Fe}(\mathrm{s})-0.44 \) \( \mathrm{~Pb}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \longrightarrow \mathrm{Pb}(\mathrm{s})-0.13 \)
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