Step 1

**$\overline{)\mathbf{\u2206}\mathbf{G}\mathbf{\xb0}\mathbf{}\mathbf{=}\mathbf{}\mathbf{-}\mathbf{nF}{\mathbf{E}\mathbf{\xb0}}_{\mathbf{cell}}}\phantom{\rule{0ex}{0ex}}{\mathbf{E}\mathbf{\xb0}}_{\mathbf{cell}}\mathbf{}\mathbf{=}\mathbf{}\frac{\mathbf{\u2206}\mathbf{G}\mathbf{\xb0}}{\mathbf{-}\mathbf{nF}}\phantom{\rule{0ex}{0ex}}{\mathbf{E}\mathbf{\xb0}}_{\mathbf{cell}}\mathbf{}\mathbf{=}\frac{\mathbf{-}\mathbf{411}\mathbf{}\overline{)\mathbf{kJ}}\mathbf{}\mathbf{\times}\mathbf{}{\displaystyle \frac{{\mathbf{10}}^{\mathbf{3}}\mathbf{}\overline{)\mathbf{J}}}{\mathbf{1}\overline{)\mathbf{}\mathbf{kJ}}}}}{\mathbf{-}\mathbf{}\mathbf{(}\mathbf{6}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{e}}^{\mathbf{-}}}\mathbf{)}\mathbf{(}\mathbf{96}\mathbf{,}\mathbf{468}\mathbf{}{\displaystyle \frac{\overline{)J}}{V\xb7\overline{)\mathrm{mol}{e}^{-}}}}\mathbf{)}}$**

**E° _{cell }= 0.71 V**

A standard galvanic cell is constructed so that the overall cell reaction is

2Al^{3+} (aq) + 3M (s) → 3M ^{2+} (aq) + 2Al (s)

where M is an unknown metal. If ΔG° = -411 kJ for the overall cell reaction, identify the metal used to construct the standard cell.

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