Calculate the Cell Potential for the Following Unbalanced Reaction That $\mathrm { Mg } ^ { 2 + }$

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ $\mathrm { Mg } ^ { 2 + }$ ] = 0.500 M and [ $\mathrm { Fe } ^ { 3 + }$ ] = 2.00 M
$\quad$$\quad$ Mg(s) + $\mathrm { Fe } ^ { 3 + }$ (aq) ? $\mathrm { Mg } ^ { 2 + }$ (aq) + Fe(s)
E°(Mg²⁺/Mg) = -2.37 V and E°(Fe³⁺/Fe) = -0.036 V

A) +2.09 V
B) -3.18 V
C) +2.35 V
D) +0.36 V
E) -1.51 V

Correct Answer:

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