Question

For a given data: E⁰_Mg2+/Mg = -2.37V E⁰_Cu²⁺/Cu = +0.34V Calculate the emf of the cell in which the following reaction takes place.

\(\underset{(0.0001M)}{Mg(s)}+ Cu^{2+}(aq)\rightarrow \underset{(0.0001M)}{Mg^{2+}(s)}+Cu(s)\)

Answer 1

E⁰_cell = E⁰_Cu²⁺/Cu – E⁰_Mg²⁺/Mg 

= 0.34 – (-2.37) = 2.71V