PLEASE HELP! this is the last section and I cant figure it out. any assistance would be greatly appreciated

Reaction of galvanic cell

Given

Redox reaction between Zn and Mg

Required

Half reaction

Potential of the cell

Solution

Zn²⁺ + 2e -> Zn E ° = -0.76 V

Mg²⁺ + 2e -> Mg E ° = - 2.37 V

The higher E ° of the cell will act as the positive pole/cathode

Electrode Zn as a cathode (reduction) and Mg as an anode (oxidation) (E ° of Zn cells is greater than Mg)

Half reaction

Cathode: Zn²⁺ + 2e ⇒ Zn E ° = -0.76 V

Anode: Mg ⇒ Mg²⁺ + 2e E ° = +2.37 V

+

Cell reaction: Zn²⁺ + Mg ---> Zn + Mg²⁺ E ° cell = +1.61 V

The reaction occurs spontaneously in the absence of an electric current, thus including galvanic cells/voltaic cells

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