Use the standard half-cell potential listed below to calculate the standard cell

Question

Use the standard half-cell potential listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 degree C. Mg(s) + Cu^2 + (aq) rightarrow Cu(s) + Mg^2+(aq) Mg^2+(aq) + 2 e^- rightarrow Mg(s) E degree = -2.38 V Cu^2+(aq) + 2e^- rightarrow Cu(s) E degree = 0.34 V EMF_____ Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 degree C. 2 K(s) + I_2(s) rightarrow 2 K^+(aq) + 2 I^-(aq) K^+(aq) + e^- rightarrow K(s) E degree = -2.93 V I_2(s) 2 e^- rightarrow 2 I^-(aq) E degree = 0.54 V

Explanation / Answer

From the overall reaction, it is clear that Mg is oxidised and the copper is reduced as the oxidation number of Mg is increased from 0 to 2, so it is oxidised and the oxidation number of Cu is reduced from 2 to 0 so it is reduced.

In general, the oxidation reaction occurs at anode so Mg is oxidised at anode and the copper is reduced at cathode.

E of the cell =E cathode-E anode

The standard oxidation potential is negative of reduction potential.

E of the cell=0.34 V +2.38 V=2.72 V

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