The standard electrode potentials for the half-cell reactions are: $Zn^{2+} + 2e^- \rightarrow Zn \quad E^\circ = -0.76 \, \text{V}$ $Fe^{2+} + 2e^- \rightarrow Fe \quad E^\circ = -0.44 \, \text{V}$ The EMF of the cell reaction: $Fe^{2+} + Zn \rightarrow Zn^{2+} + Fe$ is

Question

The standard electrode potentials for the half-cell reactions are:
$Zn^{2+} + 2e^- \rightarrow Zn \quad E^\circ = -0.76 \, \text{V}$
$Fe^{2+} + 2e^- \rightarrow Fe \quad E^\circ = -0.44 \, \text{V}$
The EMF of the cell reaction:
$Fe^{2+} + Zn \rightarrow Zn^{2+} + Fe$ is

+1.20 V

+0.32 V

-0.32 V

-1.20 V

Solution

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