Question

Determine the overall reaction and its standard cell potential (in V) at 25°C for the reaction involving the galvanic cell made from a half-cell consisting of a copper electrode in 1 M copper(I) nitrate solution and a half-cell consisting of an iron electrode in 1 M iron(III) nitrate. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.) Overall reaction

Answer 1

Answer:

Standard cell potential is 0.56V

Explanation:

Standard reduction potential ($E^{0}$) are given below-

                             $E_{Cu^{+}\mid Cu}^{0}=0.52V$

                              $E_{Fe^{3+}\mid Fe}^{0}=-0.04V$

As $E_{Cu^{+}\mid Cu}^{0}$ is greater than $E_{Fe^{3+}\mid Fe}^{0}$ therefore Fe will be oxidized to $Fe^{3+}$ and $Cu^{+}$ will be reduced to Cu

Oxidation: $Fe(s)-3e^{-}\rightarrow Fe^{3+}(aq.)$

Reduction: $Cu^{+}(aq.)+e^{-}\rightarrow Cu(s)$

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Overall: $Fe(s)+3Cu^{+}(aq.)\rightarrow Fe^{3+}(aq.)+3Cu(s)$

Standard cell potential, $E_{cell}^{0}=E_{Cu^{+}\mid Cu}^{0}-E_{Fe^{3+}\mid Fe}^{0}=(0.52+0.04)V=0.56V$