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

Standard cell potential is 0.56V

Step-by-step 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)`

------------------------------------------------------------------------------------------------------

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`