If the half-cell reactions- Cu - 2- - e - - -longrightarrow Cu- - -quad - E - o -0-15 V- Cu - 2- -2- e - - -longrightarrow Cuquad quad - E - o -0-34 VCalculate - E - o - of the half cell reaction - Cu - - - e - - -longrightarrow CuAlso predict whether - Cu - - - undergoes disproportionation or not-

Question

Toppr Admin · Accepted Answer

Addiing the -x394-G of the reactionsnFE0-nFE1-nFE22-xD7-F-xD7-0-34-1-xD7-F-xD7-0-15-1-xD7-F-xD7-E20-68-0-15-E2E2-0-53V

If for the half-cell reactions
${C u}^{2 +} + e^{-} ⟶ C u^{+} E^{o} = 0.15 V$
${C u}^{2 +} + 2 e^{-} ⟶ C u E^{o} = 0.34 V$
Calculate $E^{o}$ of the half cell reaction ${C u}^{+} + e^{-} ⟶ C u$
Also predict whether ${C u}^{+}$ undergoes disproportionation or not.

Addiing the $Δ G$ of the reactions
$n F E^{0} = n F E_{1} + n F E_{2}$
$2 \times F \times 0.34 = 1 \times F \times 0.15 + 1 \times F \times E_{2}$
$0.68 = 0.15 + E_{2}$
$E_{2} = 0.53 V$

If for the half-cell reactionsCu2++e−⟶Cu+Eo=0.15 VCu2++2e−⟶CuEo=0.34 VCalculate Eo of the half cell reaction Cu++e−⟶CuAlso predict whether Cu+ undergoes disproportionation or not.

Addiing the ΔG of the reactionsnFE0=nFE1+nFE22×F×0.34=1×F×0.15+1×F×E20.68=0.15+E2E2=0.53V

If for the half-cell reactions
${C u}^{2 +} + e^{-} ⟶ C u^{+} E^{o} = 0.15 V$
${C u}^{2 +} + 2 e^{-} ⟶ C u E^{o} = 0.34 V$
Calculate $E^{o}$ of the half cell reaction ${C u}^{+} + e^{-} ⟶ C u$
Also predict whether ${C u}^{+}$ undergoes disproportionation or not.

Addiing the $Δ G$ of the reactions
$n F E^{0} = n F E_{1} + n F E_{2}$
$2 \times F \times 0.34 = 1 \times F \times 0.15 + 1 \times F \times E_{2}$
$0.68 = 0.15 + E_{2}$
$E_{2} = 0.53 V$