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Redox Reactions and Couple

If for the ha...

Question

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.

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Solution

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

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Similar questions

Q. If for the half cell reactions

C u^{2 +} + e^{-} \to C u^{+}

E^{o} = 0.15 V

C u^{2 +} + 2 e^{-} \to C u

E^{o} = 0.34 V

E^{o}

of the half cell reaction

C u^{+} + e^{-} \to C u

also predict whether

C u^{+}

undergoes disproportionation or not.

E^{o}

values for the half cell reactions are given:

C u^{2 +} + e^{-} \to C u^{+}

E^{o} = 0.15

V

C u^{2 +} + 2 e^{-} \to C u

E^{o} = 0.34

V
What will be the

E^{o}

of the half-cell:

C u^{+} + e^{-} \to C u

?

C u^{2 +} + 2 e^{-} \to C u; E^{o} = 0.337

V

C u^{2 +} + e^{-} \to C u^{+}; E^{o} = - 0.153

V

E^{o}

value for the reaction,

C u^{+} + e \to C u

Q. If for the following half-cell reactions :

C u^{2 +} + e^{-} \to C u^{\oplus}

E^{\oplus} = 1.77 V

C u^{2 +} + 2 e^{-} \to C u

;

E^{⊖} = - 0.34

E^{⊖}

of the half-cell reaction will be (in V)

C u^{\oplus} + e^{-} \to C u

Q. Consider the following half cells

C u_{(s)} \to C u_{(a q)}^{2 +} + 2 e^{-}; E^{o} = - 0.325 V

C u_{(a q)}^{+} + e^{-} \to C u_{(s)}; E^{o} = 0.50 V

E^{o}

for the reaction

2 C u_{(a q)}^{+} \to C u_{(a q)}^{2 +} + C u_{(s)}

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