You visited us 1 times! Enjoying our articles? Unlock Full Access!

Types of Redox Reactions

If for the ha...

Question

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

Open in App

Solution

To calculate the $E^{o}$ for resultant reaction, let's reverse the first reaction and add the gibss free energy of component reactions,
$G^{o} = - n F E^{o}$
$G_{3}^{o} = G_{1}^{o} + G_{2}^{o}$
$- 1 F E_{3}^{o} = - 1 F \times (- .15) - 2 F \times .34$
$E_{3}^{o} = .53 V$
$C u^{+}$ undergoes disproportionation.

Suggest Corrections

Similar questions

{C u}^{2 +} + e^{-} ⟶ C u^{+} E^{o} = 0.15 V

{C u}^{2 +} + 2 e^{-} ⟶ C u E^{o} = 0.34 V

E^{o}

{C u}^{+} + e^{-} ⟶ C u

{C u}^{+}

E^{o}

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

E^{o} = 0.15

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

E^{o} = 0.34

E^{o}

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

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

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

E^{o}

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^{0}

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

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}

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

Join BYJU'S Learning Program