Consider the half-cell reaction-s- Cu-2-e-Cu-E-o-0-15V- Cu-2-2e-Cu-E-o-0-33V- E-o- for the half-cell reaction- - Cu-e- Cu- will be- 0-48V- 0-18V- 0-31V- 0-51V-

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Redox Reactions and Couple

Consider the ...

Question

Consider the half-cell reaction(s)
${C u}^{2 +} + e^{-} \to {C u}^{+}; E^{o} = 0.15 V$
${C u}^{2 +} + 2 e^{-} \to C u; E^{o} = 0.33 V$
$E^{o}$ for the half-cell reaction: ${C u}^{+} + e^{-} \to C u$ will be:

0.48 V

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0.18 V

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0.31 V

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0.51 V

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Solution

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Similar questions

Z n \to Z n^{+ +} + 2 e^{-}, E^{0} = 0.76 V

C u \to C u^{+ +} + 2 e^{-}, E^{0} = 0.34 V

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}

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

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

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