(A) We use the relationship between Gibbs free energy change $(\Delta G^{o})$ for the given half-reactions.Let the reactions be:$(1) Cu^{+2} + 2e^{-}

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(A) We use the relationship between Gibbs free energy change $(\Delta G^{o})$ for the given half-reactions.Let the reactions be:$(1) Cu^{+2} + 2e^{-} \to Cu$,$\Delta G_{1}^{o} = -2F X_{1}$$(2) Cu^{+} + e^{-} \to Cu$,$\Delta G_{2}^{o} = -1F X_{2}$$(3) Cu^{+2} + e^{-} \to Cu^{+}$,$\Delta G_{3}^{o} = -1F E^{o}$From Hess's Law,reaction $(3) = (1) - (2)$:$\Delta G_{3}^{o} = \Delta G_{1}^{o} - \Delta G_{2}^{o}$$-1F E^{o} = -2F X_{1} - (-1F X_{2})$$-E^{o} = -2X_{1} + X_{2}$$E^{o} = 2X_{1} - X_{2}$

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Difficult

Given the following standard electrode potentials:
$Cu^{+2} + 2e^{-} \to Cu$,$E^{o} = X_{1}$
$Cu^{+} + e^{-} \to Cu$,$E^{o} = X_{2}$
Calculate the standard electrode potential $E^{o}$ for the reaction: $Cu^{+2} + e^{-} \to Cu^{+}$

A
$2X_{1} - X_{2}$
B
$X_{1} - X_{2}$
C
$X_{2} - X_{1}$
D
$2X_{2} - X_{1}$

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Electrochemistry

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Electrode potential and ECell

Calculate the standard electromotive force $(E^o_{cell})$ for the following cell: $Zn|Zn^{2+} (1 \ M)||I^{-} (1 \ M)|CuI|Cu$. Given the half-cell reactions:
$CuI_{(s)} + e^{-} \to Cu_{(s)} + I^{-}_{(aq)}$ ; $E^o = -0.17 \ V$
$Zn^{2+}_{(aq)} + 2e^{-} \to Zn_{(s)}$ ; $E^o = -0.76 \ V$ (in $V$)

Medium

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Give the method to determine the potential of any half-cell.

Easy

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Given $E_{Fe^{+3}/Fe}^{\circ} = -0.036 \ V$ and $E_{Fe^{+2}/Fe}^{\circ} = -0.439 \ V$,calculate the standard electrode potential for the reaction: $Fe^{+3}_{(aq)} + e^{-} \rightarrow Fe^{+2}_{(aq)}$ (in $V$)

Medium

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The standard oxidation potentials for the half-reactions are given as $Zn \to Zn^{2+} + 2e^{-}; E^o = +0.76 \ V$ and $Fe \to Fe^{2+} + 2e^{-}; E^o = +0.41 \ V$. The $EMF$ for the cell reaction $Fe^{2+} + Zn \to Zn^{2+} + Fe$ is ............ $V$.

MediumAIIMS 2001

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The oxidation potentials of $Zn$,$Cu$,and $Ag$ are $0.76 \ V$,$-0.34 \ V$,and $-0.80 \ V$,respectively. Write down the order of their tendency to lose $e^-$.

Easy

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Given the following standard electrode potentials:$Cu^{+2} + 2e^{-} \to Cu$,$E^{o} = X_{1}$$Cu^{+} + e^{-} \to Cu$,$E^{o} = X_{2}$Calculate the standard electrode potential $E^{o}$ for the reaction: $Cu^{+2} + e^{-} \to Cu^{+}$

Similar Questions

Calculate the standard electromotive force $(E^o_{cell})$ for the following cell: $Zn|Zn^{2+} (1 \ M)||I^{-} (1 \ M)|CuI|Cu$. Given the half-cell reactions:$CuI_{(s)} + e^{-} \to Cu_{(s)} + I^{-}_{(aq)}$ ; $E^o = -0.17 \ V$$Zn^{2+}_{(aq)} + 2e^{-} \to Zn_{(s)}$ ; $E^o = -0.76 \ V$ (in $V$)

Give the method to determine the potential of any half-cell.

Given $E_{Fe^{+3}/Fe}^{\circ} = -0.036 \ V$ and $E_{Fe^{+2}/Fe}^{\circ} = -0.439 \ V$,calculate the standard electrode potential for the reaction: $Fe^{+3}_{(aq)} + e^{-} \rightarrow Fe^{+2}_{(aq)}$ (in $V$)

The standard oxidation potentials for the half-reactions are given as $Zn \to Zn^{2+} + 2e^{-}; E^o = +0.76 \ V$ and $Fe \to Fe^{2+} + 2e^{-}; E^o = +0.41 \ V$. The $EMF$ for the cell reaction $Fe^{2+} + Zn \to Zn^{2+} + Fe$ is ............ $V$.

The oxidation potentials of $Zn$,$Cu$,and $Ag$ are $0.76 \ V$,$-0.34 \ V$,and $-0.80 \ V$,respectively. Write down the order of their tendency to lose $e^-$.

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Given the following standard electrode potentials:
$Cu^{+2} + 2e^{-} \to Cu$,$E^{o} = X_{1}$
$Cu^{+} + e^{-} \to Cu$,$E^{o} = X_{2}$
Calculate the standard electrode potential $E^{o}$ for the reaction: $Cu^{+2} + e^{-} \to Cu^{+}$

Calculate the standard electromotive force $(E^o_{cell})$ for the following cell: $Zn|Zn^{2+} (1 \ M)||I^{-} (1 \ M)|CuI|Cu$. Given the half-cell reactions:
$CuI_{(s)} + e^{-} \to Cu_{(s)} + I^{-}_{(aq)}$ ; $E^o = -0.17 \ V$
$Zn^{2+}_{(aq)} + 2e^{-} \to Zn_{(s)}$ ; $E^o = -0.76 \ V$ (in $V$)