(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

The $EMF$ of a cell whose half-cell reactions are given below is .......... $V$.
$Mg^{2+} + 2e^- \to Mg_{(s)}; E^o = -2.37 \ V$
$Cu^{2+} + 2e^- \to Cu_{(s)}; E^o = +0.34 \ V$ (in $V$)

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When a rod of metal $A$ is dipped in an aqueous solution of metal $B$ (concentration of $B^{2+}$ ion being $1 \ M$) at $25 \ ^oC$,the standard electrode potentials are $E^o_{A^{2+}/A} = -0.76 \ V$ and $E^o_{B^{2+}/B} = +0.34 \ V$. What will happen?

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Which is the increasing order of reducing power of the following metals on the basis of standard electrode potential? $Ag^{+}/Ag = 0.80 \ V$,$Mg^{2+}/Mg = -2.37 \ V$,$Hg^{2+}/Hg = 0.79 \ V$,$Cr^{3+}/Cr = -0.74 \ V$

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The standard reduction potentials for $Cu^{2+}|Cu$ and $Cu^{2+}|Cu^{+}$ are $0.337 \, V$ and $0.153 \, V$ respectively. What is the standard electrode potential for the $Cu^{+}|Cu$ half-cell in $V$?

Medium

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If the standard potential of the electrochemical cell for the reaction $2Ag_{(aq)}^+ + Cd_{(s)} \to Cd_{(aq)}^{2+} + 2Ag_{(s)}$ is $1.20 \ V$,calculate the standard Gibbs free energy change in $kJ$.

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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: $Cu^{+2} + e^{-} \to Cu^{+}$

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The $EMF$ of a cell whose half-cell reactions are given below is .......... $V$.$Mg^{2+} + 2e^- \to Mg_{(s)}; E^o = -2.37 \ V$$Cu^{2+} + 2e^- \to Cu_{(s)}; E^o = +0.34 \ V$ (in $V$)

When a rod of metal $A$ is dipped in an aqueous solution of metal $B$ (concentration of $B^{2+}$ ion being $1 \ M$) at $25 \ ^oC$,the standard electrode potentials are $E^o_{A^{2+}/A} = -0.76 \ V$ and $E^o_{B^{2+}/B} = +0.34 \ V$. What will happen?

Which is the increasing order of reducing power of the following metals on the basis of standard electrode potential? $Ag^{+}/Ag = 0.80 \ V$,$Mg^{2+}/Mg = -2.37 \ V$,$Hg^{2+}/Hg = 0.79 \ V$,$Cr^{3+}/Cr = -0.74 \ V$

The standard reduction potentials for $Cu^{2+}|Cu$ and $Cu^{2+}|Cu^{+}$ are $0.337 \, V$ and $0.153 \, V$ respectively. What is the standard electrode potential for the $Cu^{+}|Cu$ half-cell in $V$?

If the standard potential of the electrochemical cell for the reaction $2Ag_{(aq)}^+ + Cd_{(s)} \to Cd_{(aq)}^{2+} + 2Ag_{(s)}$ is $1.20 \ V$,calculate the standard Gibbs free energy change in $kJ$.

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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: $Cu^{+2} + e^{-} \to Cu^{+}$

The $EMF$ of a cell whose half-cell reactions are given below is .......... $V$.
$Mg^{2+} + 2e^- \to Mg_{(s)}; E^o = -2.37 \ V$
$Cu^{2+} + 2e^- \to Cu_{(s)}; E^o = +0.34 \ V$ (in $V$)