(B) $1$. In a galvanic cell, the electrode with the higher reduction potential acts as the cathode (positive electrode).$2$. Given $E^0_{(Cu^{2+}|Cu)}

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$Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$

(B) $1$. In a galvanic cell, the electrode with the higher reduction potential acts as the cathode (positive electrode).$2$. Given $E^0_{(Cu^{2+}|Cu)} = +0.34 \text{ V}$ and $E^0_{(H^+|H_2)} = 0.00 \text{ V}$.$3$. Since $+0.34 \text{ V} > 0.00 \text{ V}$, the copper electrode is the cathode.$4$. Reduction occurs at the cathode: $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

$A$ galvanic cell consists of a copper electrode and a standard hydrogen electrode. If $E^0_{(Cu^{2+}(aq)|Cu(s))} = +0.34 \text{ V}$, identify the reaction taking place at the positive electrode during the working of the cell.

MHT CET 2026 All MHT CET

A
$Cu(s) \rightarrow Cu^{2+}(aq) + 2e^-$
B
$Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$
C
$H_2(g) \rightarrow 2H^+(aq) + 2e^-$
D
$H^+(aq) + e^- \rightarrow \frac{1}{2} H_2(g)$

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The standard oxidation potentials of zinc and silver in water at $298 \ K$ are:
$Zn_{(s)} \to Zn^{2+}_{(aq)} + 2e^- ; E^o_{ox} = 0.76 \ V$
$Ag_{(s)} \to Ag^{+}_{(aq)} + e^- ; E^o_{ox} = -0.80 \ V$
Which of the following reactions actually takes place spontaneously?

Medium

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Arrange the following metals in the order in which they displace each other from the solution of their salts: $Al, Cu, Fe, Mg$ and $Zn$.

Medium

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For the cell reaction:
$2 Fe^{3+}_{(aq)} + 2 I^{-}_{(aq)} \rightarrow 2 Fe^{2+}_{(aq)} + I_{2(aq)}$
$E^{\ominus}_{cell} = 0.24 \ V$ at $298 \ K$. The standard Gibbs energy $(\Delta_r G^{\ominus})$ of the cell reaction in $kJ \ mol^{-1}$ is:
[Faraday constant $F = 96500 \ C \ mol^{-1}$]

DifficultNEET 2019

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If standard reduction potentials $(E^0)$ of $(Al^{+3}(aq)|Al(s))$, $(Fe^{+2}(aq)|Fe(s))$, $(Cu^{+2}(aq)|Cu(s))$ and $(Ag^{+1}(aq)|Ag(s))$ are $-1.66 \text{ V}$, $-0.44 \text{ V}$, $+0.34 \text{ V}$ and $+0.79 \text{ V}$ respectively, which of the following reactions is non-spontaneous?

DifficultMHT CET 2026

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For the reaction $H_2 (1 \, bar) + 2AgCl_{(s)} \rightleftharpoons 2Ag_{(s)} + 2H^{+} (0.1 \, M) + 2Cl^{-} (0.1 \, M)$,$\Delta G^o = -48,250 \, J$ at $25 \, ^oC$. The standard emf of cell in which the given reaction takes place is ................. $V$

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$A$ galvanic cell consists of a copper electrode and a standard hydrogen electrode. If $E^0_{(Cu^{2+}(aq)|Cu(s))} = +0.34 \text{ V}$, identify the reaction taking place at the positive electrode during the working of the cell.

Similar Questions

The standard oxidation potentials of zinc and silver in water at $298 \ K$ are:$Zn_{(s)} \to Zn^{2+}_{(aq)} + 2e^- ; E^o_{ox} = 0.76 \ V$$Ag_{(s)} \to Ag^{+}_{(aq)} + e^- ; E^o_{ox} = -0.80 \ V$Which of the following reactions actually takes place spontaneously?

Arrange the following metals in the order in which they displace each other from the solution of their salts: $Al, Cu, Fe, Mg$ and $Zn$.

For the cell reaction:$2 Fe^{3+}_{(aq)} + 2 I^{-}_{(aq)} \rightarrow 2 Fe^{2+}_{(aq)} + I_{2(aq)}$$E^{\ominus}_{cell} = 0.24 \ V$ at $298 \ K$. The standard Gibbs energy $(\Delta_r G^{\ominus})$ of the cell reaction in $kJ \ mol^{-1}$ is:[Faraday constant $F = 96500 \ C \ mol^{-1}$]

If standard reduction potentials $(E^0)$ of $(Al^{+3}(aq)|Al(s))$, $(Fe^{+2}(aq)|Fe(s))$, $(Cu^{+2}(aq)|Cu(s))$ and $(Ag^{+1}(aq)|Ag(s))$ are $-1.66 \text{ V}$, $-0.44 \text{ V}$, $+0.34 \text{ V}$ and $+0.79 \text{ V}$ respectively, which of the following reactions is non-spontaneous?

For the reaction $H_2 (1 \, bar) + 2AgCl_{(s)} \rightleftharpoons 2Ag_{(s)} + 2H^{+} (0.1 \, M) + 2Cl^{-} (0.1 \, M)$,$\Delta G^o = -48,250 \, J$ at $25 \, ^oC$. The standard emf of cell in which the given reaction takes place is ................. $V$

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The standard oxidation potentials of zinc and silver in water at $298 \ K$ are:
$Zn_{(s)} \to Zn^{2+}_{(aq)} + 2e^- ; E^o_{ox} = 0.76 \ V$
$Ag_{(s)} \to Ag^{+}_{(aq)} + e^- ; E^o_{ox} = -0.80 \ V$
Which of the following reactions actually takes place spontaneously?

For the cell reaction:
$2 Fe^{3+}_{(aq)} + 2 I^{-}_{(aq)} \rightarrow 2 Fe^{2+}_{(aq)} + I_{2(aq)}$
$E^{\ominus}_{cell} = 0.24 \ V$ at $298 \ K$. The standard Gibbs energy $(\Delta_r G^{\ominus})$ of the cell reaction in $kJ \ mol^{-1}$ is:
[Faraday constant $F = 96500 \ C \ mol^{-1}$]