(B) $1$. In a galvanic cell, the electrode with the higher reduction potential acts as the cathode (positive electrode).$2$. The standard reduction po

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$Cu^{2+}_{(aq)} + 2e^- \longrightarrow Cu_{(s)}$

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

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

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

MHT CET 2026 All MHT CET

A
$Cu_{(s)} \longrightarrow Cu^{2+}_{(aq)} + 2e^-$
B
$Cu^{2+}_{(aq)} + 2e^- \longrightarrow Cu_{(s)}$
C
$H_2(g) \longrightarrow 2H^+_{(aq)} + 2e^-$
D
$H^+_{(aq)} + 2e^- \longrightarrow H_2(g)$

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Discuss the method to determine the cell potential of any cell when a standard hydrogen electrode is considered as the cathode with a suitable example.

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For the reaction $M^{+n}_{(aq)} + ne^{-} \rightarrow M_{(s)}$,if the standard reduction potentials of elements $M_1, M_2$,and $M_3$ are $-0.34 \ V$,$-3.05 \ V$,and $-1.66 \ V$ respectively,what is the order of their reducing strength?

Easy

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Which one among the following is the strongest reducing agent?
$Fe^{2+} + 2e^- \to Fe \ (E^\circ = -0.44 \ V)$
$Ni^{2+} + 2e^- \to Ni \ (E^\circ = -0.25 \ V)$
$Sn^{2+} + 2e^- \to Sn \ (E^\circ = -0.14 \ V)$
$Fe^{3+} + e^- \to Fe^{2+} \ (E^\circ = +0.77 \ V)$

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What is the oxidation and reduction potential of standard hydrogen electrode?

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For $Mg^{2+} + 2e^{-} \rightarrow Mg_{(s)}$,$E^{0} = -2.37 \, V$ and for $Cu^{2+} + 2e^{-} \rightarrow Cu_{(s)}$,$E^{0} = +0.33 \, V$. The $emf$ of the cell $(E^{0}_{Cell})$ is .......... $V$.

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

Similar Questions

Discuss the method to determine the cell potential of any cell when a standard hydrogen electrode is considered as the cathode with a suitable example.

For the reaction $M^{+n}_{(aq)} + ne^{-} \rightarrow M_{(s)}$,if the standard reduction potentials of elements $M_1, M_2$,and $M_3$ are $-0.34 \ V$,$-3.05 \ V$,and $-1.66 \ V$ respectively,what is the order of their reducing strength?

Which one among the following is the strongest reducing agent?$Fe^{2+} + 2e^- \to Fe \ (E^\circ = -0.44 \ V)$$Ni^{2+} + 2e^- \to Ni \ (E^\circ = -0.25 \ V)$$Sn^{2+} + 2e^- \to Sn \ (E^\circ = -0.14 \ V)$$Fe^{3+} + e^- \to Fe^{2+} \ (E^\circ = +0.77 \ V)$

What is the oxidation and reduction potential of standard hydrogen electrode?

For $Mg^{2+} + 2e^{-} \rightarrow Mg_{(s)}$,$E^{0} = -2.37 \, V$ and for $Cu^{2+} + 2e^{-} \rightarrow Cu_{(s)}$,$E^{0} = +0.33 \, V$. The $emf$ of the cell $(E^{0}_{Cell})$ is .......... $V$.

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Which one among the following is the strongest reducing agent?
$Fe^{2+} + 2e^- \to Fe \ (E^\circ = -0.44 \ V)$
$Ni^{2+} + 2e^- \to Ni \ (E^\circ = -0.25 \ V)$
$Sn^{2+} + 2e^- \to Sn \ (E^\circ = -0.14 \ V)$
$Fe^{3+} + e^- \to Fe^{2+} \ (E^\circ = +0.77 \ V)$