(A) The electrode with the higher standard reduction potential acts as the cathode. Given standard reduction potentials: $E_{Ag^+/Ag}^{\circ} = +0.80

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Copper electrode acts as anode and $E_{cell}^{\circ}$ is $+0.46 \ V$

(A) The electrode with the higher standard reduction potential acts as the cathode. Given standard reduction potentials: $E_{Ag^+/Ag}^{\circ} = +0.80 \ V$ and $E_{Cu^{2+}/Cu}^{\circ} = +0.34 \ V$. Since $E_{Ag^+/Ag}^{\circ} > E_{Cu^{2+}/Cu}^{\circ}$,the silver electrode acts as the cathode and the copper electrode acts as the anode. The standard cell potential is calculated as: $E_{cell}^{\circ} = E_{cathode}^{\circ} - E_{anode}^{\circ}$ $E_{cell}^{\circ} = +0.80 \ V - (+0.34 \ V) = +0.46 \ V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

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For a cell constructed with $Cu$ and $Ag$ electrodes,which of the following statements is correct regarding the cathode and the standard cell potential $(E_{cell}^{\circ})$?

TS EAMCET 2020 All TS EAMCET

A
Copper electrode acts as anode and $E_{cell}^{\circ}$ is $+0.46 \ V$
B
Copper electrode acts as anode and $E_{cell}^{\circ}$ is $-0.46 \ V$
C
Silver electrode acts as a cathode and $E_{cell}^{\circ}$ is $-0.34 \ V$
D
Copper electrode acts as cathode and $E_{cell}^{\circ}$ is $+0.46 \ V$

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Electrode potential and ECell

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If the cell potential of the cell at $298 \ K$ is $2.36 \ V$,write the cell reaction and calculate the standard electrode potential of the $Mg^{2+} \mid Mg$ half-cell.
$Mg_{(s)} \mid Mg^{2+}_{(1 \ M)} \parallel H^{+}_{(1 \ M)} \mid H_{2(g)} (1 \ bar) \mid Pt_{(s)}$

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What is the standard reduction potential of $Cu^{2+} \mid Cu_{(s)}$ if the $E^{\circ}$ of the following cell is $0.46 \ V$ (in $V$)?
$Cu_{(s)} \mid Cu_{(aq)}^{2+} \parallel Ag_{(aq)}^{+} \mid Ag_{(s)}$ ; $E_{Ag^{+} / Ag}^{\circ} = 0.80 \ V$

MediumMHT CET 2022

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Can $E_{cell}^o$ or $\Delta_r G^o$ for a cell reaction ever be equal to zero?

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$A$ cell constructed by coupling a standard copper electrode and a standard magnesium electrode has an $emf$ of $2.7 \ V$. If the standard reduction potential of the copper electrode is $+0.34 \ V$,the standard reduction potential of the magnesium electrode is .............. $V$.

Medium

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Which of the following metals does not liberate $\text{H}_2$ gas by reacting with $\text{HCl}$?

MediumGUJCET 2026

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For a cell constructed with $Cu$ and $Ag$ electrodes,which of the following statements is correct regarding the cathode and the standard cell potential $(E_{cell}^{\circ})$?

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If the cell potential of the cell at $298 \ K$ is $2.36 \ V$,write the cell reaction and calculate the standard electrode potential of the $Mg^{2+} \mid Mg$ half-cell.$Mg_{(s)} \mid Mg^{2+}_{(1 \ M)} \parallel H^{+}_{(1 \ M)} \mid H_{2(g)} (1 \ bar) \mid Pt_{(s)}$

What is the standard reduction potential of $Cu^{2+} \mid Cu_{(s)}$ if the $E^{\circ}$ of the following cell is $0.46 \ V$ (in $V$)?$Cu_{(s)} \mid Cu_{(aq)}^{2+} \parallel Ag_{(aq)}^{+} \mid Ag_{(s)}$ ; $E_{Ag^{+} / Ag}^{\circ} = 0.80 \ V$

Can $E_{cell}^o$ or $\Delta_r G^o$ for a cell reaction ever be equal to zero?

$A$ cell constructed by coupling a standard copper electrode and a standard magnesium electrode has an $emf$ of $2.7 \ V$. If the standard reduction potential of the copper electrode is $+0.34 \ V$,the standard reduction potential of the magnesium electrode is .............. $V$.

Which of the following metals does not liberate $\text{H}_2$ gas by reacting with $\text{HCl}$?

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If the cell potential of the cell at $298 \ K$ is $2.36 \ V$,write the cell reaction and calculate the standard electrode potential of the $Mg^{2+} \mid Mg$ half-cell.
$Mg_{(s)} \mid Mg^{2+}_{(1 \ M)} \parallel H^{+}_{(1 \ M)} \mid H_{2(g)} (1 \ bar) \mid Pt_{(s)}$

What is the standard reduction potential of $Cu^{2+} \mid Cu_{(s)}$ if the $E^{\circ}$ of the following cell is $0.46 \ V$ (in $V$)?
$Cu_{(s)} \mid Cu_{(aq)}^{2+} \parallel Ag_{(aq)}^{+} \mid Ag_{(s)}$ ; $E_{Ag^{+} / Ag}^{\circ} = 0.80 \ V$