(D) The cell reaction involves $Mg$ acting as the anode and $Cu$ acting as the cathode because $Mg$ is a stronger reducing agent than $Cu$. $E_{cell}^

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(D) The cell reaction involves $Mg$ acting as the anode and $Cu$ acting as the cathode because $Mg$ is a stronger reducing agent than $Cu$. $E_{cell}^o = E_{cathode}^o - E_{anode}^o$ $E_{cell}^o = E_{Cu^{+2}/Cu}^o - E_{Mg^{+2}/Mg}^o$ Given $E_{cell}^o = 2.7 \ V$ and $E_{Cu^{+2}/Cu}^o = 0.34 \ V$. $2.7 \ V = 0.34 \ V - E_{Mg^{+2}/Mg}^o$ $E_{Mg^{+2}/Mg}^o = 0.34 \ V - 2.7 \ V = -2.36 \ V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

$A$ 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 .............. $V$.

A
$+3.04$
B
$-3.04$
C
$+2.36$
D
$-2.36$

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Electrode potential and ECell

What is the relationship between Gibbs free energy of the cell reaction in a galvanic cell and the emf of the cell? When will the maximum work be obtained from a galvanic cell?

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Given are $E^o$ values for some half reactions:
$I_2 + 2e^- \to 2I^{-}; E^o = 0.54 \ V$
$MnO_4^- + 8H^{+} + 5e^- \to Mn^{2+} + 4H_2O; E^o = 1.52 \ V$
$Fe^{3+} + e^- \to Fe^{2+}; E^o = 0.77 \ V$
$Sn^{4+} + 2e^- \to Sn^{2+}; E^o = 0.1 \ V$
The strongest reducant and oxidant respectively are:

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$A$ standard hydrogen electrode has zero electrode potential because

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The standard reduction potential $E^{\circ}$ for half reactions are
$Zn \rightarrow Zn^{2+} + 2e^-$ $E^{\circ} = +0.76 \ V$
$Fe \rightarrow Fe^{2+} + 2e^-$ $E^{\circ} = +0.41 \ V$

The $EMF$ of the cell reaction $Fe^{2+} + Zn \rightarrow Zn^{2+} + Fe$ is

MediumWBJEE 2011

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The relation between $\Delta G$ and $E$ for a cell is $\Delta G = -nFE$. The cell reaction will be spontaneous if:

Easy

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$Zn \rightarrow Zn^{2+} + 2e^-$	$E^{\circ} = +0.76 \ V$
$Fe \rightarrow Fe^{2+} + 2e^-$	$E^{\circ} = +0.41 \ V$

$A$ 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 .............. $V$.

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What is the relationship between Gibbs free energy of the cell reaction in a galvanic cell and the emf of the cell? When will the maximum work be obtained from a galvanic cell?

Given are $E^o$ values for some half reactions:$I_2 + 2e^- \to 2I^{-}; E^o = 0.54 \ V$$MnO_4^- + 8H^{+} + 5e^- \to Mn^{2+} + 4H_2O; E^o = 1.52 \ V$$Fe^{3+} + e^- \to Fe^{2+}; E^o = 0.77 \ V$$Sn^{4+} + 2e^- \to Sn^{2+}; E^o = 0.1 \ V$The strongest reducant and oxidant respectively are:

$A$ standard hydrogen electrode has zero electrode potential because

The standard reduction potential $E^{\circ}$ for half reactions are$Zn \rightarrow Zn^{2+} + 2e^-$$E^{\circ} = +0.76 \ V$$Fe \rightarrow Fe^{2+} + 2e^-$$E^{\circ} = +0.41 \ V$The $EMF$ of the cell reaction $Fe^{2+} + Zn \rightarrow Zn^{2+} + Fe$ is

The relation between $\Delta G$ and $E$ for a cell is $\Delta G = -nFE$. The cell reaction will be spontaneous if:

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Given are $E^o$ values for some half reactions:
$I_2 + 2e^- \to 2I^{-}; E^o = 0.54 \ V$
$MnO_4^- + 8H^{+} + 5e^- \to Mn^{2+} + 4H_2O; E^o = 1.52 \ V$
$Fe^{3+} + e^- \to Fe^{2+}; E^o = 0.77 \ V$
$Sn^{4+} + 2e^- \to Sn^{2+}; E^o = 0.1 \ V$
The strongest reducant and oxidant respectively are:

The standard reduction potential $E^{\circ}$ for half reactions are
$Zn \rightarrow Zn^{2+} + 2e^-$ $E^{\circ} = +0.76 \ V$
$Fe \rightarrow Fe^{2+} + 2e^-$ $E^{\circ} = +0.41 \ V$

The $EMF$ of the cell reaction $Fe^{2+} + Zn \rightarrow Zn^{2+} + Fe$ is