(C) The cell reaction is: $2Fe^{3+} + 2I^- \to 2Fe^{2+} + I_2$Reduction half-reaction: $2Fe^{3+} + 2e^- \to 2Fe^{2+}$; $E^o_{red} = 0.771 \, V$Oxidati

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(C) The cell reaction is: $2Fe^{3+} + 2I^- \to 2Fe^{2+} + I_2$Reduction half-reaction: $2Fe^{3+} + 2e^- \to 2Fe^{2+}$; $E^o_{red} = 0.771 \, V$Oxidation half-reaction: $2I^- \to I_2 + 2e^-$; $E^o_{ox} = -E^o_{red} = -0.536 \, V$$E^o_{cell} = E^o_{red} + E^o_{ox} = 0.771 \, V + (-0.536 \, V) = 0.235 \, V$

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

The electrode potentials are given as follows:
$Fe_{(aq)}^{3+} + e^- \to Fe_{(aq)}^{2+}$; $E^o = 0.771 \, V$
$I_{2(s)} + 2e^- \to 2I_{(aq)}^-$; $E^o = 0.536 \, V$
For the cell reaction $2Fe_{(aq)}^{3+} + 2I_{(aq)}^- \to 2Fe_{(aq)}^{2+} + I_{2(s)}$,the value of $E^o_{cell}$ is:

A
$(2 \times 0.771 - 0.536) = 1.006 \, V$
B
$(0.771 - 0.5 \times 0.536) = 0.503 \, V$
C
$0.771 - 0.536 = 0.235 \, V$
D
$0.536 - 0.771 = -0.235 \, V$

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Class 12 Questions

Class 12

Chemistry Questions

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Electrochemistry

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Electrode potential and ECell

The standard reduction potentials for $Zn^{2+}/Zn$,$Ni^{2+}/Ni$,and $Fe^{2+}/Fe$ are $-0.76 \, V$,$-0.23 \, V$,and $-0.44 \, V$ respectively. For which of the following combinations will the reaction $X + Y^{2+} \rightarrow X^{2+} + Y$ be spontaneous?

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Aluminium displaces hydrogen from dilute $HCl$ whereas silver does not. The e.m.f. of a cell prepared by combining $Al/Al^{3+}$ and $Ag/Ag^{+}$ is $2.46 \ V$. The reduction potential of silver electrode is $+0.80 \ V$. The reduction potential of aluminium electrode is $........... \ V$.

Medium

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Which reference electrode is used to measure the electrode potential of other electrodes?

Medium

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$E^{\circ}_{Fe^{2+}/Fe} = -0.441 \ V$ and $E^{\circ}_{Fe^{3+}/Fe^{2+}} = 0.771 \ V$,the standard $EMF$ of the reaction $Fe + 2Fe^{3+} \rightarrow 3Fe^{2+}$ will be $.......... \ V$.

AIPMT 2006

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

The electrode potentials are given as follows:$Fe_{(aq)}^{3+} + e^- \to Fe_{(aq)}^{2+}$; $E^o = 0.771 \, V$$I_{2(s)} + 2e^- \to 2I_{(aq)}^-$; $E^o = 0.536 \, V$For the cell reaction $2Fe_{(aq)}^{3+} + 2I_{(aq)}^- \to 2Fe_{(aq)}^{2+} + I_{2(s)}$,the value of $E^o_{cell}$ is:

Similar Questions

The standard reduction potentials for $Zn^{2+}/Zn$,$Ni^{2+}/Ni$,and $Fe^{2+}/Fe$ are $-0.76 \, V$,$-0.23 \, V$,and $-0.44 \, V$ respectively. For which of the following combinations will the reaction $X + Y^{2+} \rightarrow X^{2+} + Y$ be spontaneous?

Aluminium displaces hydrogen from dilute $HCl$ whereas silver does not. The e.m.f. of a cell prepared by combining $Al/Al^{3+}$ and $Ag/Ag^{+}$ is $2.46 \ V$. The reduction potential of silver electrode is $+0.80 \ V$. The reduction potential of aluminium electrode is $........... \ V$.

Which reference electrode is used to measure the electrode potential of other electrodes?

$E^{\circ}_{Fe^{2+}/Fe} = -0.441 \ V$ and $E^{\circ}_{Fe^{3+}/Fe^{2+}} = 0.771 \ V$,the standard $EMF$ of the reaction $Fe + 2Fe^{3+} \rightarrow 3Fe^{2+}$ will be $.......... \ V$.

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

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The electrode potentials are given as follows:
$Fe_{(aq)}^{3+} + e^- \to Fe_{(aq)}^{2+}$; $E^o = 0.771 \, V$
$I_{2(s)} + 2e^- \to 2I_{(aq)}^-$; $E^o = 0.536 \, V$
For the cell reaction $2Fe_{(aq)}^{3+} + 2I_{(aq)}^- \to 2Fe_{(aq)}^{2+} + I_{2(s)}$,the value of $E^o_{cell}$ is:

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