(A) The cell reaction is: $2Fe^{3+} + 2I^- \to 2Fe^{2+} + I_2$.This reaction consists of two half-reactions:Cathode (Reduction): $2Fe^{3+} + 2e^- \to

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(A) The cell reaction is: $2Fe^{3+} + 2I^- \to 2Fe^{2+} + I_2$.This reaction consists of two half-reactions:Cathode (Reduction): $2Fe^{3+} + 2e^- \to 2Fe^{2+}$; $E^o_{\text{cathode}} = 0.771 \, V$.Anode (Oxidation): $2I^- \to I_2 + 2e^-$; $E^o_{\text{anode}} = 0.536 \, V$.$E^o_{\text{cell}} = E^o_{\text{cathode}} - E^o_{\text{anode}}$.$E^o_{\text{cell}} = 0.771 \, V - 0.536 \, V = 0.235 \, V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

Given electrode potentials:
$Fe^{3+} + e^- \to Fe^{2+}$; $E^o = 0.771 \, V$
$I_2 + 2e^- \to 2I^-$; $E^o = 0.536 \, V$
$E^o_{\text{cell}}$ for the cell reaction
$2Fe^{3+} + 2I^- \to 2Fe^{2+} + I_2$ is:

A
$0.771 - 0.536 = 0.235 \, V$
B
$0.536 - 0.771 = -0.235 \, V$
C
$2 \times 0.771 - 0.536 = 1.006 \, V$
D
$0.771 + 0.536 = 1.307 \, V$

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Electrochemistry

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Electrode potential and ECell

The $E^{\circ}$ of $Ce^{4+} / Ce^{3+} = 1.6 \ V$ and $Fe^{3+} / Fe^{2+} = 0.77 \ V$. The $E^{\circ}$ of the reaction where $Fe^{3+}$ oxidises $Ce^{3+}$ is:

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Calculate the $E_{cell}^o$ for $Zn_{(s)}|Zn_{(1M)}^{2+}| |Cd_{(1M)}^{2+}|Cd_{(s)}$ at $25^{\circ} C$ given that $E_{Zn^{2+}/Zn}^{\circ} = -0.763 \ V$ and $E_{Cd^{2+}/Cd}^{\circ} = -0.403 \ V$. (in $V$)

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

Medium

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$Cr_2O_7^{2-} + I^{-} \to I_2 + Cr^{3+}$
$E^0_{cell} = 0.79 \ V$
$E^0_{Cr_2O_7^{2-}} = 1.33 \ V$,$E^0_{I_2}$ is ........... $V$

Medium

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Calculate the standard cell potential for a cell having the following reaction: $2 Al_{(s)} + 3 Ni^{2+} \rightarrow 2 Al^{3+} + 3 Ni_{(s)}$ given that $E_{Ni^{2+}/Ni}^{\circ} = -0.25 \ V$ and $E_{Al^{3+}/Al}^{\circ} = -1.66 \ V$. (in $V$)

EasyMHT CET 2022

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Given electrode potentials:$Fe^{3+} + e^- \to Fe^{2+}$; $E^o = 0.771 \, V$$I_2 + 2e^- \to 2I^-$; $E^o = 0.536 \, V$$E^o_{\text{cell}}$ for the cell reaction$2Fe^{3+} + 2I^- \to 2Fe^{2+} + I_2$ is:

Similar Questions

The $E^{\circ}$ of $Ce^{4+} / Ce^{3+} = 1.6 \ V$ and $Fe^{3+} / Fe^{2+} = 0.77 \ V$. The $E^{\circ}$ of the reaction where $Fe^{3+}$ oxidises $Ce^{3+}$ is:

Calculate the $E_{cell}^o$ for $Zn_{(s)}|Zn_{(1M)}^{2+}| |Cd_{(1M)}^{2+}|Cd_{(s)}$ at $25^{\circ} C$ given that $E_{Zn^{2+}/Zn}^{\circ} = -0.763 \ V$ and $E_{Cd^{2+}/Cd}^{\circ} = -0.403 \ V$. (in $V$)

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)$

$Cr_2O_7^{2-} + I^{-} \to I_2 + Cr^{3+}$$E^0_{cell} = 0.79 \ V$$E^0_{Cr_2O_7^{2-}} = 1.33 \ V$,$E^0_{I_2}$ is ........... $V$

Calculate the standard cell potential for a cell having the following reaction: $2 Al_{(s)} + 3 Ni^{2+} \rightarrow 2 Al^{3+} + 3 Ni_{(s)}$ given that $E_{Ni^{2+}/Ni}^{\circ} = -0.25 \ V$ and $E_{Al^{3+}/Al}^{\circ} = -1.66 \ V$. (in $V$)

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Given electrode potentials:
$Fe^{3+} + e^- \to Fe^{2+}$; $E^o = 0.771 \, V$
$I_2 + 2e^- \to 2I^-$; $E^o = 0.536 \, V$
$E^o_{\text{cell}}$ for the cell reaction
$2Fe^{3+} + 2I^- \to 2Fe^{2+} + I_2$ is:

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

$Cr_2O_7^{2-} + I^{-} \to I_2 + Cr^{3+}$
$E^0_{cell} = 0.79 \ V$
$E^0_{Cr_2O_7^{2-}} = 1.33 \ V$,$E^0_{I_2}$ is ........... $V$