(C) The cell reaction is $2Fe^{3+} + 2I^{-} \to 2Fe^{2+} + I_2$.Here,$Fe^{3+}$ is reduced to $Fe^{2+}$ (cathode) and $I^{-}$ is oxidized to $I_2$ (ano

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(C) The cell reaction is $2Fe^{3+} + 2I^{-} \to 2Fe^{2+} + I_2$.Here,$Fe^{3+}$ is reduced to $Fe^{2+}$ (cathode) and $I^{-}$ is oxidized to $I_2$ (anode).$E^o_{\text{cell}} = E^o_{\text{cathode}} - E^o_{\text{anode}}$$E^o_{\text{cell}} = E^o_{Fe^{3+}/Fe^{2+}} - E^o_{I_2/I^{-}}$$E^o_{\text{cell}} = 0.771 \ V - 0.536 \ V = 0.235 \ V$

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Difficult

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

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Electrochemistry

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Electrode potential and ECell

The reaction $Zn^{2+} + 2e^{-} \to Zn$ has a standard electrode potential of $-0.76 \ V$. This means:

Easy

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For the reaction $F_2 + 2e^{-} \to 2F^{-}$,$E^{\circ} = 2.8 \, V$. What is the $E^{\circ}$ for the reaction $\frac{1}{2} F_2 + e^{-} \to F^{-}$?

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Given the following standard electrode potentials:
$Cu^{+2} + 2e^{-} \to Cu$,$E^{o} = X_{1}$
$Cu^{+} + e^{-} \to Cu$,$E^{o} = X_{2}$
Calculate the standard electrode potential $E^{o}$ for the reaction: $Cu^{+2} + e^{-} \to Cu^{+}$

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Which of the following expressions is correct for the standard Gibbs free energy change?

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Which of the following has been universally accepted as a reference electrode at all temperatures and has been assigned a value of zero volt?

EasyAIIMS 1998

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

Similar Questions

The reaction $Zn^{2+} + 2e^{-} \to Zn$ has a standard electrode potential of $-0.76 \ V$. This means:

For the reaction $F_2 + 2e^{-} \to 2F^{-}$,$E^{\circ} = 2.8 \, V$. What is the $E^{\circ}$ for the reaction $\frac{1}{2} F_2 + e^{-} \to F^{-}$?

Given the following standard electrode potentials:$Cu^{+2} + 2e^{-} \to Cu$,$E^{o} = X_{1}$$Cu^{+} + e^{-} \to Cu$,$E^{o} = X_{2}$Calculate the standard electrode potential $E^{o}$ for the reaction: $Cu^{+2} + e^{-} \to Cu^{+}$

Which of the following expressions is correct for the standard Gibbs free energy change?

Which of the following has been universally accepted as a reference electrode at all temperatures and has been assigned a value of zero volt?

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

Given the following standard electrode potentials:
$Cu^{+2} + 2e^{-} \to Cu$,$E^{o} = X_{1}$
$Cu^{+} + e^{-} \to Cu$,$E^{o} = X_{2}$
Calculate the standard electrode potential $E^{o}$ for the reaction: $Cu^{+2} + e^{-} \to Cu^{+}$