(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

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Electrochemistry

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Electrode potential and ECell

Fill in the blanks :
$1$. ...... metal is the strongest reducing agent in aqueous solution.
$2$. ...... gas is the strongest oxidizing agent.
$3$. The standard reduction potential of any electrode is measured with reference to ......

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Calculate $E_{\text{cell}}^{\circ}$ for the reaction: $Mg_{(s)} + 2 Ag_{(aq)}^{+} \rightarrow Mg_{(aq)}^{2+} + 2 Ag_{(s)}$,given that $E_{Ag^{+}/Ag}^{\circ} = 0.8 \ V$ and $E_{Mg^{2+}/Mg}^{\circ} = -2.37 \ V$. (in $V$)

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Standard electrode potential of $NHE$ at $298\,K$ is .............. $V$.

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When a $Zn$ piece is kept in a $CuSO_4$ solution,the copper gets precipitated because the standard reduction potential of zinc is

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Given $E_{Fe^{+3}/Fe}^{\circ} = -0.036 \ V$ and $E_{Fe^{+2}/Fe}^{\circ} = -0.439 \ V$,calculate the standard electrode potential for the reaction: $Fe^{+3}_{(aq)} + e^{-} \rightarrow Fe^{+2}_{(aq)}$ (in $V$)

Medium

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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:

Similar Questions

Fill in the blanks :$1$. ...... metal is the strongest reducing agent in aqueous solution.$2$. ...... gas is the strongest oxidizing agent.$3$. The standard reduction potential of any electrode is measured with reference to ......

Calculate $E_{\text{cell}}^{\circ}$ for the reaction: $Mg_{(s)} + 2 Ag_{(aq)}^{+} \rightarrow Mg_{(aq)}^{2+} + 2 Ag_{(s)}$,given that $E_{Ag^{+}/Ag}^{\circ} = 0.8 \ V$ and $E_{Mg^{2+}/Mg}^{\circ} = -2.37 \ V$. (in $V$)

Standard electrode potential of $NHE$ at $298\,K$ is .............. $V$.

When a $Zn$ piece is kept in a $CuSO_4$ solution,the copper gets precipitated because the standard reduction potential of zinc is

Given $E_{Fe^{+3}/Fe}^{\circ} = -0.036 \ V$ and $E_{Fe^{+2}/Fe}^{\circ} = -0.439 \ V$,calculate the standard electrode potential for the reaction: $Fe^{+3}_{(aq)} + e^{-} \rightarrow Fe^{+2}_{(aq)}$ (in $V$)

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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:

Fill in the blanks :
$1$. ...... metal is the strongest reducing agent in aqueous solution.
$2$. ...... gas is the strongest oxidizing agent.
$3$. The standard reduction potential of any electrode is measured with reference to ......