(A) The cell potential $E^o_{cell}$ is calculated as $E^o_{cell} = E^o_{cathode} - E^o_{anode}$.To obtain the maximum potential,we must choose the hal

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(A) The cell potential $E^o_{cell}$ is calculated as $E^o_{cell} = E^o_{cathode} - E^o_{anode}$.To obtain the maximum potential,we must choose the half-cell with the highest reduction potential as the cathode and the half-cell with the lowest reduction potential as the anode.Comparing the given values:$E^o_{(i)} = -0.24 \ V$$E^o_{(ii)} = +1.25 \ V$ (Highest)$E^o_{(iii)} = -1.25 \ V$ (Lowest)$E^o_{(iv)} = +0.68 \ V$Thus,the cathode is $(ii)$ and the anode is $(iii)$.$E^o_{cell} = 1.25 - (-1.25) = 2.50 \ V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Easy

The $E^o$ values of half-cells are given below. Which combination of two half-cells will form a cell with the maximum potential?
$(i)$ $A + e^- \rightarrow A^- ; E^o = -0.24 \ V$
$(ii)$ $B^- + e^- \rightarrow B^{2-} ; E^o = +1.25 \ V$
$(iii)$ $C^- + 2e^- \rightarrow C^{3-} ; E^o = -1.25 \ V$
$(iv)$ $D + 2e^- \rightarrow D^{2-} ; E^o = +0.68 \ V$

A
$(ii)$ and $(iii)$
B
$(ii)$ and $(iv)$
C
$(i)$ and $(iii)$
D
$(i)$ and $(iv)$

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Class 12

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Electrochemistry

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Electrode potential and ECell

Which of the following metals will not reduce $H_2O$?

Medium

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The standard oxidation potentials for the half-reactions are given as $Zn \to Zn^{2+} + 2e^{-}; E^o = +0.76 \ V$ and $Fe \to Fe^{2+} + 2e^{-}; E^o = +0.41 \ V$. The $EMF$ for the cell reaction $Fe^{2+} + Zn \to Zn^{2+} + Fe$ is ............ $V$.

MediumAIIMS 2001

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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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$E^o$ values for the half-cell reactions are given below:
$Cu^{2+} + e^- \to Cu^{+} \quad E^o = 0.15 \ V$
$Cu^{2+} + 2e^- \to Cu \quad E^o = 0.34 \ V$
What will be the $E^o$ for the half-cell reaction:
$Cu^{+} + e^- \to Cu$ ? $\dots \ V$

Medium

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What is the standard cell potential for the cell $Zn | Zn^{2+} (1M) || Cu^{2+} (1M) | Cu$? Given $E^o$ for $Zn^{2+} | Zn = -0.76 \ V$ and $E^o$ for $Cu^{2+} | Cu = +0.34 \ V$.

MediumAIIMS 1980

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Which of the following metals will not reduce $H_2O$?

The standard oxidation potentials for the half-reactions are given as $Zn \to Zn^{2+} + 2e^{-}; E^o = +0.76 \ V$ and $Fe \to Fe^{2+} + 2e^{-}; E^o = +0.41 \ V$. The $EMF$ for the cell reaction $Fe^{2+} + Zn \to Zn^{2+} + Fe$ is ............ $V$.

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

$E^o$ values for the half-cell reactions are given below:$Cu^{2+} + e^- \to Cu^{+} \quad E^o = 0.15 \ V$$Cu^{2+} + 2e^- \to Cu \quad E^o = 0.34 \ V$What will be the $E^o$ for the half-cell reaction:$Cu^{+} + e^- \to Cu$ ? $\dots \ V$

What is the standard cell potential for the cell $Zn | Zn^{2+} (1M) || Cu^{2+} (1M) | Cu$? Given $E^o$ for $Zn^{2+} | Zn = -0.76 \ V$ and $E^o$ for $Cu^{2+} | Cu = +0.34 \ V$.

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$E^o$ values for the half-cell reactions are given below:
$Cu^{2+} + e^- \to Cu^{+} \quad E^o = 0.15 \ V$
$Cu^{2+} + 2e^- \to Cu \quad E^o = 0.34 \ V$
What will be the $E^o$ for the half-cell reaction:
$Cu^{+} + e^- \to Cu$ ? $\dots \ V$