(A) reaction is spontaneous if $E^0_{cell} > 0$. $E^0_{cell} = E^0_{cathode} - E^0_{anode}$.For $(A)$: $E^0_{cell} = (-0.403) - (-2.866) = +2.463 \tex

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$Ca(s) + Cd^{2+}(aq) \rightarrow Ca^{2+}(aq) + Cd(s)$ $[E^0_{Ca^{2+}/Ca} = -2.866 \text{ V}, E^0_{Cd^{2+}/Cd} = -0.403 \text{ V}]$

(A) reaction is spontaneous if $E^0_{cell} > 0$. $E^0_{cell} = E^0_{cathode} - E^0_{anode}$.For $(A)$: $E^0_{cell} = (-0.403) - (-2.866) = +2.463 \text{ V}$. Since $E^0_{cell} > 0$, it is spontaneous.For $(B)$: $E^0_{cell} = (-0.136) - (1.08) = -1.216 \text{ V}$. Non-spontaneous.For $(C)$: $E^0_{cell} = (-0.257) - (0.799) = -1.056 \text{ V}$. Non-spontaneous.For $(D)$: $E^0_{cell} = (-0.763) - (1.68) = -2.443 \text{ V}$. Non-spontaneous.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Difficult

Identify which of the following cell reactions is spontaneous under standard state conditions.

MHT CET 2026 All MHT CET

A
$Ca(s) + Cd^{2+}(aq) \rightarrow Ca^{2+}(aq) + Cd(s)$ $[E^0_{Ca^{2+}/Ca} = -2.866 \text{ V}, E^0_{Cd^{2+}/Cd} = -0.403 \text{ V}]$
B
$2Br^-(aq) + Sn^{2+}(aq) \rightarrow Br_2(l) + Sn(s)$ $[E^0_{Br_2/Br^-} = 1.08 \text{ V}, E^0_{Sn^{2+}/Sn} = -0.136 \text{ V}]$
C
$2Ag(s) + Ni^{2+}(aq) \rightarrow 2Ag^+(aq) + Ni(s)$ $[E^0_{Ag^+/Ag} = 0.799 \text{ V}, E^0_{Ni^{2+}/Ni} = -0.257 \text{ V}]$
D
$2Au(s) + Zn^{2+}(aq) \rightarrow 2Au^+(aq) + Zn(s)$ $[E^0_{Au^+/Au} = 1.68 \text{ V}, E^0_{Zn^{2+}/Zn} = -0.763 \text{ V}]$

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Electrochemistry

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Electrode potential and ECell

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MHT CET 2026 Paper All MHT CET years →

For the reaction $Cr_2O_7^{2-} + I^- \to I_2 + Cr^{3+}$,if $E_{cell}^o = 0.79 \ V$ and $E_{Cr_2O_7^{2-}}^o = 1.33 \ V$,then $E_{I_2}^o = $ ............. $V$.

Medium

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Which of the following metals does not liberate $\text{H}_2$ gas by reacting with $\text{HCl}$?

MediumGUJCET 2026

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Given,the standard potentials $E_{(Cu^{2+}/Cu)}^{\circ}$ and $E_{(Cu^{+}/Cu)}^{\circ}$ as $0.340 \ V$ and $0.522 \ V$ respectively,the value of $E_{(Cu^{2+}/Cu^{+})}^{\circ}$ is $.... \ V$

MediumKVPY 2016

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Reduction potential of ions are given below:

$ClO_4^{-}$ $E^{\circ} = 1.19 \ V$

$IO_4^{-}$ $E^{\circ} = 1.65 \ V$

$BrO_4^{-}$ $E^{\circ} = 1.74 \ V$

The correct order of their oxidising power is:

DifficultJEE MAIN 2024

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What will be the $EMF$ of the cell formed by the following half-cells in $V$?
$Mg^{2+} + 2e^- \to Mg_{(s)}; E = -2.37 \ V$
$Cu^{2+} + 2e^- \to Cu_{(s)}; E = +0.33 \ V$

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$ClO_4^{-}$	$E^{\circ} = 1.19 \ V$
$IO_4^{-}$	$E^{\circ} = 1.65 \ V$
$BrO_4^{-}$	$E^{\circ} = 1.74 \ V$

Identify which of the following cell reactions is spontaneous under standard state conditions.

Similar Questions

For the reaction $Cr_2O_7^{2-} + I^- \to I_2 + Cr^{3+}$,if $E_{cell}^o = 0.79 \ V$ and $E_{Cr_2O_7^{2-}}^o = 1.33 \ V$,then $E_{I_2}^o = $ ............. $V$.

Which of the following metals does not liberate $\text{H}_2$ gas by reacting with $\text{HCl}$?

Given,the standard potentials $E_{(Cu^{2+}/Cu)}^{\circ}$ and $E_{(Cu^{+}/Cu)}^{\circ}$ as $0.340 \ V$ and $0.522 \ V$ respectively,the value of $E_{(Cu^{2+}/Cu^{+})}^{\circ}$ is $.... \ V$

Reduction potential of ions are given below: $ClO_4^{-}$ $E^{\circ} = 1.19 \ V$ $IO_4^{-}$ $E^{\circ} = 1.65 \ V$ $BrO_4^{-}$ $E^{\circ} = 1.74 \ V$ The correct order of their oxidising power is:

What will be the $EMF$ of the cell formed by the following half-cells in $V$?$Mg^{2+} + 2e^- \to Mg_{(s)}; E = -2.37 \ V$$Cu^{2+} + 2e^- \to Cu_{(s)}; E = +0.33 \ V$

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Reduction potential of ions are given below:

$ClO_4^{-}$ $E^{\circ} = 1.19 \ V$

$IO_4^{-}$ $E^{\circ} = 1.65 \ V$

$BrO_4^{-}$ $E^{\circ} = 1.74 \ V$

The correct order of their oxidising power is:

What will be the $EMF$ of the cell formed by the following half-cells in $V$?
$Mg^{2+} + 2e^- \to Mg_{(s)}; E = -2.37 \ V$
$Cu^{2+} + 2e^- \to Cu_{(s)}; E = +0.33 \ V$