(A) reaction is non-spontaneous if the standard cell potential $E^0_{cell} < 0$.$E^0_{cell} = E^0_{cathode} - E^0_{anode}$.For option $(A)$: $2Ag(s) +

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$2Ag(s) + Fe^{+2}_{(aq)} \rightarrow 2Ag^{+1}_{(aq)} + Fe(s)$

(A) reaction is non-spontaneous if the standard cell potential $E^0_{cell} $E^0_{cell} = E^0_{cathode} - E^0_{anode}$.For option $(A)$: $2Ag(s) + Fe^{+2}_{(aq)} \rightarrow 2Ag^{+1}_{(aq)} + Fe(s)$.$E^0_{cathode} = E^0_{(Fe^{+2}|Fe)} = -0.44 \text{ V}$.$E^0_{anode} = E^0_{(Ag^{+1}|Ag)} = +0.79 \text{ V}$.$E^0_{cell} = -0.44 - 0.79 = -1.23 \text{ V}$.Since $E^0_{cell} < 0$, the reaction is non-spontaneous.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

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If standard reduction potentials $(E^0)$ of $(Al^{+3}_{(aq)}|Al(s))$, $(Fe^{+2}_{(aq)}|Fe(s))$, $(Cu^{+2}_{(aq)}|Cu(s))$ and $(Ag^{+1}_{(aq)}|Ag(s))$ are $-1.66 \text{ V}$, $-0.44 \text{ V}$, $+0.34 \text{ V}$ and $+0.79 \text{ V}$ respectively, which of the following reactions is non-spontaneous?

MHT CET 2026 All MHT CET

A
$2Ag(s) + Fe^{+2}_{(aq)} \rightarrow 2Ag^{+1}_{(aq)} + Fe(s)$
B
$2Al(s) + 3Cu^{+2}_{(aq)} \rightarrow 2Al^{+3}_{(aq)} + 3Cu(s)$
C
$Fe(s) + Cu^{+2}_{(aq)} \rightarrow Fe^{+2}_{(aq)} + Cu(s)$
D
$2Al(s) + 3Fe^{+2}_{(aq)} \rightarrow 2Al^{+3}_{(aq)} + 3Fe(s)$

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Electrode potential and ECell

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What happens to the Gibbs free energy in a spontaneous electrochemical process?

Easy

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From the given values,which one is a strong oxidizing agent?
$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-, E^o = -0.35 \ V$
$Fe^{2+} \to Fe^{3+} + e^-, E^o = -0.77 \ V$

Easy

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Assertion : Copper reacts with $HCl$ and liberates hydrogen.
Reason : Hydrogen is present above $Cu$ in the reactivity series.

DifficultAIIMS 2000

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If the emf of the cell $Cu(s) | Cu^{2+}(1M) || Ag^+(1M) | Ag(s)$ is $0.463 \text{ V}$ at $25^{\circ} \text{C}$ and the standard electrode potential of the $Cu$ electrode is $0.337 \text{ V}$, find the standard electrode potential of the $Ag$ electrode. (in $\text{ V}$)

DifficultMHT CET 2026

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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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If standard reduction potentials $(E^0)$ of $(Al^{+3}_{(aq)}|Al(s))$, $(Fe^{+2}_{(aq)}|Fe(s))$, $(Cu^{+2}_{(aq)}|Cu(s))$ and $(Ag^{+1}_{(aq)}|Ag(s))$ are $-1.66 \text{ V}$, $-0.44 \text{ V}$, $+0.34 \text{ V}$ and $+0.79 \text{ V}$ respectively, which of the following reactions is non-spontaneous?

Similar Questions

What happens to the Gibbs free energy in a spontaneous electrochemical process?

From the given values,which one is a strong oxidizing agent?$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-, E^o = -0.35 \ V$$Fe^{2+} \to Fe^{3+} + e^-, E^o = -0.77 \ V$

Assertion : Copper reacts with $HCl$ and liberates hydrogen.Reason : Hydrogen is present above $Cu$ in the reactivity series.

If the emf of the cell $Cu(s) | Cu^{2+}(1M) || Ag^+(1M) | Ag(s)$ is $0.463 \text{ V}$ at $25^{\circ} \text{C}$ and the standard electrode potential of the $Cu$ electrode is $0.337 \text{ V}$, find the standard electrode potential of the $Ag$ electrode. (in $\text{ V}$)

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)$

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From the given values,which one is a strong oxidizing agent?
$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-, E^o = -0.35 \ V$
$Fe^{2+} \to Fe^{3+} + e^-, E^o = -0.77 \ V$

Assertion : Copper reacts with $HCl$ and liberates hydrogen.
Reason : Hydrogen is present above $Cu$ in the reactivity series.

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