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

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

(A) reaction is non-spontaneous if the standard cell potential $E^0_{cell} For option $A$: $E^0_{cell} = E^0_{cathode} - E^0_{anode} = E^0_{Fe^{+2}/Fe} - E^0_{Ag^{+}/Ag} = -0.44 - 0.79 = -1.23 \text{ V}$. Since $E^0_{cell} For option $B$: $E^0_{cell} = 0.34 - (-1.66) = 2.00 \text{ V} > 0$ (Spontaneous).For option $C$: $E^0_{cell} = 0.34 - (-0.44) = 0.78 \text{ V} > 0$ (Spontaneous).For option $D$: $E^0_{cell} = -0.44 - (-1.66) = 1.22 \text{ V} > 0$ (Spontaneous).

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Difficult

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
$2Ag(s) + Fe^{+2}(aq) \rightarrow 2Ag^{+}(aq) + Fe(s)$
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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$Cu^{+} + e^- \to Cu$ ; $E^o = X_1 \ V$
$Cu^{2+} + 2e^- \to Cu$ ; $E^o = X_2 \ V$
Then for $Cu^{2+} + e^- \to Cu^{+}$ ; $E^o$ will be ?

Medium

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$FeO_4^{2-}$ $\xrightarrow{2.0 \ V} Fe^{3+}$ $\xrightarrow{0.8 \ V} Fe^{2+}$ $\xrightarrow{-0.44 \ V} Fe^0$
In the above diagram,the standard electrode potentials are given in volts. The value of $E_{FeO_4^{2-}/Fe^{2+}}^{\Theta}$ is: (in $V$)

DifficultJEE MAIN 2025

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

Medium

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If $E^0_{Fe^{2+} / Fe} = -0.441 \ V$ and $E^0_{Fe^{3+} / Fe^{2+}} = 0.771 \ V$,the standard emf of the cell reaction $Fe_{(s)} + 2 Fe^{3+}_{(aq)} \longrightarrow 3 Fe^{2+}_{(aq)}$ is

MediumAP EAMCET 2025

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On the basis of the following $E^o$ values,the strongest oxidizing agent is:
$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-; E^o = -0.35 \ V$
$Fe^{2+} \to Fe^{3+} + e^-; E^o = -0.77 \ V$

MediumAIPMT 2008

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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

$Cu^{+} + e^- \to Cu$ ; $E^o = X_1 \ V$$Cu^{2+} + 2e^- \to Cu$ ; $E^o = X_2 \ V$Then for $Cu^{2+} + e^- \to Cu^{+}$ ; $E^o$ will be ?

$FeO_4^{2-}$ $\xrightarrow{2.0 \ V} Fe^{3+}$ $\xrightarrow{0.8 \ V} Fe^{2+}$ $\xrightarrow{-0.44 \ V} Fe^0$In the above diagram,the standard electrode potentials are given in volts. The value of $E_{FeO_4^{2-}/Fe^{2+}}^{\Theta}$ is: (in $V$)

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

If $E^0_{Fe^{2+} / Fe} = -0.441 \ V$ and $E^0_{Fe^{3+} / Fe^{2+}} = 0.771 \ V$,the standard emf of the cell reaction $Fe_{(s)} + 2 Fe^{3+}_{(aq)} \longrightarrow 3 Fe^{2+}_{(aq)}$ is

On the basis of the following $E^o$ values,the strongest oxidizing agent is:$[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$

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$Cu^{+} + e^- \to Cu$ ; $E^o = X_1 \ V$
$Cu^{2+} + 2e^- \to Cu$ ; $E^o = X_2 \ V$
Then for $Cu^{2+} + e^- \to Cu^{+}$ ; $E^o$ will be ?

$FeO_4^{2-}$ $\xrightarrow{2.0 \ V} Fe^{3+}$ $\xrightarrow{0.8 \ V} Fe^{2+}$ $\xrightarrow{-0.44 \ V} Fe^0$
In the above diagram,the standard electrode potentials are given in volts. The value of $E_{FeO_4^{2-}/Fe^{2+}}^{\Theta}$ is: (in $V$)

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

On the basis of the following $E^o$ values,the strongest oxidizing agent is:
$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-; E^o = -0.35 \ V$
$Fe^{2+} \to Fe^{3+} + e^-; E^o = -0.77 \ V$