(C) For a cell to be feasible,$E^{\circ}_{cell}$ must be positive.$E^{\circ}_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode}$Here,$Co^{3+}$ is reduce

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(C) For a cell to be feasible,$E^{\circ}_{cell}$ must be positive.$E^{\circ}_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode}$Here,$Co^{3+}$ is reduced $(cathode)$ and $Al$ is oxidized $(anode)$.$E^{\circ}_{cathode} = E^{\circ}_{Co^{3+}/Co^{2+}} = 1.81 \, V$$E^{\circ}_{anode} = E^{\circ}_{Al^{3+}/Al} = -1.66 \, V$$E^{\circ}_{cell} = 1.81 \, V - (-1.66 \, V) = 1.81 + 1.66 = 3.47 \, V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

Two half-cell reactions are given below:
$Co^{3+} + e^- \rightarrow Co^{2+}, E^{\circ}_{Co^{3+}/Co^{2+}} = 1.81 \, V$
$Al^{3+} + 3e^- \rightarrow Al(s), E^{\circ}_{Al^{3+}/Al} = -1.66 \, V$
The standard $EMF$ of a cell with a feasible redox reaction will be:

NEET 2022 All NEET

A
$+7.09 \, V$
B
$+0.15 \, V$
C
$+3.47 \, V$
D
$-3.47 \, V$

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Class 12

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Electrochemistry

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Electrode potential and ECell

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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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Given the standard electrode potentials:
$K^{+} / K = -2.93 \, V$,$Ag^{+} / Ag = 0.80 \, V$
$Hg^{2+} / Hg = 0.79 \, V$
$Mg^{2+} / Mg = -2.37 \, V$,$Cr^{3+} / Cr = -0.74 \, V$
Arrange these metals in their increasing order of reducing power.

Medium

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The values of $E^0$ for metals $A$,$B$,and $C$ are $0.34 \ V$,$-0.80 \ V$,and $-0.46 \ V$ respectively. State the correct order for their ability to act as reducing agents.

EasyGUJCET 2015

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$Zn^{2+} + 2e^- \to Zn_{(s)}$; $E^o = -0.76 \ V$
$Fe^{3+} + e^- \to Fe^{2+}$; $E^o = +0.77 \ V$
$Cr^{3+} + 3e^- \to Cr_{(s)}$; $E^o = -0.74 \ V$
$H^{+} + e^- \to 1/2 H_2$; $E^o = 0.00 \ V$
Which of the following is the strongest reducing agent?

Easy

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$Cr_2O_7^{2-} + I^{-} \to I_2 + Cr^{3+}$
$E^0_{cell} = 0.79 \ V$
$E^0_{Cr_2O_7^{2-}} = 1.33 \ V$,$E^0_{I_2}$ is ........... $V$

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Two half-cell reactions are given below:$Co^{3+} + e^- \rightarrow Co^{2+}, E^{\circ}_{Co^{3+}/Co^{2+}} = 1.81 \, V$$Al^{3+} + 3e^- \rightarrow Al(s), E^{\circ}_{Al^{3+}/Al} = -1.66 \, V$The standard $EMF$ of a cell with a feasible redox reaction will be:

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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 $\text{ V}$)

Given the standard electrode potentials:$K^{+} / K = -2.93 \, V$,$Ag^{+} / Ag = 0.80 \, V$$Hg^{2+} / Hg = 0.79 \, V$$Mg^{2+} / Mg = -2.37 \, V$,$Cr^{3+} / Cr = -0.74 \, V$Arrange these metals in their increasing order of reducing power.

The values of $E^0$ for metals $A$,$B$,and $C$ are $0.34 \ V$,$-0.80 \ V$,and $-0.46 \ V$ respectively. State the correct order for their ability to act as reducing agents.

$Zn^{2+} + 2e^- \to Zn_{(s)}$; $E^o = -0.76 \ V$$Fe^{3+} + e^- \to Fe^{2+}$; $E^o = +0.77 \ V$$Cr^{3+} + 3e^- \to Cr_{(s)}$; $E^o = -0.74 \ V$$H^{+} + e^- \to 1/2 H_2$; $E^o = 0.00 \ V$Which of the following is the strongest reducing agent?

$Cr_2O_7^{2-} + I^{-} \to I_2 + Cr^{3+}$$E^0_{cell} = 0.79 \ V$$E^0_{Cr_2O_7^{2-}} = 1.33 \ V$,$E^0_{I_2}$ is ........... $V$

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Two half-cell reactions are given below:
$Co^{3+} + e^- \rightarrow Co^{2+}, E^{\circ}_{Co^{3+}/Co^{2+}} = 1.81 \, V$
$Al^{3+} + 3e^- \rightarrow Al(s), E^{\circ}_{Al^{3+}/Al} = -1.66 \, V$
The standard $EMF$ of a cell with a feasible redox reaction will be:

Given the standard electrode potentials:
$K^{+} / K = -2.93 \, V$,$Ag^{+} / Ag = 0.80 \, V$
$Hg^{2+} / Hg = 0.79 \, V$
$Mg^{2+} / Mg = -2.37 \, V$,$Cr^{3+} / Cr = -0.74 \, V$
Arrange these metals in their increasing order of reducing power.

$Zn^{2+} + 2e^- \to Zn_{(s)}$; $E^o = -0.76 \ V$
$Fe^{3+} + e^- \to Fe^{2+}$; $E^o = +0.77 \ V$
$Cr^{3+} + 3e^- \to Cr_{(s)}$; $E^o = -0.74 \ V$
$H^{+} + e^- \to 1/2 H_2$; $E^o = 0.00 \ V$
Which of the following is the strongest reducing agent?

$Cr_2O_7^{2-} + I^{-} \to I_2 + Cr^{3+}$
$E^0_{cell} = 0.79 \ V$
$E^0_{Cr_2O_7^{2-}} = 1.33 \ V$,$E^0_{I_2}$ is ........... $V$