(D) The cell reaction is $Fe^{2+} + Zn \longrightarrow Zn^{2+} + Fe$.Here,$Zn$ is oxidized to $Zn^{2+}$ (anode) and $Fe^{2+}$ is reduced to $Fe$ (cath

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(D) The cell reaction is $Fe^{2+} + Zn \longrightarrow Zn^{2+} + Fe$.Here,$Zn$ is oxidized to $Zn^{2+}$ (anode) and $Fe^{2+}$ is reduced to $Fe$ (cathode).The formula for the $emf$ of the cell is $E^{\circ}_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode}$.Substituting the given values: $E^{\circ}_{cell} = E^{\circ}_{Fe^{2+}/Fe} - E^{\circ}_{Zn^{2+}/Zn}$.$E^{\circ}_{cell} = -0.44 \ V - (-0.76 \ V)$.$E^{\circ}_{cell} = -0.44 \ V + 0.76 \ V = +0.32 \ V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

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The standard electrode potential for the half-cell reactions are
$Zn^{2+} + 2e^{-} \longrightarrow Zn ; E^{\circ} = -0.76 \ V$
$Fe^{2+} + 2e^{-} \longrightarrow Fe ; E^{\circ} = -0.44 \ V$
The $emf$ of the cell reaction,
$Fe^{2+} + Zn \longrightarrow Zn^{2+} + Fe$ is

KCET 2009 All KCET

A
$-0.32 \ V$
B
$-1.20 \ V$
C
$+1.20 \ V$
D
$+0.32 \ V$

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Electrode potential and ECell

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The $(\frac{\partial E}{\partial T})_P$ of different types of half cells are as follows:
$A$ $B$ $C$ $D$
$1 \times 10^{-4}$ $2 \times 10^{-4}$ $0.1 \times 10^{-4}$ $0.2 \times 10^{-4}$

(Where $E$ is the electromotive force)
Which of the above half cells would be preferred to be used as reference electrode?

$A$	$B$	$C$	$D$
$1 \times 10^{-4}$	$2 \times 10^{-4}$	$0.1 \times 10^{-4}$	$0.2 \times 10^{-4}$

DifficultJEE MAIN 2022

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The standard electrode potential (in $V$) values for $Al^{3+}/Al$ and $Tl^{3+}/Tl$ are respectively:

EasyAP EAMCET 2023

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$A$ cell constructed by coupling a standard copper electrode and a standard magnesium electrode has an $emf$ of $2.7 \ V$. If the standard reduction potential of the copper electrode is $+0.34 \ V$,the standard reduction potential of the magnesium electrode is .............. $V$.

Medium

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If the standard reduction potentials of four electrodes $A$, $B$, $C$, and $D$ are $+2.5 \text{ V}$, $+3.0 \text{ V}$, $-2.0 \text{ V}$, and $-1.5 \text{ V}$ respectively, in which of the following cases is the standard $emf$ of the cell maximum?

DifficultMHT CET 2026

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If $E^{\circ}(Fe^{+2}_{(aq)} \mid Fe_{(s)}) = -0.44 \ V$ and $E^{\circ}(Sn^{+2}_{(aq)} \mid Sn_{(s)}) = -0.14 \ V$,what is the standard $emf$ of the cell containing the two electrodes?

EasyMHT CET 2025

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The standard electrode potential for the half-cell reactions are$Zn^{2+} + 2e^{-} \longrightarrow Zn ; E^{\circ} = -0.76 \ V$$Fe^{2+} + 2e^{-} \longrightarrow Fe ; E^{\circ} = -0.44 \ V$The $emf$ of the cell reaction,$Fe^{2+} + Zn \longrightarrow Zn^{2+} + Fe$ is

Similar Questions

The $(\frac{\partial E}{\partial T})_P$ of different types of half cells are as follows:$A$$B$$C$$D$$1 \times 10^{-4}$$2 \times 10^{-4}$$0.1 \times 10^{-4}$$0.2 \times 10^{-4}$(Where $E$ is the electromotive force)Which of the above half cells would be preferred to be used as reference electrode?

The standard electrode potential (in $V$) values for $Al^{3+}/Al$ and $Tl^{3+}/Tl$ are respectively:

$A$ cell constructed by coupling a standard copper electrode and a standard magnesium electrode has an $emf$ of $2.7 \ V$. If the standard reduction potential of the copper electrode is $+0.34 \ V$,the standard reduction potential of the magnesium electrode is .............. $V$.

If the standard reduction potentials of four electrodes $A$, $B$, $C$, and $D$ are $+2.5 \text{ V}$, $+3.0 \text{ V}$, $-2.0 \text{ V}$, and $-1.5 \text{ V}$ respectively, in which of the following cases is the standard $emf$ of the cell maximum?

If $E^{\circ}(Fe^{+2}_{(aq)} \mid Fe_{(s)}) = -0.44 \ V$ and $E^{\circ}(Sn^{+2}_{(aq)} \mid Sn_{(s)}) = -0.14 \ V$,what is the standard $emf$ of the cell containing the two electrodes?

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The standard electrode potential for the half-cell reactions are
$Zn^{2+} + 2e^{-} \longrightarrow Zn ; E^{\circ} = -0.76 \ V$
$Fe^{2+} + 2e^{-} \longrightarrow Fe ; E^{\circ} = -0.44 \ V$
The $emf$ of the cell reaction,
$Fe^{2+} + Zn \longrightarrow Zn^{2+} + Fe$ is