(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

Easy

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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Standard potential of electrode reaction $Cu^{2+}_{(aq)} + 2e^{-} \rightarrow Cu_{(s)}$ is $+0.34 \ V$. What is the standard potential of the reaction $2Cu_{(s)} \rightarrow 2Cu^{2+}_{(aq)} + 4e^{-}$?

MediumMHT CET 2025

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$I_2 + 2e^{-} \to 2I^{-}$; $E^{o} = 0.54 \ V$
$Cl_2 + 2e^{-} \to 2Cl^{-}$; $E^{o} = 1.36 \ V$
$Mn^{3+} + e^{-} \to Mn^{2+}$; $E^{o} = 1.50 \ V$
$Fe^{3+} + e^{-} \to Fe^{2+}$; $E^{o} = 0.77 \ V$
Which of the following is a correct statement?

Medium

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The $emf$ of a galvanic cell,with electrode potentials of silver $= +0.80 \ V$ and that of copper $= +0.34 \ V$,is ........... $V$.

MediumAIIMS 1999

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Aluminium displaces hydrogen from acids but copper does not. $A$ galvanic cell prepared by combining $Cu/Cu^{2+}$ and $Al/Al^{3+}$ has an e.m.f. of $2.0 \ V$ at $298 \ K$. If the potential of copper electrode is $+0.34 \ V$,that of aluminium is .......... $V$

Medium

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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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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

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Standard potential of electrode reaction $Cu^{2+}_{(aq)} + 2e^{-} \rightarrow Cu_{(s)}$ is $+0.34 \ V$. What is the standard potential of the reaction $2Cu_{(s)} \rightarrow 2Cu^{2+}_{(aq)} + 4e^{-}$?

$I_2 + 2e^{-} \to 2I^{-}$; $E^{o} = 0.54 \ V$$Cl_2 + 2e^{-} \to 2Cl^{-}$; $E^{o} = 1.36 \ V$$Mn^{3+} + e^{-} \to Mn^{2+}$; $E^{o} = 1.50 \ V$$Fe^{3+} + e^{-} \to Fe^{2+}$; $E^{o} = 0.77 \ V$Which of the following is a correct statement?

The $emf$ of a galvanic cell,with electrode potentials of silver $= +0.80 \ V$ and that of copper $= +0.34 \ V$,is ........... $V$.

Aluminium displaces hydrogen from acids but copper does not. $A$ galvanic cell prepared by combining $Cu/Cu^{2+}$ and $Al/Al^{3+}$ has an e.m.f. of $2.0 \ V$ at $298 \ K$. If the potential of copper electrode is $+0.34 \ V$,that of aluminium is .......... $V$

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

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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

$I_2 + 2e^{-} \to 2I^{-}$; $E^{o} = 0.54 \ V$
$Cl_2 + 2e^{-} \to 2Cl^{-}$; $E^{o} = 1.36 \ V$
$Mn^{3+} + e^{-} \to Mn^{2+}$; $E^{o} = 1.50 \ V$
$Fe^{3+} + e^{-} \to Fe^{2+}$; $E^{o} = 0.77 \ V$
Which of the following is a correct statement?

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