(C) The standard cell potential is calculated using the formula: $E^o_{cell} = E^o_{cathode} - E^o_{anode}$.In the given cell $Zn | Zn^{2+} || Cu^{2+}

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(C) The standard cell potential is calculated using the formula: $E^o_{cell} = E^o_{cathode} - E^o_{anode}$.In the given cell $Zn | Zn^{2+} || Cu^{2+} | Cu$,the $Cu^{2+} | Cu$ electrode acts as the cathode and $Zn^{2+} | Zn$ acts as the anode.Given $E^o_{cathode} = E^o_{Cu^{2+} | Cu} = +0.34 \ V$ and $E^o_{anode} = E^o_{Zn^{2+} | Zn} = -0.76 \ V$.Substituting these values: $E^o_{cell} = 0.34 \ V - (-0.76 \ V) = 0.34 + 0.76 = 1.10 \ V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

What is the standard cell potential for the cell $Zn | Zn^{2+} (1M) || Cu^{2+} (1M) | Cu$? Given $E^o$ for $Zn^{2+} | Zn = -0.76 \ V$ and $E^o$ for $Cu^{2+} | Cu = +0.34 \ V$.

AIIMS 1980 All AIIMS

A
$-0.76 + (-0.34) = -0.42 \ V$
B
$-0.34 + 0.76 = +0.42 \ V$
C
$0.34 - (-0.76) = 1.10 \ V$
D
$-0.76 - (+0.34) = -1.10 \ V$

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Electrode potential and ECell

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AIIMS 1980 Paper All AIIMS years →

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

DifficultAIIMS 2000

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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 standard oxidation potentials for the half-reactions are given as $Zn \to Zn^{2+} + 2e^{-}; E^o = +0.76 \ V$ and $Fe \to Fe^{2+} + 2e^{-}; E^o = +0.41 \ V$. The $EMF$ for the cell reaction $Fe^{2+} + Zn \to Zn^{2+} + Fe$ is ............ $V$.

MediumAIPMT 1993

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Given that $E^o_{K^{+}/K} = -2.93 \ V$,$E^o_{Fe^{2+}/Fe} = -0.44 \ V$,$E^o_{Zn^{2+}/Zn} = -0.76 \ V$,and $E^o_{Cu^{2+}/Cu} = 0.34 \ V$. Based on this data,which of the following is the strongest reducing agent?

DifficultAIIMS 2011

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If $E^o_{A^{+2}/A} = -0.30 \ V$ and $E^o_{A^{+3}/A^{+2}} = 0.40 \ V$,the standard $EMF$ of the reaction: $A + 2A^{+3} \to 3A^{+2}$ will be ............ $V$.

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What is the standard cell potential for the cell $Zn | Zn^{2+} (1M) || Cu^{2+} (1M) | Cu$? Given $E^o$ for $Zn^{2+} | Zn = -0.76 \ V$ and $E^o$ for $Cu^{2+} | Cu = +0.34 \ V$.

Similar Questions

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

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 standard oxidation potentials for the half-reactions are given as $Zn \to Zn^{2+} + 2e^{-}; E^o = +0.76 \ V$ and $Fe \to Fe^{2+} + 2e^{-}; E^o = +0.41 \ V$. The $EMF$ for the cell reaction $Fe^{2+} + Zn \to Zn^{2+} + Fe$ is ............ $V$.

Given that $E^o_{K^{+}/K} = -2.93 \ V$,$E^o_{Fe^{2+}/Fe} = -0.44 \ V$,$E^o_{Zn^{2+}/Zn} = -0.76 \ V$,and $E^o_{Cu^{2+}/Cu} = 0.34 \ V$. Based on this data,which of the following is the strongest reducing agent?

If $E^o_{A^{+2}/A} = -0.30 \ V$ and $E^o_{A^{+3}/A^{+2}} = 0.40 \ V$,the standard $EMF$ of the reaction: $A + 2A^{+3} \to 3A^{+2}$ will be ............ $V$.

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

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.