(A) The standard free energy change $\Delta G^o$ is related to the standard cell potential $E^o$ by the equation: $\Delta G^o = -nFE^o$. In the given

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(A) The standard free energy change $\Delta G^o$ is related to the standard cell potential $E^o$ by the equation: $\Delta G^o = -nFE^o$. In the given reaction,$\frac{1}{2}Cu_{(s)} + \frac{1}{2}Cl_{2(g)} \rightleftharpoons \frac{1}{2}Cu^{2+} + Cl^-$,the number of electrons transferred $(n)$ is $1$. The Faraday constant $F$ is $96500 \ C \ mol^{-1}$ and the standard cell potential $E^o$ is $1.02 \ V$. Substituting these values: $\Delta G^o = -1 \times 96500 \times 1.02 = -98430 \ J$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

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Calculate the standard free energy change for the reaction $\frac{1}{2}Cu_{(s)} + \frac{1}{2}Cl_{2(g)} \rightleftharpoons \frac{1}{2}Cu^{2+} + Cl^-$ taking place at $25\ ^oC$ in a cell whose standard e.m.f. is $1.02 \ V$ (in $J$).

A
$-98430$
B
$98430$
C
$96500$
D
$-49215$

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Electrochemistry

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Electrode potential and ECell

For the cell $Zn_{(s)} | Zn^{2+}_{(aq)} || M^{x+}_{(aq)} | M_{(s)}$,different half cells and their standard electrode potentials are given below:
$M^{x+}_{(aq)} / M_{(s)}$ $Au^{3+}_{(aq)} / Au_{(s)}$ $Ag^{+}_{(aq)} / Ag_{(s)}$ $Fe^{3+}_{(aq)} / Fe^{2+}_{(aq)}$ $Fe^{2+}_{(aq)} / Fe_{(s)}$
$E^o M^{x+} / M (V)$ $1.40$ $0.80$ $0.77$ $-0.44$

If $E^o Zn^{2+}/Zn = -0.76 \ V$,which cathode will give a maximum value of $E^o_{cell}$ per electron transferred?

DifficultJEE MAIN 2019

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$Li$ occupies a higher position in the electrochemical series of metals as compared to $Cu$ since:

EasyWBJEE 2012

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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 ............ $V$.

MediumIIT 1988

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Standard electrode potential of three metals $X$,$Y$ and $Z$ are $-1.2 \, V$,$+0.5 \, V$ and $-3.0 \, V$ respectively. The reducing power of these metals will be

MediumAIPMT 2011

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Identify the reaction from the following that corresponds to the standard electrode potential of the $Cu^{+2}/Cu$ electrode being $0.34 \text{ V}$ with respect to the $SHE$?

EasyMHT CET 2026

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$M^{x+}_{(aq)} / M_{(s)}$	$Au^{3+}_{(aq)} / Au_{(s)}$	$Ag^{+}_{(aq)} / Ag_{(s)}$	$Fe^{3+}_{(aq)} / Fe^{2+}_{(aq)}$	$Fe^{2+}_{(aq)} / Fe_{(s)}$
$E^o M^{x+} / M (V)$	$1.40$	$0.80$	$0.77$	$-0.44$

Calculate the standard free energy change for the reaction $\frac{1}{2}Cu_{(s)} + \frac{1}{2}Cl_{2(g)} \rightleftharpoons \frac{1}{2}Cu^{2+} + Cl^-$ taking place at $25\ ^oC$ in a cell whose standard e.m.f. is $1.02 \ V$ (in $J$).

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$Li$ occupies a higher position in the electrochemical series of metals as compared to $Cu$ since:

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 ............ $V$.

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