(C) At equilibrium,the cell potential $E$ becomes $0$.Substituting $E = 0$ and $Q = K_{eq}$ into the Nernst equation: $0 = E^o - \frac{RT}{nF} \ln K_{

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(C) At equilibrium,the cell potential $E$ becomes $0$.Substituting $E = 0$ and $Q = K_{eq}$ into the Nernst equation: $0 = E^o - \frac{RT}{nF} \ln K_{eq}$.This implies $E^o = \frac{RT}{nF} \ln K_{eq}$.Rearranging for $K_{eq}$,we get $\ln K_{eq} = \frac{n E^o F}{RT}$,which leads to $K_{eq} = e^{\frac{n E^o F}{RT}}$.Therefore,the statement $E = E^o$ is incorrect because at equilibrium $E = 0$,not $E^o$.

Class 12 Chemistry Electrochemistry Nernst equation and ECS

Medium

The Nernst equation is given by $E = E^o - \frac{RT}{nF} \ln Q$. If $Q = K_{eq}$,then which of the following is not correct?

A
$E = 0$
B
$\frac{RT}{nF} \ln K_{eq} = E^o$
C
$E = E^o$
D
$K_{eq} = e^{\frac{n E^o F}{RT}}$

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Nernst equation and ECS

The Nernst equation is related to:

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DifficultAP EAMCET 2020

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MediumKVPY 2015

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The Nernst equation is given by $E = E^o - \frac{RT}{nF} \ln Q$. If $Q = K_{eq}$,then which of the following is not correct?

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The Nernst equation is related to:

Calculate the equilibrium constant for the following reaction: $Ni_{(s)} + Cu_{(aq)}^{2+} \to Cu_{(s)} + Ni_{(aq)}^{2+}$. Given: $E_{Ni^{2+}|Ni}^o = -0.25 \ V$ and $E_{Cu^{2+}|Cu}^o = 0.34 \ V$.

For the cell reaction,$3 Sn^{4+} + 2 Cr \longrightarrow 3 Sn^{2+} + 2 Cr^{3+}$,$E^{\circ}_{cell}$ is $0.89 \ V$. Then $\Delta G^{\circ}$ for the reaction is

The standard cell potential of a cell reaction involving the transfer of $2$ electrons at $25^{\circ}C$ is $0.295 \ V$. What is its equilibrium constant at $25^{\circ}C$?

The standard cell potential for $Zn \mid Zn^{2+} \parallel Cu^{2+} \mid Cu$ is $1.10 \ V$. When the cell is completely discharged,$\log ([Zn^{2+}] / [Cu^{2+}])$ is closest to $.....$

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