(D) The cell reaction is as follows:Anode (Oxidation): $Mg_{(s)} \rightarrow Mg_{(aq)}^{2+} + 2e^-$Cathode (Reduction): $Cl_{2_{(g)}} + 2e^- \rightarr

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$E_{cell} = E_{cell}^0 - \frac{0.059}{2} \log [Mg^{2+}][Cl^{-}]^2$

(D) The cell reaction is as follows:Anode (Oxidation): $Mg_{(s)} \rightarrow Mg_{(aq)}^{2+} + 2e^-$Cathode (Reduction): $Cl_{2_{(g)}} + 2e^- \rightarrow 2Cl_{(aq)}^{-}$Overall reaction: $Mg_{(s)} + Cl_{2_{(g)}} \rightarrow Mg_{(aq)}^{2+} + 2Cl_{(aq)}^{-}$The Nernst equation is given by: $E_{cell} = E_{cell}^0 - \frac{0.059}{n} \log Q$Here,$n = 2$ and the reaction quotient $Q = \frac{[Mg^{2+}][Cl^{-}]^2}{P_{Cl_2}}$.Since $P_{Cl_2} = 1 \ bar$,$Q = [Mg^{2+}][Cl^{-}]^2$.Thus,the correct equation is $E_{cell} = E_{cell}^0 - \frac{0.059}{2} \log [Mg^{2+}][Cl^{-}]^2$.

Class 12 Chemistry Electrochemistry Nernst equation and ECS

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Which of the following is correct as a Nernst equation for the given electrochemical cell ?
$Mg_{(s)}|Mg_{(aq)}^{2+}(0.1 \ M)||Cl_{(aq)}^{-}(0.1 \ M)|Cl_{2_{(g)}}(1 \ bar)|Pt_{(s)}$

GUJCET 2023 All GUJCET

A
$E_{cell} = E_{cell}^0 - \frac{0.059}{2} \log \frac{[Mg^{2+}][Cl^{-}]^2}{P_{Cl_2}}$
B
$E_{cell} = E_{cell}^0 - \frac{0.059}{2} \log \frac{[Mg^{2+}]}{[Cl^{-}]^2}$
C
$E_{cell} = E_{cell}^0 - \frac{0.059}{2} \log \frac{1}{[Mg^{2+}][Cl^{-}]^2}$
D
$E_{cell} = E_{cell}^0 - \frac{0.059}{2} \log [Mg^{2+}][Cl^{-}]^2$

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At $298 \, K$,the standard reduction potential for $Cu^{2+}/Cu$ electrode is $0.34 \, V$.
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DifficultJEE MAIN 2023

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The standard electrode potential of $Cu^{2+}/Cu$ is $0.34 \text{ V}$ at $298 \text{ K}$. Calculate its electrode potential at the same temperature when the $Cu^{2+}$ ion concentration is $0.1 \text{ M}$. (in $\text{ V}$)

DifficultMHT CET 2026

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Which of the following will increase the voltage of the cell represented by the equation
$Cu_{(s)} + 2Ag^{+}_{(aq)} \to Cu^{2+}_{(aq)} + 2Ag_{(s)}$

Medium

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Find the observed $EMF$ of the cell $Cd | Cd^{2+}(0.01 \ M) || Cu^{2+}(0.01 \ M) | Cu$ under conditions where the internal resistance is $4 \ \Omega$ and it is producing a current of $0.15 \ A$. (Given: $E^{\circ}_{Cu^{2+}/Cu} = 0.35 \ V$ and $E^{\circ}_{Cd^{2+}/Cd} = -0.4 \ V$) (in $V$)

MediumAP EAMCET 2020

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Consider the following electrode processes of a cell: $Cl^{-} \rightarrow \frac{1}{2} Cl_2 + e^{-}$ and $MCl + e^{-} \rightarrow M + Cl^{-}$. If the $EMF$ of this cell is $-1.140 \ V$ and the $E^{\circ}$ value of the cell is $-0.55 \ V$ at $298 \ K$,the value of the equilibrium constant $(K_{sp})$ of the sparingly soluble salt $MCl$ is in the order of:

DifficultTS EAMCET 2017

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Which of the following is correct as a Nernst equation for the given electrochemical cell ?$Mg_{(s)}|Mg_{(aq)}^{2+}(0.1 \ M)||Cl_{(aq)}^{-}(0.1 \ M)|Cl_{2_{(g)}}(1 \ bar)|Pt_{(s)}$

Similar Questions

The standard electrode potential of $Cu^{2+}/Cu$ is $0.34 \text{ V}$ at $298 \text{ K}$. Calculate its electrode potential at the same temperature when the $Cu^{2+}$ ion concentration is $0.1 \text{ M}$. (in $\text{ V}$)

Which of the following will increase the voltage of the cell represented by the equation$Cu_{(s)} + 2Ag^{+}_{(aq)} \to Cu^{2+}_{(aq)} + 2Ag_{(s)}$

Find the observed $EMF$ of the cell $Cd | Cd^{2+}(0.01 \ M) || Cu^{2+}(0.01 \ M) | Cu$ under conditions where the internal resistance is $4 \ \Omega$ and it is producing a current of $0.15 \ A$. (Given: $E^{\circ}_{Cu^{2+}/Cu} = 0.35 \ V$ and $E^{\circ}_{Cd^{2+}/Cd} = -0.4 \ V$) (in $V$)

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Which of the following is correct as a Nernst equation for the given electrochemical cell ?
$Mg_{(s)}|Mg_{(aq)}^{2+}(0.1 \ M)||Cl_{(aq)}^{-}(0.1 \ M)|Cl_{2_{(g)}}(1 \ bar)|Pt_{(s)}$

Which of the following will increase the voltage of the cell represented by the equation
$Cu_{(s)} + 2Ag^{+}_{(aq)} \to Cu^{2+}_{(aq)} + 2Ag_{(s)}$