(C) The cell reaction is: $M + Cu^{2+} \rightarrow M^{2+} + Cu$ According to the Nernst equation: $E_{\text{cell}} = E^{\circ}_{\text{cell}} - \frac{0

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(C) The cell reaction is: $M + Cu^{2+} \rightarrow M^{2+} + Cu$ According to the Nernst equation: $E_{\text{cell}} = E^{\circ}_{\text{cell}} - \frac{0.06}{n} \log \frac{[M^{2+}]}{[Cu^{2+}]}$ Given: $E^{\circ}_{\text{cell}} = 0.3 \ V$ $n = 2$ $[M^{2+}] = 0.1 \ M$ $E_{\text{cell}} = 0$ Substituting the values: $0 = 0.3 - \frac{0.06}{2} \log \frac{0.1}{[Cu^{2+}]}$ $0.3 = 0.03 \log \frac{0.1}{[Cu^{2+}]}$ $10 = \log \frac{0.1}{[Cu^{2+}]}$ $\frac{0.1}{[Cu^{2+}]} = 10^{10}$ $[Cu^{2+}] = \frac{0.1}{10^{10}} = 10^{-11} \ mol \ L^{-1}$

Class 12 Chemistry Electrochemistry Nernst equation and ECS

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The $E^{\circ}$ of $M \mid M^{2+} \parallel Cu^{2+} \mid Cu$ is $0.3 \ V$. At what concentration of $Cu^{2+}$ (in $mol \ L^{-1}$),the $E_{\text{cell}}$ value becomes zero?
$\left(\frac{2.303 \ RT}{F} = 0.06\right)$,$\left(\text{Conc. of } M^{2+} = 0.1 \ M\right)$

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A
$10^{-9}$
B
$10^{-8}$
C
$10^{-11}$
D
$10^{-10}$

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$Cu_{(s)} | Cu^{+2}(aq, 10^{-3} M) || Ag^{+}(aq, 10^{-5} M) | Ag_{(s)}$
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The $E^{\circ}$ of $M \mid M^{2+} \parallel Cu^{2+} \mid Cu$ is $0.3 \ V$. At what concentration of $Cu^{2+}$ (in $mol \ L^{-1}$),the $E_{\text{cell}}$ value becomes zero? $\left(\frac{2.303 \ RT}{F} = 0.06\right)$,$\left(\text{Conc. of } M^{2+} = 0.1 \ M\right)$

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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 $\text{ V}$)

Calculate the electrode potential at $298 \; K$ for $Zn|Zn^{2+}$ electrode in which the activity of zinc ions is $0.001 \; M$ and $E^o_{Zn^{2+}/Zn}$ is $-0.76 \; V$. (in $; V$)

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$Cu_{(s)} | Cu^{+2}(aq, 10^{-3} M) || Ag^{+}(aq, 10^{-5} M) | Ag_{(s)}$If $E^{o}_{Cu^{+2}/Cu} = +0.34 \ V$$E^{o}_{Ag^{+}/Ag} = +0.80 \ V$$E_{cell}$ will be

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The $E^{\circ}$ of $M \mid M^{2+} \parallel Cu^{2+} \mid Cu$ is $0.3 \ V$. At what concentration of $Cu^{2+}$ (in $mol \ L^{-1}$),the $E_{\text{cell}}$ value becomes zero?
$\left(\frac{2.303 \ RT}{F} = 0.06\right)$,$\left(\text{Conc. of } M^{2+} = 0.1 \ M\right)$

$Cu_{(s)} | Cu^{+2}(aq, 10^{-3} M) || Ag^{+}(aq, 10^{-5} M) | Ag_{(s)}$
If $E^{o}_{Cu^{+2}/Cu} = +0.34 \ V$
$E^{o}_{Ag^{+}/Ag} = +0.80 \ V$
$E_{cell}$ will be