(B) The electrode reaction for the copper cathode is: $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$.According to the Nernst equation for this electrode:$E_{C

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(B) The electrode reaction for the copper cathode is: $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$.According to the Nernst equation for this electrode:$E_{Cu^{2+}/Cu} = E_{Cu^{2+}/Cu}^{\ominus} - \frac{0.059}{n} \log \frac{1}{[Cu^{2+}]}$.Given $\frac{2.303 \ RT}{F} = 0.06 \ V$,we use $0.06$ instead of $0.059$:$E_{Cu^{2+}/Cu} = 0.34 - \frac{0.06}{2} \log \frac{1}{0.1}$.$E_{Cu^{2+}/Cu} = 0.34 - 0.03 \log(10)$.Since $\log(10) = 1$,we have:$E_{Cu^{2+}/Cu} = 0.34 - 0.03 = 0.31 \ V$.

Class 12 Chemistry Electrochemistry Nernst equation and ECS

Medium

In a cell,a copper electrode was used as a cathode. What is the electrode potential (in $V$) of the copper electrode dipped in $0.1 \ M \ Cu^{2+}$ solution at $298 \ K$?
$(E_{Cu^{2+}/Cu}^{\ominus} = 0.34 \ V; \frac{2.303 \ RT}{F} = 0.06 \ V)$

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A
$0.34$
B
$0.31$
C
$0.37$
D
$0.40$

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Nernst equation and ECS

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The cell reaction of the given cell is spontaneous if:
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The $E^o$ for the cell $Zn|Zn^{2+}_{(aq)}||Cu^{2+}_{(aq)}|Cu$ is $1.10 \ V$ at $25 \ ^oC$. The equilibrium constant for the reaction $Zn + Cu^{2+}_{(aq)} \rightleftharpoons Cu + Zn^{2+}_{(aq)}$ is of the order of:

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In a cell,a copper electrode was used as a cathode. What is the electrode potential (in $V$) of the copper electrode dipped in $0.1 \ M \ Cu^{2+}$ solution at $298 \ K$?$(E_{Cu^{2+}/Cu}^{\ominus} = 0.34 \ V; \frac{2.303 \ RT}{F} = 0.06 \ V)$

Similar Questions

For the cell reaction $Zn(s) + Cu^{2+}(aq) (1.0 \, M) \to Cu(s) + Zn^{2+}(aq) (0.1 \, M)$,the measured $e.m.f.$ at $25 \, ^oC$ is $1.3 \, V$. Calculate the $E^o$ value for the cell reaction. (in $, V$)

The $EMF$ of the cell $Cr|Cr^{3+}(0.1 \ M) \| Fe^{2+}(0.01 \ M)|Fe$ is: $(E^{\circ}_{Cr^{3+}|Cr} = -0.75 \ V, E^{\circ}_{Fe^{2+}|Fe} = -0.45 \ V)$ (in $V$)

Which of the following expressions indicates the correct relationship between molar conductivity of a strong electrolyte and its concentration $c$?

The cell reaction of the given cell is spontaneous if:$Pt | Cl_2 (P_1 \, atm) | Cl^{-} (1 \, M) || Cl^{-} (1 \, M) | Cl_2 (P_2 \, atm) | Pt$

The $E^o$ for the cell $Zn|Zn^{2+}_{(aq)}||Cu^{2+}_{(aq)}|Cu$ is $1.10 \ V$ at $25 \ ^oC$. The equilibrium constant for the reaction $Zn + Cu^{2+}_{(aq)} \rightleftharpoons Cu + Zn^{2+}_{(aq)}$ is of the order of:

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In a cell,a copper electrode was used as a cathode. What is the electrode potential (in $V$) of the copper electrode dipped in $0.1 \ M \ Cu^{2+}$ solution at $298 \ K$?
$(E_{Cu^{2+}/Cu}^{\ominus} = 0.34 \ V; \frac{2.303 \ RT}{F} = 0.06 \ V)$

The cell reaction of the given cell is spontaneous if:
$Pt | Cl_2 (P_1 \, atm) | Cl^{-} (1 \, M) || Cl^{-} (1 \, M) | Cl_2 (P_2 \, atm) | Pt$