(A) The Nernst equation describes the relationship between the cell potential and the reaction quotient for an electrochemical cell. The general form

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$E = E^o - \frac{RT}{nF} \ln \frac{[\text{product}]}{[\text{reactant}]}$

(A) The Nernst equation describes the relationship between the cell potential and the reaction quotient for an electrochemical cell. The general form of the Nernst equation is given by $E = E^o - \frac{RT}{nF} \ln Q$,where $Q$ is the reaction quotient,defined as the ratio of the concentration of products to the concentration of reactants. Therefore,the correct expression is $E = E^o - \frac{RT}{nF} \ln \frac{[\text{product}]}{[\text{reactant}]}$.

Class 12 Chemistry Electrochemistry Nernst equation and ECS

Easy

Which of the following is the correct expression for the electrode potential of a cell?

A
$E = E^o - \frac{RT}{nF} \ln \frac{[\text{product}]}{[\text{reactant}]}$
B
$E = E^o + \frac{RT}{F} \ln \frac{[\text{product}]}{[\text{reactant}]}$
C
$E = E^o - \frac{RT}{nF} \ln \frac{[\text{reactant}]}{[\text{product}]}$
D
$E = - \frac{RT}{F} \ln \frac{[\text{product}]}{[\text{reactant}]}$

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Nernst equation and ECS

$A$ hydrogen gas electrode is made by dipping platinum wire in a solution of $HCl$ of $pH = 10$ and by passing hydrogen gas around the platinum wire at $1 \ atm$ pressure. The oxidation potential of the electrode would be $.......... \ V$.

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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 $V$)

Medium

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For the cell reaction $Zn + Cu^{2+} \rightarrow Cu + Zn^{2+}$,the standard $EMF$ value at $25^{\circ}C$ is $1.10 \ V$. If $0.1 \ M \ Cu^{2+}$ and $0.1 \ M \ Zn^{2+}$ solutions are used,the $EMF$ will be .......... $V$.

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At $298 \ K$, the $emf$ of the cell is ............ $V$.
$Pt | H_{2(2 \ atm)} | H_{(0.02 \ M)}^{+} || H_{(0.1 \ M)}^{+} | H_{2(1 \ atm)} | Pt$

Medium

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Calculate $E_{cell}$ of the reaction $Mg_{(s)} + 2Ag^{+}_{(aq)} (0.0001 \ M) \to Mg^{2+}_{(aq)} (0.100 \ M) + 2Ag_{(s)}$ in $V$. If $E^o_{cell} = 3.17 \ V$.

Medium

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Which of the following is the correct expression for the electrode potential of a cell?

Similar Questions

$A$ hydrogen gas electrode is made by dipping platinum wire in a solution of $HCl$ of $pH = 10$ and by passing hydrogen gas around the platinum wire at $1 \ atm$ pressure. The oxidation potential of the electrode would be $.......... \ V$.

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 $V$)

For the cell reaction $Zn + Cu^{2+} \rightarrow Cu + Zn^{2+}$,the standard $EMF$ value at $25^{\circ}C$ is $1.10 \ V$. If $0.1 \ M \ Cu^{2+}$ and $0.1 \ M \ Zn^{2+}$ solutions are used,the $EMF$ will be .......... $V$.

At $298 \ K$, the $emf$ of the cell is ............ $V$.$Pt | H_{2(2 \ atm)} | H_{(0.02 \ M)}^{+} || H_{(0.1 \ M)}^{+} | H_{2(1 \ atm)} | Pt$

Calculate $E_{cell}$ of the reaction $Mg_{(s)} + 2Ag^{+}_{(aq)} (0.0001 \ M) \to Mg^{2+}_{(aq)} (0.100 \ M) + 2Ag_{(s)}$ in $V$. If $E^o_{cell} = 3.17 \ V$.

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At $298 \ K$, the $emf$ of the cell is ............ $V$.
$Pt | H_{2(2 \ atm)} | H_{(0.02 \ M)}^{+} || H_{(0.1 \ M)}^{+} | H_{2(1 \ atm)} | Pt$