(A) The cell reaction is: $Ni_{(s)} + 2Ag^{+}_{(aq)} \rightarrow Ni^{2+}_{(aq)} + 2Ag_{(s)}$.Applying the Nernst equation at $298 \ K$: $E_{cell} = E^

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less than $E^{\circ}_{cell}$ by $0.0592 \ V$

(A) The cell reaction is: $Ni_{(s)} + 2Ag^{+}_{(aq)} \rightarrow Ni^{2+}_{(aq)} + 2Ag_{(s)}$.Applying the Nernst equation at $298 \ K$: $E_{cell} = E^{\circ}_{cell} - \frac{0.0591}{n} \log Q$.Here,$n = 2$ and $Q = \frac{[Ni^{2+}]}{[Ag^{+}]^2} = \frac{0.01}{(0.01)^2} = \frac{0.01}{0.0001} = 100$.Substituting the values: $E_{cell} = E^{\circ}_{cell} - \frac{0.0592}{2} \log(100)$.$E_{cell} = E^{\circ}_{cell} - 0.0296 \times 2 = E^{\circ}_{cell} - 0.0592 \ V$.Thus,the cell emf is less than $E^{\circ}_{cell}$ by $0.0592 \ V$.

Class 12 Chemistry Electrochemistry Nernst equation and ECS

Medium

Which of the following statements is true regarding the cell emf at $298 \ K$ for the cell $Ni_{(s)} | Ni^{2+}(0.01 \ M) || Ag^{+}(0.01 \ M) | Ag_{(s)}$?

MHT CET 2025 All MHT CET

A
less than $E^{\circ}_{cell}$ by $0.0592 \ V$
B
greater than $E^{\circ}_{cell}$ by $0.0592 \ V$
C
less than $E^{\circ}_{cell}$ by $0.0296 \ V$
D
greater than $E^{\circ}_{cell}$ by $0.0296 \ V$

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Calculate $\Delta G$ and $E_{cell}$ for the following cell at $298 \ K$ temperature.
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Medium

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What will be the electrode potential of $Cu$ electrode dipped in $0.025 \ M$ $CuSO_4$ solution at $298 \ K$? Given that the standard reduction potential of $Cu^{2+}/Cu$ is $0.34 \ V$.

Medium

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The reduction potential of a half cell consisting of a $Pt$ electrode immersed in $2.0 \ M \ Fe^{2+}$ and $0.02 \ M \ Fe^{3+}$ solution (in $V$) is. Given: $\left(\frac{2.303 \ RT}{F} = 0.059, E^0_{Fe^{3+} \mid Fe^{2+}} = 0.771 \ V\right)$

MediumTS EAMCET 2023

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Consider the single electrode process $2H^{+} + 2e^{-} \rightleftharpoons H_2$ catalyzed by a platinum black electrode in $HCl$ electrolyte. The potential of the electrode is $-0.059 \ V$. What is the concentration of the acid in the hydrogen half-cell if the $H_2$ pressure is $1 \ bar$ (in $M$)?

DifficultTS EAMCET 2017

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Which of the following relations represents the correct relation between standard electrode potential and equilibrium constant?
$I$. $\log K = \frac{nF E^o}{2.303 RT}$
$II$. $K = e^{\frac{nF E^o}{RT}}$
$III$. $\log K = -\frac{nF E^o}{2.303 RT}$
$IV$. $\log K = 0.4342 \frac{nF E^o}{RT}$
Choose the correct statement$(s)$.

MediumAIIMS 2017

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Which of the following statements is true regarding the cell emf at $298 \ K$ for the cell $Ni_{(s)} | Ni^{2+}(0.01 \ M) || Ag^{+}(0.01 \ M) | Ag_{(s)}$?

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Calculate $\Delta G$ and $E_{cell}$ for the following cell at $298 \ K$ temperature.$Al_{(s)} | Al^{3+} (0.01 \ M) || Fe^{2+} (0.02 \ M) | Fe_{(s)}$ $\left[ E^o_{Al^{3+}|Al} = -1.66 \ V \right.$ and $\left. E^o_{Fe^{2+}|Fe} = -0.44 \ V \right]$

What will be the electrode potential of $Cu$ electrode dipped in $0.025 \ M$ $CuSO_4$ solution at $298 \ K$? Given that the standard reduction potential of $Cu^{2+}/Cu$ is $0.34 \ V$.

The reduction potential of a half cell consisting of a $Pt$ electrode immersed in $2.0 \ M \ Fe^{2+}$ and $0.02 \ M \ Fe^{3+}$ solution (in $V$) is. Given: $\left(\frac{2.303 \ RT}{F} = 0.059, E^0_{Fe^{3+} \mid Fe^{2+}} = 0.771 \ V\right)$

Consider the single electrode process $2H^{+} + 2e^{-} \rightleftharpoons H_2$ catalyzed by a platinum black electrode in $HCl$ electrolyte. The potential of the electrode is $-0.059 \ V$. What is the concentration of the acid in the hydrogen half-cell if the $H_2$ pressure is $1 \ bar$ (in $M$)?

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Calculate $\Delta G$ and $E_{cell}$ for the following cell at $298 \ K$ temperature.
$Al_{(s)} | Al^{3+} (0.01 \ M) || Fe^{2+} (0.02 \ M) | Fe_{(s)}$ $\left[ E^o_{Al^{3+}|Al} = -1.66 \ V \right.$ and $\left. E^o_{Fe^{2+}|Fe} = -0.44 \ V \right]$