(D) The Nernst equation for the reaction is: $E = E^{\circ} - \frac{0.0591}{n} \log \frac{[Cr^{3+}]^2}{[Cr_2O_7^{2-}][H^{+}]^{14}}$Given $E^{\circ} =

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(D) The Nernst equation for the reaction is: $E = E^{\circ} - \frac{0.0591}{n} \log \frac{[Cr^{3+}]^2}{[Cr_2O_7^{2-}][H^{+}]^{14}}$Given $E^{\circ} = 1.33 \ V$,$n = 6$,$[Cr^{3+}] = 1 \ M$,$[Cr_2O_7^{2-}] = 1 \ M$,and $pH = 2.0$,so $[H^{+}] = 10^{-2} \ M$.Substituting the values: $E = 1.33 - \frac{0.0591}{6} \log \frac{1^2}{1 \times (10^{-2})^{14}}$$E = 1.33 - \frac{0.0591}{6} \log (10^{28})$$E = 1.33 - \frac{0.0591}{6} \times 28$$E = 1.33 - 0.2758 = 1.0542 \ V$.

Class 12 Chemistry Electrochemistry Nernst equation and ECS

Medium

The standard electrode potential for the following reaction is $+1.33 \ V$. What is the potential at $pH = 2.0$ for the reaction: $Cr_2O_7^{2-} (aq, 1 \ M) + 14H^{+} (aq) + 6e^{-} \rightarrow 2Cr^{3+} (aq, 1 \ M) + 7H_2O (l)$?

A
$1.820 \ V$
B
$+1.990 \ V$
C
$+1.608 \ V$
D
$+1.054 \ V$

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Electrochemistry

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Nernst equation and ECS

$A$ copper electrode is dipped in a $0.1 \, M$ copper sulfate solution at $25 \, ^\circ C$. Calculate the reduction potential of the copper electrode. $(E^o_{Cu^{2+}/Cu} = 0.34 \, V)$ (in $, V$)

Medium

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The potential of the cell for the reaction $M_{(s)} + 2H^{+}(1 \ M) \to H_2(1 \ atm) + M^{2+}(0.1 \ M)$ is $1.5 \ V$. The standard reduction potential for $M^{2+}/M_{(s)}$ couple is ............. $V$.

Medium

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For the redox reaction $Zn(s) + Cu^{2+}(0.1 \ M) \rightarrow Zn^{2+}(1 \ M) + Cu(s)$,given $E^o_{cell} = 1.10 \ V$,calculate the $E_{cell}$ value in $V$. (Given: $2.303 \frac{RT}{F} = 0.0591$) (in $V$)

Easy

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If $A$ is the reactant and $P$ is the product,which one of the following is the correct form of the Nernst equation?

MediumTS EAMCET 2019

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For the cell $Zn_{(s)} | Zn^{2+} (0.1 \ M) || Fe^{2+} (0.01 \ M) | Fe_{(s)}$ at $298 \ K$,$E_{cell} = 0.2905 \ V$. What is the equilibrium constant $(K_c)$ for the reaction $Zn_{(s)} + Fe^{2+}_{(aq)} \rightleftharpoons Zn^{2+}_{(aq)} + Fe_{(s)}$?

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The standard electrode potential for the following reaction is $+1.33 \ V$. What is the potential at $pH = 2.0$ for the reaction: $Cr_2O_7^{2-} (aq, 1 \ M) + 14H^{+} (aq) + 6e^{-} \rightarrow 2Cr^{3+} (aq, 1 \ M) + 7H_2O (l)$?

Similar Questions

$A$ copper electrode is dipped in a $0.1 \, M$ copper sulfate solution at $25 \, ^\circ C$. Calculate the reduction potential of the copper electrode. $(E^o_{Cu^{2+}/Cu} = 0.34 \, V)$ (in $, V$)

The potential of the cell for the reaction $M_{(s)} + 2H^{+}(1 \ M) \to H_2(1 \ atm) + M^{2+}(0.1 \ M)$ is $1.5 \ V$. The standard reduction potential for $M^{2+}/M_{(s)}$ couple is ............. $V$.

For the redox reaction $Zn(s) + Cu^{2+}(0.1 \ M) \rightarrow Zn^{2+}(1 \ M) + Cu(s)$,given $E^o_{cell} = 1.10 \ V$,calculate the $E_{cell}$ value in $V$. (Given: $2.303 \frac{RT}{F} = 0.0591$) (in $V$)

If $A$ is the reactant and $P$ is the product,which one of the following is the correct form of the Nernst equation?

For the cell $Zn_{(s)} | Zn^{2+} (0.1 \ M) || Fe^{2+} (0.01 \ M) | Fe_{(s)}$ at $298 \ K$,$E_{cell} = 0.2905 \ V$. What is the equilibrium constant $(K_c)$ for the reaction $Zn_{(s)} + Fe^{2+}_{(aq)} \rightleftharpoons Zn^{2+}_{(aq)} + Fe_{(s)}$?

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