(A) For the given reaction,the number of electrons transferred $n = 2$. Given $E^{\circ}_{cell} = 0.22 \ V$ at $25^{\circ} C$. At equilibrium,the rela

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(A) For the given reaction,the number of electrons transferred $n = 2$. Given $E^{\circ}_{cell} = 0.22 \ V$ at $25^{\circ} C$. At equilibrium,the relationship between $E^{\circ}_{cell}$ and equilibrium constant $K_{C}$ is given by: $E^{\circ}_{cell} = \frac{0.0591}{n} \log K_{C}$ Substituting the values: $0.22 = \frac{0.0591}{2} \log K_{C}$ $\log K_{C} = \frac{0.22 \times 2}{0.0591} \approx 7.445$ $K_{C} = \text{antilog}(7.445) \approx 2.786 \times 10^{7} \approx 2.8 \times 10^{7}$

Class 12 Chemistry Electrochemistry Nernst equation and ECS

Difficult

$H_{2(g)} + 2 AgCl_{(s)} \rightleftharpoons 2 Ag_{(s)} + 2 HCl_{(aq)}$. The $E^{\circ}_{cell}$ at $25^{\circ} C$ for the cell is $0.22 \ V$. The equilibrium constant at $25^{\circ} C$ is

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A
$2.8 \times 10^{7}$
B
$5.2 \times 10^{8}$
C
$2.8 \times 10^{5}$
D
$5.2 \times 10^{4}$

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Class 12

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Electrochemistry

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Nernst equation and ECS

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For the cell at $298 \ K$:
$Ag_{(s)} | AgBr_{(s)} | Br^{-}(0.01 \ M) || I^{-}(0.02 \ M) | AgI_{(s)} | Ag_{(s)}$
The correct information is:
[Given: $K_{sp}(AgBr) = 4 \times 10^{-13}$,$K_{sp}(AgI) = 8 \times 10^{-17}$,$\frac{2.303 \ RT}{F} = 0.06 \ V$,$\log 2 = 0.3$]

Difficult

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At $25\,^{\circ}C$,calculate the equilibrium constant for the cell reaction,
$X_{(s)} + Y_{(aq)}^{2+} \rightleftharpoons Y_{(s)} + X_{(aq)}^{2+}$
Given:
$E_{X^{2+}/X}^{o} = -1.36\,V$;
$E_{Y^{2+}/Y}^{o} = -0.76\,V$; $\frac{2.303\,RT}{F} = 0.06$

Medium

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What is the standard free energy change for the cell,having the following cell reaction (in $kJ$)?
$2 Ag_{(aq)}^{+} + Cd_{(s)} \longrightarrow 2 Ag_{(s)} + Cd_{(aq)}^{2+}, E^{\circ}_{cell} = 1.20 \ V$

MediumMHT CET 2020

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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 .......... $V$.

Medium

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For the cell reaction $Zn_{(s)} + 2H^+_{(aq)} \to Zn^{2+}_{(aq)} + H_{2(g)}$,what happens when $H_2SO_4$ is added to the cathode compartment?

Medium

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$H_{2(g)} + 2 AgCl_{(s)} \rightleftharpoons 2 Ag_{(s)} + 2 HCl_{(aq)}$. The $E^{\circ}_{cell}$ at $25^{\circ} C$ for the cell is $0.22 \ V$. The equilibrium constant at $25^{\circ} C$ is

Similar Questions

For the cell at $298 \ K$:$Ag_{(s)} | AgBr_{(s)} | Br^{-}(0.01 \ M) || I^{-}(0.02 \ M) | AgI_{(s)} | Ag_{(s)}$The correct information is:[Given: $K_{sp}(AgBr) = 4 \times 10^{-13}$,$K_{sp}(AgI) = 8 \times 10^{-17}$,$\frac{2.303 \ RT}{F} = 0.06 \ V$,$\log 2 = 0.3$]

At $25\,^{\circ}C$,calculate the equilibrium constant for the cell reaction,$X_{(s)} + Y_{(aq)}^{2+} \rightleftharpoons Y_{(s)} + X_{(aq)}^{2+}$Given:$E_{X^{2+}/X}^{o} = -1.36\,V$;$E_{Y^{2+}/Y}^{o} = -0.76\,V$; $\frac{2.303\,RT}{F} = 0.06$

What is the standard free energy change for the cell,having the following cell reaction (in $kJ$)?$2 Ag_{(aq)}^{+} + Cd_{(s)} \longrightarrow 2 Ag_{(s)} + Cd_{(aq)}^{2+}, E^{\circ}_{cell} = 1.20 \ V$

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 .......... $V$.

For the cell reaction $Zn_{(s)} + 2H^+_{(aq)} \to Zn^{2+}_{(aq)} + H_{2(g)}$,what happens when $H_2SO_4$ is added to the cathode compartment?

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For the cell at $298 \ K$:
$Ag_{(s)} | AgBr_{(s)} | Br^{-}(0.01 \ M) || I^{-}(0.02 \ M) | AgI_{(s)} | Ag_{(s)}$
The correct information is:
[Given: $K_{sp}(AgBr) = 4 \times 10^{-13}$,$K_{sp}(AgI) = 8 \times 10^{-17}$,$\frac{2.303 \ RT}{F} = 0.06 \ V$,$\log 2 = 0.3$]

At $25\,^{\circ}C$,calculate the equilibrium constant for the cell reaction,
$X_{(s)} + Y_{(aq)}^{2+} \rightleftharpoons Y_{(s)} + X_{(aq)}^{2+}$
Given:
$E_{X^{2+}/X}^{o} = -1.36\,V$;
$E_{Y^{2+}/Y}^{o} = -0.76\,V$; $\frac{2.303\,RT}{F} = 0.06$

What is the standard free energy change for the cell,having the following cell reaction (in $kJ$)?
$2 Ag_{(aq)}^{+} + Cd_{(s)} \longrightarrow 2 Ag_{(s)} + Cd_{(aq)}^{2+}, E^{\circ}_{cell} = 1.20 \ V$