(C) The relationship between standard $emf$ and equilibrium constant $(K_{eq})$ is given by the Nernst equation at $25^o \ C$ $(298 \ K)$: $E^o_{cell}

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(C) The relationship between standard $emf$ and equilibrium constant $(K_{eq})$ is given by the Nernst equation at $25^o \ C$ $(298 \ K)$: $E^o_{cell} = \frac{0.0591}{n} \log K_{eq}$ Given: $E^o_{cell} = 0.295 \ V$,$n = 2$. Substituting the values: $0.295 = \frac{0.0591}{2} \log K_{eq}$ $0.295 \times 2 = 0.0591 \log K_{eq}$ $0.59 = 0.0591 \log K_{eq}$ $\log K_{eq} = \frac{0.59}{0.0591} \approx 10$ Therefore,$K_{eq} = 10^{10}$.

Class 12 Chemistry Electrochemistry Nernst equation and ECS

Easy

For a cell having a standard $emf$ of $0.295 \ V$ at $25^o \ C$ involving a two-electron change,the equilibrium constant for the reaction is:

A
$29.5 \times 10^{-2}$
B
$10$
C
$10^{10}$
D
$29.5 \times 10^{10}$

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Nernst equation and ECS

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 $0.34 \ V$.

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At $298 \ K$,find out the $emf$ for the cell:
$Al_{(s)} | Al^{+3} (0.1 \ M) || Fe^{+2} (0.001 \ M) | Fe_{(s)}$
Given: $E^o_{Al^{+3}/Al} = -1.66 \ V$ and $E^o_{Fe^{+2}/Fe} = -0.44 \ V$.

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$A$ 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 $, V$)

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The standard electrode potential for $Cu^{+2}/Cu$ is $0.34 \ V$. Calculate the reduction potential at $pH = 14$ for the above couple $V$ $[K_{sp}[Cu(OH)_2] = 1 \times 10^{-19}]$

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Which one of the following has a potential more than zero?

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For a cell having a standard $emf$ of $0.295 \ V$ at $25^o \ C$ involving a two-electron change,the equilibrium constant for the reaction is:

Similar Questions

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 $0.34 \ V$.

At $298 \ K$,find out the $emf$ for the cell:$Al_{(s)} | Al^{+3} (0.1 \ M) || Fe^{+2} (0.001 \ M) | Fe_{(s)}$Given: $E^o_{Al^{+3}/Al} = -1.66 \ V$ and $E^o_{Fe^{+2}/Fe} = -0.44 \ V$.

$A$ 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 standard electrode potential for $Cu^{+2}/Cu$ is $0.34 \ V$. Calculate the reduction potential at $pH = 14$ for the above couple $V$ $[K_{sp}[Cu(OH)_2] = 1 \times 10^{-19}]$

Which one of the following has a potential more than zero?

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At $298 \ K$,find out the $emf$ for the cell:
$Al_{(s)} | Al^{+3} (0.1 \ M) || Fe^{+2} (0.001 \ M) | Fe_{(s)}$
Given: $E^o_{Al^{+3}/Al} = -1.66 \ V$ and $E^o_{Fe^{+2}/Fe} = -0.44 \ V$.