For the cell reaction- 2Cu-aq- Cus-Cu2-aq- the standard cell potential is 0-36V- The equilibrium constant for the reaction is-

The correct option is A 1.2× 10^6 We know that, logK=E^0_cell× n0.0591 For the given reaction, n=1 logK=0.36× 10.0591 =6.09 K_c= ...

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Standard XII

Chemistry

Equilibrium Constant from Nernst Equation

For the cell ...

Question

For the cell reaction: $2 C u_{(a q)}^{+} \to C u_{(s)} + C u_{(a q)}^{2 +}$ , the standard cell potential is $0.36 V .$ The equilibrium constant for the reaction is?

1.2 \times 10^{6}

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7.4 \times 10^{12}

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2.4 \times 10^{6}

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5.5 \times 10^{8}

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Solution

The correct option is A $1.2 \times 10^{6}$
We know that,

$l o g K = \frac{E_{c e l l}^{0} \times n}{0.0591}$

For the given reaction, $n = 1$

$l o g K = \frac{0.36 \times 1}{0.0591}$ $= 6.09$

$K_{c} =$ antilog $6.09 = 1.2 \times 10^{6}$

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Similar questions

Given the half cell reactions:
$C u^{+} (a q) + e^{-} \to C u (s); E^{0} = + 0.52 V C u^{2 +} (a q) + e^{-} \to C u^{+} (a q); E^{0} = + 0.165 V$
The equilibrium constant for the disproportionation reaction at 298 K is:
$2 C u^{+} (a q) \to C u (s) + C u^{2 +} (a q)$

$E^{0}$ for the cell, $Z n | Z n {^{2 +}}_{(a q)} | | C u {^{2 +}}_{(a q)} | C u$ is $1.10 V$ at $25^{0} C$ . The equilibrium constant for $Z n + C u {^{2 +}}_{(a q)} \to Z n {^{2 +}}_{(a q)} + C u$ the cell reaction is of the order of :