In a reaction $A + B ⇌ C + D$ , the rate constant of forward reaction and backward reaction is $K_{1}$ and $K_{2}$ , then the equilibrium constant (K) for reaction is expressed as

K_{c} = \frac{K_{2}}{K_{1}}

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K_{c} = \frac{K_{1}}{K_{2}}

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K_{c} = K_{1} \times K_{2}

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K_{c} = K_{1} + K_{2}

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Solution

The correct option is B $K_{c} = \frac{K_{1}}{K_{2}}$
$r_{f} = k_{1} [A] [B]$
$r_{b} = k_{2} [C] [D]$

At equilibrium, $r_{f} = r_{b} = r$

$K = \frac{[C] [D]}{[A] [B]} = \frac{r / k_{2}}{r / k_{1}} = \frac{k_{1}}{k_{2}}$

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In a reaction A+B⇌C+D, the rate constant of forward reaction and backward reaction is K1 and K2, then the equilibrium constant (K) for reaction is expressed as

The correct option is B Kc=K1K2rf=k1[A][B]rb=k2[C][D]At equilibrium, rf=rb=rK=[C][D][A][B]=r/k2r/k1=k1k2

In a reaction $A + B ⇌ C + D$ , the rate constant of forward reaction and backward reaction is $K_{1}$ and $K_{2}$ , then the equilibrium constant (K) for reaction is expressed as

The correct option is B $K_{c} = \frac{K_{1}}{K_{2}}$
$r_{f} = k_{1} [A] [B]$
$r_{b} = k_{2} [C] [D]$

At equilibrium, $r_{f} = r_{b} = r$

$K = \frac{[C] [D]}{[A] [B]} = \frac{r / k_{2}}{r / k_{1}} = \frac{k_{1}}{k_{2}}$