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Standard XII

Chemistry

Effective Equilibrium Constant

In a reaction...

Question

In a reaction $A + B ⇌ C + D$ , $40 %$ of $B$ has reacted at equilibrium, when $1$ mol of $A$ was heated with $1$ mol of $B$ in a $10$ litres closed vessel. The value of $K_{c}$ is:

0.44

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0.18

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0.22

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0.36

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Solution

The correct option is A $0.44$
A B C D
Initial number of moles 1 1
0
0
Equilibrium number of moles
0.6 0.6 0.4 0.4
Equilibrium molar concentration
0.06 0.06 0.04 0.04

The equilibrium constant expression is:

$K = \frac{[C] [D]}{[A] [B]}$

$K = \frac{0.04 \times 0.04}{0.06 \times 0.06} = 0.44$

Note: Since B is $40 %$ dissociated at equilibrium, the number of moles of B that have decomposed to reach equilibrium are $1 m o l \times \frac{40}{100} = 0.4$
The number of moles of B present at equilibrium are $1 - 0.4 = 0.6$ .

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	A	B	C	D
Initial number of moles	1	1	0	0
Equilibrium number of moles	0.6	0.6	0.4	0.4
Equilibrium molar concentration	0.06	0.06	0.04	0.04

In a reaction A+B⇌C+D, 40% of B has reacted at equilibrium, when 1 mol of A was heated with 1 mol of B in a 10 litres closed vessel. The value of Kc is:

In a reaction $A + B ⇌ C + D$ , $40 %$ of $B$ has reacted at equilibrium, when $1$ mol of $A$ was heated with $1$ mol of $B$ in a $10$ litres closed vessel. The value of $K_{c}$ is: