In the reaction $A + B ⇌ A B$ , if the concentration of A and B is increased by a factor of 2, it will cause the equilibrium concentration of AB to change to :

Two times to original value

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Three times to original value

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Same

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Zero

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Solution

The correct option is A Two times to original value
For $A + B ⇌ A B$
$K = \frac{[A B]}{[A] [B]}$
When $2 A + 2 B ⇌ 2 A B$
$K = 2 A B$

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In the reaction A+B⇌AB, if the concentration of A and B is increased by a factor of 2, it will cause the equilibrium concentration of AB to change to :

The correct option is A Two times to original valueFor A+B⇌ABK=[AB][A][B]When 2A+2B⇌2ABK=2AB

In the reaction $A + B ⇌ A B$ , if the concentration of A and B is increased by a factor of 2, it will cause the equilibrium concentration of AB to change to :

The correct option is A Two times to original value
For $A + B ⇌ A B$
$K = \frac{[A B]}{[A] [B]}$
When $2 A + 2 B ⇌ 2 A B$
$K = 2 A B$