Assume equilibrium has been reached in the following reaction:
$A (g) + B (g) ⇌ C (g) + D (g)$
On an increase in the pressure, the system will:

Shift to the products

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Shift to the reactants

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Not change because pressure never affects equilibrium positions

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Not change because there are equal number of moles of gas in reactant and product

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Solution

The correct option is D Not change because there are equal number of moles of gas in reactant and product
The given reaction is :-
$A (g) + B (g) ⇌ C (g) + D (g)$
In this reaction, the no. of moles of gaseous species are same on reactants and product side. So, As per Le Chatelier's principle, pressure will have on effect on it.

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