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NEET levelSingle correct optionDifficulty 1 of 3ce007

For $N X_{2} (g) + 3 H X_{2} (g) 2 NH X_{3} (g)$ at equilibrium, the pressure is increased at constant temperature by decreasing the volume. The equilibrium shifts

Atowards $NH X_{3}$ (forward), because there are fewer gas moles on the product side
Btowards $N X_{2}$ and $H X_{2}$ (backward), because there are more gas moles on the product side
Cneither way, because the number of gas moles is the same on both sides
Dtowards $NH X_{3}$ , because $K_{c}$ increases with pressure

Answer: A

Increasing pressure favours the side with fewer moles of gas (Le Chatelier). Reactants have 4 mol of gas and products 2 mol, so the shift is forward.

K_{c}

does not change with pressure.

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