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JEE Main levelOne or more correct optionsDifficulty 2 of 3ce031

For the equilibrium $N X_{2} (g) + 3 H X_{2} (g) 2 NH X_{3} (g)$ at constant temperature, which of the following changes will shift the equilibrium in the forward direction (towards $NH X_{3}$ )?

ADecreasing the volume of the container
BAdding more $N X_{2}$ at constant volume
CAdding argon at constant volume
DRemoving some $NH X_{3}$ from the vessel at constant volume

Answer: A, B, D

Decreasing the volume favours fewer gas moles (forward). Adding

N X_{2}

or removing

NH X_{3}

makes

Q_{c} < K_{c}

, so the reaction goes forward. Argon at constant volume leaves all concentrations unchanged, so there is no shift.

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