10. Given the equation representing a reaction at equilibrium:

N₂(g) + 3H₂(g) ↔ 2NH₃(g) + energy

Which change causes the equilibrium to shift to the right?

A)    Decreasing the concentration of H₂(g)

B)    Decreasing the pressure

C)    Increasing the concentration of N₂(g)

D)    Increasing the temperature

Correct Answer: Option C - Increasing the concentration of N₂(g)

Increasing the concentration of nitrogen gas aids, further reaction with hydrogen thus forming more ammonia and releasing more energy; shifting the reaction to the right.

Incorrect Options:

Decreasing the concentration of hydrogen will make lesser hydrogen available for the reaction causing the reaction to shift left. Hence, option A is incorrect.

Pressure is not involved in the reaction; hence, decreasing the pressure will not affect the reaction. Hence, option B is incorrect.

Increasing the temperature will increase the right side elements in the reaction, causing the reaction to shift left. Hence, option D is incorrect.