For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what is the effect of decreasing the

For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what is the effect of decreasing the volume of the container?

For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what is the effect of decreasing the volume of the container?

Step 1: Understand the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g). This means nitrogen gas and hydrogen gas react to form ammonia gas.
Step 2: Note that there are 4 moles of gas on the left side (1 N2 + 3 H2) and 2 moles of gas on the right side (2 NH3).
Step 3: Recognize that decreasing the volume of the container increases the pressure inside the container.
Step 4: Apply Le Chatelier's Principle, which states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.
Step 5: Since the pressure increases, the equilibrium will shift to the side with fewer moles of gas to reduce the pressure.
Step 6: Identify that the right side (2 NH3) has fewer moles of gas (2 moles) compared to the left side (4 moles).
Step 7: Conclude that the equilibrium will shift to the right, favoring the production of ammonia (NH3).

Le Chatelier's Principle – This principle states that if an external change is applied to a system at equilibrium, the system will adjust to counteract that change and restore a new equilibrium.
Gas Laws – Understanding how changes in volume affect pressure and the behavior of gases in a closed system.
Stoichiometry of Gases – Recognizing the relationship between the number of moles of reactants and products in a chemical reaction.