For the equilibrium reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens if the volum

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Question: For the equilibrium reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens if the volume of the container is decreased?

Options:

Correct Answer: Shift to the right

Solution:

Decreasing the volume increases the pressure, which shifts the equilibrium to the side with fewer moles of gas, favoring the production of NH3.

For the equilibrium reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens if the volume of the container is decreased?

For the equilibrium reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens if the volume of the container is decreased?

Step 1: Understand that the reaction involves gases: N2, H2, and NH3.
Step 2: Recognize that decreasing the volume of the container increases the pressure inside the container.
Step 3: Know that in a chemical equilibrium, the system will respond to changes to minimize the effect of that change.
Step 4: Identify the number of moles of gas on each side of the reaction: 1 mole of N2 + 3 moles of H2 = 4 moles of gas on the left side, and 2 moles of NH3 on the right side.
Step 5: Since there are fewer moles of gas (2 moles) on the right side (NH3) compared to the left side (4 moles), the equilibrium will shift to the right to reduce the pressure.
Step 6: Conclude that decreasing the volume favors the production of NH3.

Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in conditions (such as pressure or volume), the equilibrium will shift in a direction that counteracts that change.
Gas Laws – Understanding how changes in volume affect pressure and the behavior of gases in a chemical reaction.
Stoichiometry of Gases – Recognizing the relationship between the number of moles of gas and the volume of the container in equilibrium reactions.