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

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

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

Step 1: Understand the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g). This means we have 1 mole of N2 and 3 moles of H2 on the left side, and 2 moles of NH3 on the right side.
Step 2: Count the total moles of gas on each side. The left side has 1 + 3 = 4 moles of gas, and the right side has 2 moles of gas.
Step 3: Know 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 when the volume decreases, the equilibrium will shift towards the side with fewer moles of gas to reduce the pressure.
Step 6: Identify which side has fewer moles of gas. The right side has 2 moles of NH3, which is fewer than the 4 moles on the left side.
Step 7: Conclude that the equilibrium will shift to the right side, producing more 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.
Equilibrium Position – The position of equilibrium refers to the relative concentrations of reactants and products in a reversible reaction at equilibrium.
Moles of Gas – In reactions involving gases, the number of moles on each side of the equation can influence the direction of the shift in equilibrium when volume or pressure changes.