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

For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium if the volume of the container is decreased? (2020)

For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium if the volume of the container is decreased? (2020)

Step 1: Understand that the reaction involves gases: N2, H2, and NH3.
Step 2: Identify the number of gas molecules on each side of the reaction.
Step 3: Count the moles of gas: On the left side (reactants), there are 1 mole of N2 and 3 moles of H2, totaling 4 moles. On the right side (products), there are 2 moles of NH3.
Step 4: Recognize that decreasing the volume of the container increases the pressure of the gases inside.
Step 5: Apply Le Chatelier's principle, which states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.
Step 6: Since there are fewer moles of gas on the right side (2 moles of NH3) compared to the left side (4 moles of N2 and H2), the equilibrium will shift to the right side to reduce the pressure.

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 and pressure affect gas behavior and equilibrium in chemical reactions.