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 pressure is increased?

For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium position if the pressure is increased?

Correct Answer: Equilibrium shifts to the right side (towards NH3).

Step 1: Identify the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g).
Step 2: Count the number of gas moles on each side of the reaction.
Step 3: On the left side (reactants), there are 1 mole of N2 and 3 moles of H2, totaling 4 moles.
Step 4: On the right side (products), there are 2 moles of NH3.
Step 5: Compare the total moles: 4 moles on the left and 2 moles on the right.
Step 6: Understand that increasing pressure favors the side with fewer moles of gas.
Step 7: Since the right side has fewer moles (2 moles), the equilibrium will shift to the right.

Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in pressure, temperature, or concentration, the system will adjust to counteract that change and restore a new equilibrium.
Mole Count in Gaseous Reactions – Understanding the relationship between the number of moles of gas on each side of a reaction is crucial for predicting the direction of the shift in equilibrium when pressure changes.