What will happen to the equilibrium position of the reaction N2(g) + 3H2(g) ⇌ 2N

What will happen to the equilibrium position of the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) when the pressure is increased?

What will happen to the equilibrium position of the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) when the pressure is increased?

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 vs. 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.

No concepts available.