For the equilibrium reaction N2(g) + 3H2(g) ⇌ 2NH3(g), if the pressure is increased, what will be the effect on the equilibrium?

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Q: For the equilibrium reaction N2(g) + 3H2(g) ⇌ 2NH3(g), if the pressure is increased, what will be the effect on the equilibrium?

Solution: Increasing the pressure will shift the equilibrium to the right, favoring the formation of NH3, which has fewer moles of gas.

Steps: 7

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