Le Chatelier's Principle on Pressure in Gaseous Equilibria

Steps:

• Count gas moles: 1 on left (SO2Cl2), 2 on right (SO2 + Cl2).
• Increasing pressure favors fewer moles, shifting equilibrium left to reduce pressure.
• Higher pressure increases molecular collisions, raising both forward and reverse rates.
• Net effect: rates increase, but equilibrium position moves left.

Why C is correct:

• Le Chatelier's principle dictates shift to fewer moles (left) under increased pressure; higher concentrations boost collision frequency, increasing rates per kinetic molecular theory.

Why the others are wrong:

• A: Rates increase, not decrease, with pressure.
• B: Equilibrium shifts left, not right, due to mole difference.
• D: Equilibrium moves left, not right, to oppose pressure increase.

Final answer: C