See image — Alcohols Phenols and Ethers Chemistry Question

💡 Solution & Explanation

Concept: Le Chatelier's Principle states that if a stress is applied to a system at equilibrium, the system will shift to partially counteract that stress. The reaction is: CH3COOH + CH3OH <=> CH3COOCH3 + H2O This is an esterification equilibrium reaction (acetic acid + methanol <=> methyl acetate + water). Analyzing each option: (a) Equimolar quantities of reactants: With equimolar starting amounts, the equilibrium constant (Keq ≈ 4 for typical esterifications) means the conversion is only about 2/3, not the greatest possible yield. Using excess of one reactant would give a higher yield. So (a) is FALSE. (b) Removal of water: Water is a product on the right side. By Le Chatelier's Principle, removing a product shifts the equilibrium to the RIGHT (toward products), increasing the formation of ester. This is correct and TRUE. Removal of water drives the forward reaction, producing more CH3COOCH3. (c) Addition of CH3COOCH3: Adding a product (ester) shifts the equilibrium to the LEFT (toward reactants), producing more CH3COOH and CH3OH, NOT more water in equal moles to the ester added. The equilibrium shifts back, so the statement 'equal number of moles of water' formed is not necessarily accurate — the shift produces reactants, not water equivalently. So (c) is misleading/FALSE as stated. (d) Application of pressure: Both sides of the reaction have equal moles of gas (in solution-phase reactions, pressure has negligible effect; and even in gas phase, both sides have 2 moles total: 2 moles reactants and 2 moles products). Since moles on both sides are equal, pressure change does not shift the equilibrium. So (d) is FALSE. Therefore, the correct answer is B.