Question

What amount of acid is esterified if a mixture consists initially of 1.0 mole of ethanoic acid, 1.0 mole of ethanol, and 1.0 mole of water? Given that the equilibrium constant for the reaction at 100 degrees Celsius is 4.0 CH3COOH+CH3CH2OH→CH3COOCH2CH3+H2O.

A. 0.25 mole
B. 0.5 mole
C. 1.0 mole
D. 2.0 moles

Answer 1

The amount of acid esterified is 0.171 moles, which is the same as the amount of ethanol consumed.

Step-by-step explanation:

The equilibrium constant for the reaction CH3COOH + CH3CH2OH → CH3COOCH2CH3 + H2O at 100 degrees Celsius is 4.0.

Given that the initial mixture consists of 1.0 mole of ethanoic acid (CH3COOH), 1.0 mole of ethanol (CH3CH2OH), and 1.0 mole of water (H2O), we can use the equilibrium constant to determine the equilibrium concentrations of the species.

Since the coefficients of both ethanoic acid and ethanol are 1 in the balanced chemical equation, the mole ratio for the reactant is 1:1. Therefore, the limiting reactant is ethanol and the excess reactant is ethanoic acid.

Hence, the amount of acid esterified is 0.171 moles, which is the same as the amount of ethanol consumed.