A 4.0 g sample of acetic acid is esterified with excess ethanol in the presence of concentrated H₂SO₄ to give ethyl acetate. Calculate the theoretical mass of ethyl acetate that can be formed. (Molar mass CH₃COOH = 60.05 g mol⁻¹, CH₃COOC₂H₅ = 88.11 g mol⁻¹.)

Step-by-step solution

1. Determine moles of acetic acid: $\frac{4.0\text{ g}}{60.05{\text{ g mol}}^{-1}}=0.0666\text{ mol}$.
2. The esterification stoichiometry is 1:1: 1 mol acetic acid → 1 mol ethyl acetate.
3. Hence moles of ethyl acetate produced = 0.0666 mol.
4. Calculate mass of ethyl acetate: $0.0666\text{ mol}\times 88.11{\text{ g mol}}^{-1}=5.87\text{ g}$.
5. Theoretical mass of ethyl acetate that can be formed is 5.87 g.

Concept tested: Fischer esterification yield calculation

Published 11 September 2026 · Last updated 16 September 2026 · How this solution was prepared and checked