Question

How to find theoretical yield using 6 mL 1-propanol, 10 mL acetic acid and 1 mL sulfuric acid.

Answer 1

Sulfuric acid is the catalyst for the reaction. There is no need to acknowledge it in calculations.

. Theoretical Yield:

Mass of alcohol used (g):

Mass of acid used (g):

Moles of alcohol (mol):

Moles of acid (mol):

Expected number of moles of ester product (mol):

Molecular weight of ester product (g/mol):

Theoretical yield of ester (g):

CH3CH2CH2OH + CH3COOH à C5H10O2 + H2O

Step 1

We need to calculate mass of alcohol and acid

a) 1-Propanol – Density is 0.803 g/mL = 4.818 g

b) Acetic acid – Density is 1.09 g/mL = 10.9 g

1. Determine the number of moles of one of the propyl ethanoate produced if all

of each reactant is used up.

(i)

10.9 g Acetic Acid * (1mol Acetic acid/60.05 g Acetic acid) * (1mol propyl ethanoate/1mole of Acetic acid)

= 0.1815 mole propyl ethanoate

(ii)

4.818 g Propanol*(1mol propanol/60.09 g Propanol) * (1mol propyl ethanoate/1mole propanol)

= 0.0801 mole propyl ethanoate

Step 2

Use the smallest number of moles of the product from step 1 to calculate the

theoretical yield of product

0.0801 mol propyl ethanoate * (102.131 g Propyl ethanoate/1 mol propyl etha.)

= 8.180 g Propyl ethanoate