A student performs a Fischer esterification reaction between butanoic acid (6 mL
ID: 557043 • Letter: A
Question
A student performs a Fischer esterification reaction between butanoic acid (6 mL) and 2-propanol (4 mL) catalyzed by sulfuric acid. The density of butanoic acid is 0.953 g/mL and the molar mass is 88 g/mol. The density of 2-propanol is 0.786 g/mL and the molar mass is 60 g/mol. (a) Draw an equation to describe this reaction 3. (b) Calculate the moles of each of the reagents butanoic acid and 2-propanol used in this experiment (c) State which compound is the limiting reagent? (d) What is the molecular formula of the product? e) Calculate the molar mass of the ester product assuming C-12 g/mol; O-16 g/mol and H-l g/mol. (1) Calculate the maximum theoretical yield of the ester product.Explanation / Answer
a) The reaction is :
H2SO4
CH3CH2CH2COOH + (CH3)2CH-OH --------> CH3CH2CH2COOCH(CH3)2 + H2O
b) no. moles butanoic acid = mass/mol.wt
= (6mL x 0.953 g/mL)/88 g/mol
= 0.0715 mol
no. moles of propanol = mass/mol.wt
= (4mL x 0.786 g/mL)/60 g/mol
= 0.0848 mol
C) Therefore, the limiting reagent is butanoic acid, because butanoic acid has less no. moles (0.0717 mol) than propanol.
The answer is butanoic acid.
d) the molecular formula for the product is:
CH3CH2CH2COOCH(CH3)2
Therefore, the molecular formula for the product is: C7H14O2
e) molar mass of the product :
12x7 + 1x14 + 2x16 = 130 g/mol
The molar mass of the product is = 130 g/mol
f) The theoretical yield of the ester is:
Theoretical yield = no.moles of product formed x molar mass of product
= 0.0715 mol x 130 g/mol
= 9.295 g
Therefore, the theoretical yield of ester = 9.30g
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