alcohol + acetic acid H2SO ester product 60.05 3.0 mL 1.05 g/mL 1.5 mL 2-3 drops

Question

alcohol + acetic acid H2SO ester product 60.05 3.0 mL 1.05 g/mL 1.5 mL 2-3 drops volume density mass mmol equiv. Theoretical Yield Theoretical Yield cat.* number of equivalents based on reaction stoichiometry/amounts used. catalytic amount 4. a) Show your calculations to determine the maximum possible amount (= maximum theoretical yield) of ester using the amounts in the table above. (1 point): b) As can be deduced from the table above, excess acetic acid is used in this reaction. Explain why (in two sentences or less) (2 point):

Explanation / Answer

4(a)

Volume of alcohol is = 1.5 ml

Volume of acetic acid is = 3.0 ml

Density of acid is = 1.05 g/ml

MW of acid is = 60.05

now according to simple mole concept 1.5 ml of alcohol will consume 1.5 ml of acetic acid.

so the theoretical yield would be 1.5 ml of acid

or, 1.5ml*1.05 g/ml= 1.575 g of Acetic acid

moles of acid = weight/MW

= 1.575/60.05

= 0.02622 moles or 26.22 mili-moles as 1 mole as 1000 mili-moles

4(b)

Since the given reaction is an equilibrium so, both backward and forward reactions must be going on simultaneously , to favour the forward reaction the acid has been taken in access (Le-Chatelier's principle)

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