Chem Lab 2

# Chem Lab 2 - Synthesis of Aspirin 1 Calculations for the...

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Synthesis of Aspirin 1. Calculations for the Economics of Industrial Preparation of Aspirin For a bulk preparation of a minimum of 25.00 kg of aspirin, I used the following equation: C 7 H 6 O 3 + C 4 H 6 O 3 C 9 H 8 O 4 + CH 3 COOH. First, I determined the theoretical yield of aspirin. Since we assumed a 90% yield, the theoretical yield is 27.78 kg (percentage yield = (experimental yield/theoretical yield) x 100, so 25 kg = 0.9x). As a result of the following stoichiometeric equations, I was able to determine that I would need 21.3 kg of salicylic acid (C 7 H 6 O 3 ) and 14.55 L of acetic anhydride. •(27.78 kg C 9 H 8 O 4 )(1000 g/ kg)(mole C 9 H 8 O 4 / 180.16 g C 9 H 8 O 4 )(mole C 9 H 8 O 4 / mole C 7 H 6 O 3 )(138.12 g C 7 H 6 O 3 / mole C 7 H 6 O 3 )(1000 g/ kg)= 21.3 kg salicylic acid •(27.78 kg C 9 H 8 O 4 )(1000 g/ kg)(mole C 9 H 8 O 4 / 180.16 g C 9 H 8 O 4 )(mole C 9 H 8 O 4 / mole C 4 H 6 O 3 )(102.09 g C 4 H 6 O 3 / mole C 4 H 6 O 3 )(ml/ 1.082 g)(1000ml/L)= 14.55 L acetic

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## This note was uploaded on 05/18/2008 for the course CHEM 11171 taught by Professor Johnson during the Fall '08 term at Notre Dame.

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Chem Lab 2 - Synthesis of Aspirin 1 Calculations for the...

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