Aspirin, C9H8O4, is produced from salicylic acid, C7H6O3, and acetic anhydride, C4H6O3, as shown below.
C7H6O3 + C4H6O3 C9H8O4 + HC2H3O2
(b) How much salicylic acid would be required if only 53% of the salicylic acid is converted to aspirin?
(c) What is the theoretical yield of aspirin if 159 kg of salicylic acid is allowed to react with 149 kg of acetic anhydride?
(d) If the situation described in part (c) produces 163 kg of aspirin, what is the percentage yield?
2006-09-04 18:10:17 · 2 answers · asked by cheezzznitz 5 in Science & Mathematics ➔ Mathematics
please answer other questions
2006-09-04 18:10:28 · update #1
b) 1/0.53 = 206%
c) Calculate moles of C7H6O3 and C4H6O3 to determine which is limiting reagent.
d) 1 mole of limiting reagent above gives one mole of product (from your equation), so calculate theoretical yield on that basis then compare practical yield:
% yield = practical yield/theoretical yield x 100
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2006-09-05 05:33:18 · answer #1 · answered by Auriga 5 · 0⤊ 0⤋
Aspirin is acetylsalicylic acid which hydrolyses interior the presence of water to variety salicylic acid and acetic acid. in case you open an previous bottle of aspirin pills you may stumble on a faint heady scent of vinegar (acetic acid).
2016-12-18 05:03:34 · answer #2 · answered by ? 4 · 0⤊ 0⤋