0.1 points 014 Submissions Used Aspirin, C9H804, is produced from salicylic acid
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Question
0.1 points 014 Submissions Used Aspirin, C9H804, is produced from salicylic acid, C7H603, and acetic anhydride, C4H603, as shown below. 17. My Notes Ask Your Teacher (a) How much salicylic acid is required to produce 1.4 x 102 kg of aspirin, assuming that all of the salicylic acid is converted to aspirin? kg (b) How much salicylic acid would be required if only 53% of the salicylic acid is converted to aspirin? kg (c) What is the theoretical yield of aspirin if 165 kg of salicylic acid is allowed to react with 149 kg of acetic anhydride? kg (d) If the situation described in part (c) produces 159 kg of aspirin, what is the percentage yield?Explanation / Answer
Balanced equation
C7H6O3 + C4H6O3 ---------> C9H8O4 + C2H4O2
Salicylic acid Acetic anhydride Aspirin Acetic acid
1 mol 1 mol 1 mol 1 mol
M W 138.121 102.09 180.157 60.01
a. First we need to calculate the mol of aspirin
mol of aspirin = mass of aspirin/molecular weight of aspirin = 140000 g / 180.157 g/mol =
777.1 mol
From balance equation we know that 1 mol of salicylic acid will produce 1 mol of aspirin, so, 777.1 mol of aspirin will require 777.1 mol of salicylic acid.
Convert mol inti mass
mass of salicylic acid required = mol of salicylic acid × molecular weight of salicylic acid = 777.1 mol × 138.121g/mol = 1.07 × 102 kg.
b. we know that
% of salicylic acid = required salicylic acid /Total salicylic acid ×100
53 = required salicylic acid/ 1.07 × 102 kg × 100
Required salicylic acid = 56.71 kg
c. The salicylic acid is a limiting reagent
Theoretical yield = molecular weight of aspirin/ molecular weight of salicylic acid × mass of salicylic acid = 180.157/138.121× 165 kg = 215. 216 kg.
d. we know that
% yield = practical yield / theoretical yield × 100 = 159 /215.216 × 100 = 73.88 %
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