Aspirin (C9H8O4) is produced from salicylic acid (C7H6O3), and acetic anhydride (C4H6O3), as shown below.
C7H6O3 + C4H6O3 → C9H8O4 + HC2H3O2
(a) How much salicylic acid is required to produce 1.0 102 kg of aspirin, assuming that all of the salicylic acid is converted to aspirin?
(b) How much salicylic acid would be required if only 56% of the salicylic acid is converted to aspirin?
(c) What is the theoretical yield of aspirin if 181 kg of salicylic acid is allowed to react with 124 kg of acetic anhydride?
Thank you for the opportunity to help you with your question!
a) molar mass of aspirin=148
molar mass of salicylic acid=114
b) 56 percent=77.03kg
aspirins molar mass is 180.17
and salyic acid is 138.13
so have you used the molar masses while doing the calculating the masses?
i figured out (a) but can you please explain b your work is a little ambiguous
and c is wrong
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