Aspirin (C9H8O4) is produced from salicylic acid (C7H6O3) and acetic anhydride (

Question

Aspirin (C9H8O4) is produced from salicylic acid

(C7H6O3) and acetic anhydride (C4H6O3):

C7H6O3+C4H6O3?C9H8O4+HC2H3O2.

a)  How much salicylic acid is required to produce 190kg of aspirin, assuming that all of the salicylic acid is converted to aspirin?

b)  How much salicylic acid would be required if only 85% of the salicylic acid is converted to aspirin?

c)  What is the theoretical yield of aspirin if 180kg of salicylic acid is allowed to react with 122kg of acetic anhydride?

d)  If the situation described in part (c) produces 174kg of aspirin, what is the percentage yield?

If you could also show the steps so I know how to approach this problem in the future, that would be great!  

Thanks!

Explanation / Answer

a)Moles aspirin = 190000 g / 180.16 g/mol =1054.62

= moles salicylic acid

Mass salicylic acid = 1054.62 mol x 138.123 g/mol =145667 g => 145.667 Kg


b)145.667 x 100 / 85 = 171.373 Kg

c)
Moles salicylic acid = 180000 g / 138.123 =1303
Moles acetic anhydride = 122000 g / 102.1 g/mol =1194.9

Since the ratio is 1 : 1 acetic anhydride is the limiting reactant

we would get 1194.9 moles of aspirin

d)Mass aspirin = 1194.9 mol x 180.16 =215274.437 g => 215.275 Kg

174 x 100 / 215.275 =80.827 %

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