Stoichem stuff problems

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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?

All

Jul 24th, 2015

Thank you for the opportunity to help you with your question!

a) molar mass of aspirin=148

molar mass of salicylic acid=114

114x100kg/148=77.03kg

b) 56 percent=77.03kg

100x77.03/56

=137.55kg

c) 181/124

=1.46

Please let me know if you need any clarification. I'm always happy to answer your questions.
Jul 24th, 2015

aspirins molar mass is 180.17

Jul 24th, 2015

and salyic acid is 138.13

Jul 24th, 2015

so have you used the molar masses while doing the calculating the masses?

Jul 24th, 2015

i figured out (a) but can you please explain b your work is a little ambiguous

Jul 24th, 2015

and c is wrong


Jul 24th, 2015

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