the reaction of salicylic acid (C7H6 O3)with acetic anhydride (C4H6 O3) produces

Question

the reaction of salicylic acid (C7H6 O3)with acetic anhydride (C4H6 O3) produces aspirin (C9H8 O4) and acetic acid (C2H4 O2) according to the following equation :
C7H6O3+C4H6O3-->C9H8O4+C2H4O2
assuming the reaction goes to completion if salicylic acid is reacted with an excess of acetic anhydride to produce 2.70kg of aspirin , how many grams of salicylic acid would be needed to complete the reaction? how many moles of salicylic acid is this ? the molar mass of aspirin = 180.3 g/mol and the molar mass of salicylic acid = 138.1 g/mol.

Explanation / Answer

From the above equation we can see that, 1 mole of salicylic acid produces 1 mole of aspirin.

Now, given is 2.7 kG (2700 g) of aspirin.

Let us convert this into moles of aspirin

moles = 2700 / 180.3 = 14.98 moles

Now, since moles of aspirin = moles of salicylic acid

moles of salicylic acid = 14.98 moles

grams of salicylic acid needed will be = 14.98 x 138.1 = 2068 g

Thus 2068 g of salicylic acid would be needed to complete this reaction.

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.