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Aspirin can be prepared from salicylic acid ( C 7 H 6 O 3 ), which has a molar mass of 138.12 g/mol, and acetic anhydride ( C 4 H 6 O 3 ), which has a molar mass of 102.04 g/mol. The density of acetic anhydride is 1.082 g/mL. C 7 H 6 O 3 + C 4 H 6 O 3 ⟶ C 9 H 8 O 4 + C 2 H 3 O 2 What is the yield of aspirin ( C 9 H 8 O 4 ), which has a molar mass of 180.15 g/mol, possible when reacting 2.18 g of salicylic acid with 1.01 mL of acetic anhydride?

Respuesta :

Answer:

1.93 g.

Explanation:

The mass of acetic anhydride used = density * volume == 1.01 * 1.082

= 1.09282 g

C 7 H 6 O 3 + + C 4 H 6 O 3 ⟶ C 9 H 8 O 4 + C 2 H 4 O 2

138.12 g of salicylic acid reacts with 102.04 g of acetic anhydride  to give

180.15 g aspirin.

So maximum possible yield  for 1.09282 g of acetic anhydride  is

(180.15 / 102.04) * 1.09282 = 1.93 g.

Maximum yield for  2.18g of salicylic acid =  (180.15 / 138.12) * 2.18 = 2.84 g

So the answer is 1.93 g.

pstnonsonjoku

The yield of aspirin obtained from the reaction is 1.93 g

Given that;

The reaction equation is

[tex]C7H6O3 + C4H6O3 ------> C9H8O4 + C2H3O2[/tex]

Amount of salicylic acid = 2.18 g/138.12 g/mol = 0.0158 moles

Density of acetic anhydride = 1.082 g/mL

Mass of acetic anhydride =  1.082 g/mL × 1.01 mL = 1.093 g

Amount of acetic anhydride = 1.093 g/102.04 g/mol = 0.0107 moles

We have to find the limiting reactant. It is the reactant that gives the lowest yield of products

Since the mole ratio of the reaction is 1:1:1:1, the limiting reactant is acetic anhydride.

Mass of aspirin produced = 0.0107 moles of asprin × 180.15 g/mol = 1.93 g

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