Question

A student reacts 36g of salicylic acid with 60 mL of acetic anhydride producing 29.5g of acetyl salicylic acid. What is the percent yield of the reaction?

Answer 1

62.82%

Step-by-step explanation:

From the equation of reaction:

`C_7H_6O_3 + C_4H_6O_3 --> C_9H_8O_4 + C_2H_4O_2`

1 mole of salicyclic acid requires 1 mole of acetic anhydride to yield 1 mole of aspirin (acetyl salicyclic acid).

Mass of 1 mole of salicyclic acid = 138.121 g

Mass of 1 mole of acetic anhydride = 102.09 g

Mass of 1 mole of aspirin = 180.158 g

Therefore,

138.121 g of salicyclic acid is supposed to yield 180.158 g of aspiring

36 g of salicyclic acid will yield = 180.158 x 36/138.121

= 46.957 g of aspiring

But 29.5 g of aspirin was produced.

Hence, percent yield of the reaction = 29.5/46.957 x 100%

= 62.82%

The percentage yield of the reaction is 62.82%.

Answer 2

The percentage yield for this reaction is 62.8%

Step-by-step explanation:

The reaction for this equation is:

C7H6O3 + C4H6O3 → C9H8O4 + CH3COOH

The mole ratio of salicylic acid to acetyl salicylic acid (C7H6O3) is 1 : 1 (equal moles)

If 1 mole C7H6O3 - 138.12 g

? moles C7H6O3- 36g

= 36/138.121 = 0.2606 mole

But 1 mol of C9H8O4 - 180.158 grams

0.2606 mole of C9H8O4 - ? grams

= 180.158 × 0.2606 = 46.9566 g

⇒ 46.9566g acetyl salicylic acid is supposed to be produced during this reaction (theoretical yield). However, the experiment yielded 29.5 g acetyl salicylic acid (experimental yield).

% Yield =
`(Experimental Yield)/(THeoritical Yield)` × 100

=
`(29.5)/(46.9566)` × 100

% Yield = 62.8 %