Answer:
The percentage yield for this reaction is 62.8%
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 = [tex]\frac{Experimental Yield}{THeoritical Yield}[/tex] × 100
= [tex]\frac{29.5}{46.9566}[/tex] × 100
% Yield = 62.8 %
Answer:
62.82%
Explanation:
From the equation of reaction:
[tex]C_7H_6O_3 + C_4H_6O_3 --> C_9H_8O_4 + C_2H_4O_2[/tex]
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%.
