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The chemical reaction of 100 g of salicylic acid, C7H6O3, with excess acetic anhydride produces 50.0 g of aspirin, C9H8O4, according to the equation. What is the percentage yield for the reaction shown below? Please show your work.
C7H6O3 + C4H6O3 → C9H8O4 + C2H4O2

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manjotsanghera628

C7H6O3 + C4H6O3 → C9H8O4 + C2H4O2

Convert the 100g of salicylic acid (SA) into moles and the ratio is 1:1.

Convert moles of aspirin into grams of aspirin where grams = molar mass *moles which is the theoretical yield.Percentage yield =50g (actual yield)* 100

Percentage yield for the reaction is 38.3%.

Reaction:-

[tex]C_7H_6O_3 + C_4H_6O_3 \rightarrow C_9H_8O_4 + C_2H_4O_2[/tex]

Molar mass of Salicylic acid = 138.12 g/mol

Molar mass of aspirin = 180.16 g/mol

138.12 g Salicylic acid gives 180.16 g/mol

100 g Salicylic acid gives[tex]100\times\frac{180.16}{138.12} \\\\=130.44\ g[/tex]

The actual yield is 50 g.

[tex]\%=\frac{actual\ yield}{Theortical\ yield} \times100\\\\=\frac{50}{130.44} \times100\\\\=38.3\%[/tex]

So, the percentage yield for the reaction is 38.3%.

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