If you started with exactly 1.885 g of salicylic acid and 3.50 mL of acetic anhy

Question

If you started with exactly 1.885 g of salicylic acid and 3.50 mL of acetic anhydride, calculate the theoretical yield of asprin. The density of acetic anhydride is 1.08 g/mL (Hint: determine the limiting reactant). If a team obtains 1.85 g of asprin product form, what was the percent yield?
**PLEASE show work. Detailed explanation is very appreciated. Thank you!!!**

4- If you staned wth exacth 1.sns g af salatk acid and 3so mu ot at tut arhyond., (Hint: determine the limiting reactanty H a team obtains 1.ES of aspirin produt from, Percent yield?

Explanation / Answer

Answer

Molecular weight of salicylic acid = 138.121 g/mol

Weight of Saliyclic acid = 1.885 g

Number of moles = weight/ molecular weight= 1.885/138.12 = 0.0136 moles

Volume of acetic anhydride = 3.50 mL

Density of acetic anhydride = 1.08 g/ml

We have Density = Mass/ Volume

Therefore

Mass = Density x Volume = 1.08 x 3.05 = 3.294 g

Molecular weight of acetic anhydride = 102.09 g/mol

Number of moles = weight/ molar mass= = 3.294 g/ 102.09 g/mol = 0.0320 moles

Here salicylic acid used has less number of moles , so it is the limiting reactant

Yield= number of moles of limiting reactant x product molecular weight

Here the product is acetyl salicylic acid ( aspirin)

Aspirin molecular weight =180.157 g/mol

So the

Yield = 0.0136 x 180.157 = 2.45 g which is 100 % yield ( theorectical yield)

If the team get 1.85 g, the yield = ?

We have

2.45 = 100 %

1.85 = ?

? = (1.85 x 100)/ 2.45 = 60.65%  

So the yield got is 60.65%

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