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
Same process + a little more from the NaN3 problem above.
Find mols aspirin produced by 100 g salicylic acid, convert to grams aspirin, and that is the theoretical yield. Then % yield = (actual yield/theoretical yield)*100 = ?
To find the percentage yield for a chemical reaction, you need to compare the actual yield (the amount of product obtained in the experiment) to the theoretical yield (the amount of product that can be calculated from the balanced equation and stoichiometry).
First, let's calculate the theoretical yield of aspirin (C9H8O4) based on the reaction equation:
- We have 100 g of salicylic acid (C7H6O3).
- The molar mass of salicylic acid (C7H6O3) is 138.12 g/mol.
- We can calculate the number of moles of salicylic acid by dividing the mass by the molar mass, so 100 g / 138.12 g/mol = 0.723 mol.
- Referring to the balanced equation, we see that 1 mole of salicylic acid gives 1 mole of aspirin, so we expect a theoretical yield of 0.723 mol of aspirin (C9H8O4).
Next, we need to convert the theoretical yield from moles to grams:
- The molar mass of aspirin (C9H8O4) is 180.16 g/mol.
- Multiplying the number of moles (0.723 mol) by the molar mass (180.16 g/mol) gives the theoretical yield: 0.723 mol * 180.16 g/mol = 130.43 g.
Now, let's calculate the percentage yield:
- The actual yield is given as 50.0 g of aspirin (C9H8O4).
- To calculate the percentage yield, divide the actual yield by the theoretical yield and multiply by 100: (50.0 g / 130.43 g) * 100 = 38.33%.
Therefore, the percentage yield for the reaction is 38.33%.