How do I find the Actual Yield and the Percent Yield if I have the mass of salicylic acid as 1.46 g, volume of acetic anhydride as 3 mL, mass of acetic anhydride as 3.24 g, and theoretical yield of aspirin as 1.90 g/mol?
write the balanced equation
Find how many moles you use on input
The equation will tell you how many moles to expect on output
divide what you got by what you expected for % yield
Let me point out a number of problems with this post.
1. A theoretical yield of 1.90 g/mol makes no sense. You must have meant 1.90 grams.
2. The only way you get an actual yield is if the problem tells you or if you do the actual experiment. Frankly, I suspect the 1.90 above is the actual yield and you are to calculate theoretical yield from oobleck's post. From that you can calculate % yield.
To find the actual yield and the percent yield, you'll need to follow these steps:
Step 1: Calculate the moles of salicylic acid (C7H6O3):
To do this, you need to calculate the number of moles of salicylic acid using its molar mass. The molar mass of salicylic acid is 138.12 g/mol (12.01 g/mol for carbon + 1.01 g/mol for hydrogen + 16.00 g/mol for oxygen).
Number of moles of salicylic acid (C7H6O3) = mass of salicylic acid (1.46 g) / molar mass of salicylic acid (138.12 g/mol).
Step 2: Convert the volume of acetic anhydride (C4H6O3) to moles:
Since you know the volume of acetic anhydride, you need to convert it to moles using its molar volume. The molar volume of a liquid is typically given in mL/mol, so you need to know the molar mass of acetic anhydride to convert the volume to moles.
Number of moles of acetic anhydride = volume of acetic anhydride (3 mL) * (1 L/1000 mL) * (1 mol/molar volume of acetic anhydride).
Step 3: Determine the limiting reactant:
Compare the moles of salicylic acid and acetic anhydride to determine the limiting reactant. The limiting reactant is the one that is completely consumed in the reaction and determines the maximum amount of product that can be formed.
Step 4: Calculate the theoretical yield of aspirin:
The theoretical yield is the maximum amount of product that can be obtained from the limiting reactant. In this case, aspirin is the product, and its molar mass is given as 1.90 g/mol.
Theoretical yield of aspirin = limiting reactant (moles) * molar mass of aspirin.
Step 5: Calculate the actual yield:
The actual yield is the amount of product obtained in a real-world experiment.
Actual yield = mass of aspirin (if given).
Step 6: Calculate the percent yield:
The percent yield is a ratio of the actual yield to the theoretical yield, expressed as a percentage.
Percent yield = (actual yield / theoretical yield) * 100.
By following these steps and plugging in the given values, you can calculate the actual yield and the percent yield.