Determine the percent yield for the following generic reaction using the information given below: Compound A --> Compound B if you start with 10.0 mL of Compound A and obtain 9.0 g of Compound B. Density of Compound A = 0.75 g/mL MW of Compound A = 150. g/mol MW Compound B = 300. g/mol [x1] % yield
1 mol A ==> 1 mol B
grams A = determined from density.
mass = volume x density = 10 mL x 0.75 g/mL = 7.5 g.
mols A = grams/molar mass = ?
Since the reaction is 1 mol A to 1 mol B, then mols B = mols A
Grams B = mols B x molar mass B = ?g theoretical yield (TY). The actual yield (AY) is 9.00 g.
%yield = (AY/TY)*100 = ?
To determine the percent yield, you need to compare the amount of Compound B obtained (the actual yield) with the maximum possible yield of Compound B (the theoretical yield). The percent yield is calculated using the formula:
Percent yield = (actual yield / theoretical yield) x 100
Now, let's calculate the theoretical yield:
1. Begin by determining the number of moles of Compound A using the volume and density provided:
moles of Compound A = (volume of Compound A) x (density of Compound A)
moles of Compound A = (10.0 mL) x (0.75 g/mL) = 7.5 g
2. Next, calculate the theoretical yield of Compound B by converting the moles of Compound A to moles of Compound B, using their respective molecular weights:
moles of Compound B = (moles of Compound A) x (MW of Compound B / MW of Compound A)
moles of Compound B = 7.5 g x (300 g/mol / 150 g/mol) = 15.0 g
3. Finally, calculate the percent yield using the formula mentioned earlier:
Percent yield = (actual yield / theoretical yield) x 100
Percent yield = (9.0 g / 15.0 g) x 100 = 60%
Therefore, in this reaction, the percent yield is 60%.