Question

Suppose 5.5 g of Compound A are consumed in a reaction with 3.5 g of Compound B that produces only one product,
Compound C.
Suppose 8.4 g of C are actually isolated at the end of the reaction.
What is the percent yield of Compound C?
Round your answer to the nearest whole percent.

Answer 1

The theoretical yield of Compound C can be calculated based on the stoichiometry of the reaction and the amount of Compound A and Compound B consumed.

First, we need to determine the limiting reactant by calculating the moles of Compound A and Compound B:
- Moles of Compound A: 5.5 g / molar mass of A
- Moles of Compound B: 3.5 g / molar mass of B

Next, we need to determine the theoretical yield of Compound C using the stoichiometry of the reaction:
- The balanced equation will tell you the mole ratio between Compound A, Compound B, and Compound C
- Use the moles of the limiting reactant to calculate the moles of Compound C
- Convert moles of Compound C to grams

Now, to calculate the percent yield:
- Percent yield = (actual yield / theoretical yield) x 100
- Substitute the actual yield and theoretical yield values to find the percent yield

After these calculations, you can round the percent yield to the nearest whole percent.