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.
Solve
To find the percent yield of Compound C, we first need to calculate the theoretical yield of Compound C based on the amount of Compound A and Compound B used in the reaction.
1. Calculate the molar mass of Compound A and Compound B:
Compound A: 5.5 g
Compound B: 3.5 g
Molar mass of Compound A = ?
Molar mass of Compound B = ?
2. Convert the masses of Compound A and Compound B to moles:
moles of Compound A = 5.5 g / molar mass of Compound A
moles of Compound B = 3.5 g / molar mass of Compound B
3. Determine the limiting reactant. This will be the reactant that produces the least amount of Compound C.
4. Determine the theoretical yield of Compound C based on the limiting reactant.
5. Calculate the percent yield of Compound C using the formula:
Percent yield = (actual yield / theoretical yield) * 100
Plug in the values and calculate the percent yield.