How many grams of CO2 would be produced? - Show Work Please

Question

Question: For the balanced equation shown below, if the reaction of 91.3 grams of C3H6 produces a 81.3% yield, how many grams of CO2 would be produced?

 

Equation: 2C3H6 + 9O2 = 6CO2 + 6H2O

Answer 1

2C3H6 + 9O2 = 6CO2 + 6H2O  Balanced equation

moles C3H6 present = 91.3 g x 1 mole/42.1 g = 2.17 moles 

Theoretical yield of CO2 = 2.17 moles C3H6 x 6 moles CO2/2 moles C3H6 = 6.51 moles CO2

If 81.3% is produced, that will be 0.813 x 6.51 moles = 5.29 moles CO2

mass CO2 = 5.29 moles x 44 g/mole = 232.9 g = 233 g of CO2