Question

What is the percent yield when 28.16 g of CO₂ are formed from the reaction of 4.000 moles of C8H18 with 4.000 moles of O₂?

1) 25.00
2) 50.00
3) 75.00
4) 100.00

Answer 1

The percent yield in this reaction is 8.0%

Step-by-step explanation:

The percent yield is a measure of the efficiency of a chemical reaction and is calculated by dividing the actual yield by the theoretical yield and multiplying by 100. The theoretical yield is the amount of product that would be obtained if the reaction went to completion based on the stoichiometry of the balanced equation. In this case, the balanced equation is:

2 C8H18 + 25 O2 → 16 CO2 + 18 H2O

From the balanced equation, we can see that 2 moles of C8H18 react to produce 16 moles of CO2. So if 4.000 moles of C8H18 react, the theoretical yield of CO2 would be:

(4.000 moles C8H18) * (16 moles CO2 / 2 moles C8H18) * (44.01 g CO2 / 1 mole CO2) = 352.16 g CO2

The actual yield is given as 28.16 g CO2. Therefore, the percent yield is:

(28.16 g CO2 / 352.16 g CO2) * 100 = 8.0%