The reaction of 5.25 g of Carbon with excess O2 yields 10.2 g of CO2. What is the percent yield of this reaction?
find moles of C and moles CO2 ... should be the same in a complete reaction
percent yield = (moles CO2 / moles C) * 100%
To calculate the percent yield of a reaction, you need to use the following formula:
Percent Yield = (Actual Yield / Theoretical Yield) × 100
In this case, the actual yield is given as 10.2 g of CO2. However, we need to determine the theoretical yield first, which represents the maximum possible amount of CO2 that could be produced under ideal conditions.
To find the theoretical yield, we need to calculate the amount of CO2 produced from 5.25 g of carbon. The molar mass of carbon (C) is 12.01 g/mol, and the molar mass of carbon dioxide (CO2) is 44.01 g/mol.
1. Convert the mass of carbon to moles:
Number of Moles of Carbon = Mass of Carbon / Molar Mass of Carbon
Number of Moles of Carbon = 5.25 g / 12.01 g/mol
2. Use the stoichiometry of the balanced chemical equation to find the number of moles of CO2 produced:
From the balanced equation C + O2 -> CO2, we see that one mole of carbon produces one mole of CO2.
Number of Moles of CO2 = Number of Moles of Carbon
3. Convert the moles of CO2 to grams:
Mass of CO2 = Number of Moles of CO2 × Molar Mass of CO2
Mass of CO2 = Number of Moles of CO2 × 44.01 g/mol
After calculating the theoretical yield using the steps above, you can substitute the values into the percent yield formula to find the answer:
Percent Yield = (Actual Yield / Theoretical Yield) × 100
Percent Yield = (10.2 g / Theoretical Yield) × 100
C + O₂ => CO₂
(5.25-gC/12g/mol) = 0.4375 mole C => 0.4375 mole CO₂ x 44 g/mole = 19.25 g (Theoretical Yield)
%Yield = [Actual Yield / Theoretical Yield] x 100% = (10.2-g/19.25-g) x 100% ≈ 53% Yield