If, in the reaction below, 31 g of C4H10 produces 41 41 g of CO2, what is the percent yield? Assume that the one reactant is limiting. 2C4H10 + 13O2 + 10H2O
Did you make a typo? Is that 41 g, 41.41, or some other number? I know you made a typo in the reaction.
#1. There is no arrow.
#2. There is no CO2 shown.
Balance the equation.
2C4H10 + 13O2 ==> 8CO2 + 10H2O.
mols C4H10 = grams/molar mass.
Using the coefficients in the balanced equation, convert mols C4H10 to mols CO2.
Convert mols CO2 to g. grams = mols x molar mass. This is the theoretical yield.
%yield (actual grams CO2/theoretical yield)*100 =
To find the percent yield, we need to compare the actual yield (the given amount of CO2 produced) with the theoretical yield (the amount of CO2 that would be produced if the reaction went to completion).
First, we need to find the molar mass of C4H10 (butane) and CO2 (carbon dioxide):
- The molar mass of C4H10 is calculated as follows:
C: (4 atoms x 12.01 g/mol) = 48.04 g/mol
H: (10 atoms x 1.01 g/mol) = 10.10 g/mol
Total molar mass of C4H10 = 48.04 g/mol + 10.10 g/mol = 58.14 g/mol
- The molar mass of CO2 is calculated as follows:
C: (1 atom x 12.01 g/mol) = 12.01 g/mol
O: (2 atoms x 16.00 g/mol) = 32.00 g/mol
Total molar mass of CO2 = 12.01 g/mol + 32.00 g/mol = 44.01 g/mol
Next, we convert the given amounts of reactants and products from grams to moles:
- Mass of C4H10 = 31 g
Moles of C4H10 = 31 g / 58.14 g/mol = 0.533 mol (rounded to three decimal places)
- Mass of CO2 = 41 g
Moles of CO2 = 41 g / 44.01 g/mol = 0.932 mol (rounded to three decimal places)
Now, we determine the stoichiometric ratio between C4H10 and CO2 from the balanced equation. From the equation, we see that the ratio is 2:1. This means that for every 2 moles of C4H10, 1 mole of CO2 is produced.
Since C4H10 is the limiting reactant, the theoretical yield will be based on the moles of C4H10.
The theoretical yield of CO2 can be calculated as follows:
Moles of CO2 (theoretical) = Moles of C4H10 x (1 mole CO2 / 2 moles C4H10) = 0.533 mol x (1/2) = 0.266 mol (rounded to three decimal places)
To find the percent yield, divide the actual yield by the theoretical yield and multiply by 100:
Percent yield = (Actual yield / Theoretical yield) x 100
= (0.932 mol / 0.266 mol) x 100
= 350.37% (rounded to two decimal places)
Thus, the percent yield is approximately 350.37%.