What is the percent yield of CO2 if 80g of Fe2(CO3)3 is decomposed to yield Fe2O3 + 22g of CO2
80 g Fe2(CO3)2 x (2*molar mass CO2/molar mass Fe2(CO3)2) = about 30 g which is the theoretical yield of CO2. You should calculate a more exact answer.
Then %yield = (22/30)*100 = ?
56.1%
To calculate the percent yield of CO2, you need to compare the actual yield of CO2 (which is given as 22g) with the theoretical yield of CO2 (which can be calculated based on the balanced chemical equation and the starting amount of Fe2(CO3)3).
First, you need to determine the molar mass of Fe2(CO3)3:
Molar mass of Fe = 55.8 g/mol
Molar mass of C = 12.0 g/mol
Molar mass of O = 16.0 g/mol
Molar mass of CO3 = 12.0 g/mol (C) + (16.0 g/mol x 3) (O) = 60.0 g/mol
Molar mass of Fe2(CO3)3 = (55.8 g/mol x 2) (Fe) + (60.0 g/mol) (CO3) = 291.6 g/mol
Next, calculate the moles of Fe2(CO3)3:
moles of Fe2(CO3)3 = 80g / 291.6 g/mol = 0.274 moles
According to the balanced chemical equation:
Fe2(CO3)3(s) -> Fe2O3(s) + 3CO2(g)
From the equation, we see that the mole ratio between Fe2(CO3)3 and CO2 is 1:3. Therefore, the theoretical yield of CO2 can be calculated using the mole ratio:
moles of CO2 = 0.274 moles (Fe2(CO3)3) x (3 moles CO2 / 1 mole Fe2(CO3)3) = 0.822 moles
Now, calculate the theoretical mass of CO2:
mass of CO2 = moles of CO2 x molar mass of CO2 = 0.822 moles x 44.0 g/mol = 36.17 g
Finally, calculate the percent yield of CO2:
percent yield = (actual yield / theoretical yield) x 100
percent yield = (22g / 36.17g) x 100 = 60.87%
Therefore, the percent yield of CO2 in this reaction is approximately 60.87%.