Propene, C3H6 (100 g) was subjected to combustion. The actual yield of carbon dioxide is 200 g. Calculate the percent yield of carbon dioxide.
2 C3H6 + 9 O2 → 6 H2O+ 6 CO2
(Molar mass: C=12 g/mol; H= 1g/mol; O =16 g/mol)
64.00%
45.45%
22.80%
22.75%
The balanced equation shows that 2 moles of propene produce 6 moles of carbon dioxide. Therefore, for 100 g of propene, the theoretical yield of carbon dioxide would be:
(100 g propene) / (42 g/mol propene) x (6 mol CO2 / 2 mol propene) x (44 g/mol CO2) = 378.1 g CO2
The percent yield can now be calculated by dividing the actual yield (200 g) by the theoretical yield (378.1 g) and multiplying by 100:
Percent yield = (200 g / 378.1 g) x 100% = 52.9%
Therefore, the correct answer is not provided as an option.
To calculate the percent yield of carbon dioxide, we need to compare the actual yield to the theoretical yield.
First, let's calculate the theoretical yield of carbon dioxide:
1. Calculate the molar mass of propene (C3H6):
Molar mass of C3H6 = (3 * molar mass of C) + (6 * molar mass of H)
= (3 * 12 g/mol) + (6 * 1 g/mol)
= 36 g/mol + 6 g/mol
= 42 g/mol
2. Calculate the moles of propene:
Moles of C3H6 = mass of propene / molar mass of C3H6
= 100 g / 42 g/mol
≈ 2.38 mol
3. Determine the limiting reactant:
From the balanced equation, we can see that 1 mole of C3H6 reacts with 3 moles of CO2. Therefore, the theoretical yield of CO2 is:
Moles of CO2 = 3 * moles of C3H6
= 3 * 2.38 mol
≈ 7.14 mol
4. Calculate the theoretical mass of carbon dioxide:
Mass of CO2 = moles of CO2 x molar mass of CO2
= 7.14 mol x (12 g/mol + 2 * 16 g/mol)
= 7.14 mol x 44 g/mol
≈ 314 g
Now, let's calculate the percent yield:
Percent yield = (actual yield / theoretical yield) * 100
= (200 g / 314 g) * 100
≈ 63.69%
Therefore, the percent yield of carbon dioxide is approximately 63.69%. None of the given options matches this result, so there may have been a calculation error.