A student was tasked with synthesizing a Diels alder adduct of maleic anhydride and a diene. The student started with 6.0 g sample of a crude oil that was determined to contain 65 % by weight of diene. [MW of diene 136g/mol]
The amount of maleic anhydride used was intended to completely react with the diene in the crude oil sample.
If the final weight of product (adduct) after synthesis and purification was determined to be 3.0 grams, calculate the student’s overall reaction yield.
To calculate the student's overall reaction yield, we need to determine the theoretical yield and the actual yield.
1. Theoretical Yield:
The theoretical yield is the maximum amount of product that can be obtained assuming complete reaction. In this case, the maleic anhydride should completely react with the diene in the crude oil sample.
First, we need to calculate the amount of diene in the crude oil sample:
Amount of diene = 65% of the 6.0 g sample = 0.65 * 6.0 g = 3.9 g
Next, we need to convert the amount of diene to moles:
Number of moles of diene = Amount of diene / Molecular weight of diene
Number of moles of diene = 3.9 g / 136 g/mol = 0.028676 mol
Since the maleic anhydride is intended to completely react with the diene, the theoretical yield of the adduct will be equal to the number of moles of diene used.
Theoretical yield = Number of moles of diene = 0.028676 mol
2. Actual Yield:
The actual yield is the yield obtained from the synthesis and purification process. In this case, the final weight of the purified adduct is given as 3.0 grams.
Actual Yield = 3.0 g
3. Overall Reaction Yield:
To calculate the overall reaction yield, we can use the following formula:
Overall reaction yield = (Actual yield / Theoretical yield) * 100
Plugging the values:
Overall reaction yield = (3.0 g / 0.028676 mol) * 100 = 10447.3%
Therefore, the student's overall reaction yield is approximately 10447.3%.