Final answer:
The percent yield of the Diels-Alder product can be calculated by dividing the actual yield by the theoretical yield and multiplying by 100. The actual yield is given as 1.9387 grams of product. In order to find the theoretical yield, we need to determine the limiting reactant and calculate the moles of each reactant using their masses and molar masses.
Step-by-step explanation:
The percent yield of a reaction can be calculated by dividing the actual yield of the product by the theoretical yield, and then multiplying by 100. In this case, the actual yield is given as 1.9387 grams of product. To find the theoretical yield, we need to determine the limiting reactant, which is the reactant that is completely consumed in the reaction. To do this, we compare the moles of maleic anhydride and 3-sulfolene and see which one produces a smaller amount of product. From the balanced chemical equation, we can see that one mole of maleic anhydride reacts with one mole of 3-sulfolene to produce one mole of the Diels-Alder product. Since the ratios are 1:1, we can compare the masses directly. The molar mass of maleic anhydride is 98.06 g/mol and the molar mass of 3-sulfolene is 114.18 g/mol. Therefore, the theoretical yield can be calculated as follows:
1.5034 g maleic anhydride * (1 mol/98.06 g) * (1 mol Diels-Alder/1 mol maleic anhydride) = 0.01534 mol
2.4876 g 3-sulfolene * (1 mol/114.18 g) * (1 mol Diels-Alder/1 mol 3-sulfolene) = 0.02178 mol
The smaller value is 0.01534 mol, which indicates that maleic anhydride is the limiting reactant. Therefore, the theoretical yield is 0.01534 mol of Diels-Alder product. To convert this to grams, we can use the molar mass of the Diels-Alder product, which is 158.15 g/mol:
0.01534 mol * (158.15 g/1 mol) = 2.4278 g
Finally, we can calculate the percent yield:
(1.9387 g/2.4278 g) * 100 = 79.9%