For this reaction, 0.1g of anthracene and 0.57g of maleic anhydride was used. During the second part of the experiment, the product was recrystallized. The total amount of crystals recovered was found to be 0.051g. From there the next step was to find the molarity of the reactants. The formula used to calculate the molarity was the weight of the sample divided by its molar mass. Given that the molar mass of anthracene is 178.2g, the moles of anthracene used was 0.00056M. Given that the molar mass of maleic anhydride was 98.1g, the moles of maleic anhydride used was …show more content…
The next thing that was found was the percent yield which is equal to the actual yield over the theoretical yield times 100. Since the theoretical yield was 0.00056M, the result was a 34% yield. The melting point was found to be 262.7 oC, which lies within the correct range theoretically. The results of the TLC plate testing also concluded that the product was pure. The spot from the product appeared half way up the card while the anthracene was at the top and the maleic anhydride was at the bottom. This single dot indicates a pure