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Unformatted text preview: 1.3 % Discussion:
Overall, the product obtained from the Diels-Alder reaction was somewhat pure. Based
on looks, the crystals were mostly white with some brown discoloration due to the heating of the
solution with the boiling stones. The discoloration of the crystals indicates impurity. The
measured melting point of the crystals also indicates impurities were present. The first melting point measured was 92.7-94.2 oC, and the second was 93.2-94.3 oC. The fact that the measured
melting point is quite a bit less than the literature melting point of 103-104 oC indicates impurity.
If the crystals were more pure, the melting point would’ve been closer to lit value. The mass of
my following product was 0.046 grams. Based on percent yield, the product’s yield is about
average. As compared to ten classmates who have yields of 0.027 g, 0.002 g, 0.037g, 0.021 g,
0.057 g, 0.027 g, 0.027 g, 0.02 g, 0.06 g, and 0.057 g. The average yield among ten classmates
was 0.0335 grams. As compared to my classmates, I had a relatively above average product yield
with 0.046 grams. The percent yield of my product was 31.3% as compared to ten classmates
who had 17.58%, 1.9%, 34%, 16%, 38.26%, 18%, 19.59%, 14.2%, 47.2%, and 39.1%. The
average of my ten classmate’s percent yield was 24.6%, making my percent yield slightly above
average. Overall, the yields of my experiment were good, for they were slightly above average
when compared to ten other classmate’s data.
There were multiple places for error to occur throughout the experiment. The first loss of
product occurred when transferring the crystalline powders of maleic anhydride and butadiene
sulfone from their tarred aluminum trays into the conical vial. Some of the solid powder stuck to
the aluminum tray, making the amount measured more than what was actually put in. A second
place where product loss could’ve occurred is when the conical vial was set on ice and allowed
to recrystallize. Because the vial only sat on ice for 10 minutes,...
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