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chemistry
Theoretical yield: 1.99g (1 mole/138.12g) x (180.16g/mL)=2.59 g (smaller)
4.644g x (1 mole/102.08g) x (180.16g/1 mole)=8.196g
% Yield: 2.66g/2.50g x 100= 102.7%
Purity: Very pure. Intense violet.
Mass of salicylic acid used: 2.25g
Volume of acetic anhydride used: 4.8mL
Mass of acetic anhydride used: 5.184g
Density: 1.08g/mL
Mass of aspirin obtained: 2.87g
Discussion: After the experiment was completed it seems that the closer the actual yield was close to the theoretical yield. Seeing as how the percentage yield in this case was so high there was very little room for air. But it is possible for things to still go wrong in the experiment. The results of the experiment could have many different sources of error. Possible errors include that the glassware was not sanitary, mass salicylic acid not measured correctly, or the the volume of the acetic anhydride wasn’t measured correctly.
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Wow! i have absoloutly no idea....=(
sorry -&hearts-
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You should ask MFS this question, he's a chemist!
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