Boiling Points - Individual Report Template
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Boiling Points Individual Report Name: Grace Foster Do not modify or remove the question text. Do not use bold font in your answers. Do not use red-colored text. 1.
Report the three measured boiling points for the substance you measured, and their average and standard deviation. (
Note:
You can find the formula for the standard deviation in
Appendix A: Mistakes, Errors, Accuracy, and Precision
for standard deviation.)
Trial 1 Boiling point: 98.3
°࠵? (317.45 ࠵?)
Trial 2 Boiling point: 101.6
°࠵?(374.75࠵?)
Trial 3 Boiling point: 99.2
°࠵?(372.35࠵?)
Average Boiling Point: 372.85K SD: 38.965 2.
What is the commonly accepted boiling point for your substance (can be found through an online search)? Make sure to cite your source in your lab report.
Boiling point for Pentanone is 102
°࠵? (࠵?࠵?࠵?. ࠵?࠵?࠵?)
https://pubchem.ncbi.nlm.nih.gov/compound/2-Pentanone#section=Color-Form 3.
Compare your measurement to the known boiling point you looked up. Calculate the percent relative error of your measurement, and comment on both the accuracy and the precision of this measurement. Suggest how the accuracy of your measurement could have been improved. The most common method to improve the precision of a measurement is to increase the number of replications. Explain how the precision could be improved without having to make a large number of measurements. Our percent error was .61%. Our percent error was pretty good based off the fact that our average boiling point was only 2.3 degrees warmer than the known boiling point. The precision and the accuracy of the experiment were all close together all being within 4 degrees within each other. The precision could be improved by making sure that the substance was brought all the way back down to room temperature rather than just waiting for it to cool off 20-30 degrees like we did in the lab, also maybe taking the time to completely calibrate the tools used to measure the temperature in between trails could help rule out other environmental factors. Use the concepts developed in this experiment to explain the following observations
4.
The following four alcohols have the same molecular weight and molecular formula but differ in their boiling points: 1-butanol 2-methyl-1-propanol 2-butanol 2-methyl-2-propanol MW = 74 MW = 74 MW = 74 MW = 74 b.p. = 118 °C b.p. = 108 °C b.p. = 100 °C b.p. = 83 °C Boiling points are able to increase with the amount of surface tension that a molecule has because there are more molecules available for bondage. 5.
1-Butanol and diethyl ether are structural isomers of the formula C
4
H
10
O, but differ markedly in boiling point: 1-butanol, b.p. = 118 °C diethyl ether, b.p. = 35 °C 1-butanol has a much higher boiling point because it can have hydrogen bonds, hydrogen bonds required more heat to be able to break the bonds. Diethyl bonds are dipole-dipole which means they require less heat to break the bonds, resulting in a lower boiling point. H
3
C
CH
C
H
2
OH
CH
3
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(% C)
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