Evaporation and Intermolecular Attractions

Lets Begin!!!
Evaporation and Intermolecular Attractions
Yes that's ATTRACTION not Reaction! It's time to get down to the relationship status!

1st Come the Materials:

• Computer (DUH! OBVIOUSLY!)
• Serial Box Interface ULI
• Data Logger
• Two Probes
• 6 Pieces of Filter Paper
• 2 Small Rubber Bands
• Methanol ( Methyl Alcohol)
• Ethanol (Ethyl Alchohol)
• 1-Propanol
• 1-Butanol
• n-Hexane
• n-Pentane

Procedure, Procedure, Procedure! This Is What it Comes Down TO!:

1. Open "Experiment 9" from the Chemistry with Computers from the experiment files of Logger Pro.
2. Wrap filter paper around the tips of probes 1 and 2, and secure them with the rubber bands. By the way this was the hardest part!!!!
3. Place both probes into a container holding a sample of either methanol or ethanol.
4. After the probes have been in the liquids for around 30 seconds, begin data collection. Monitor the temperature for around 15 seconds to establish the initial temperature of each liquid.
5. Simultaneously remove the probes from the liquids and tape them with the tips of the probes extended of the edge of the counter.
6. When both temperatures have reached minimums, stop data collection, it kinda stops itself...
7. Find the maximum and minimum temperatures, then subtract them to find the change of temperature during evaporation.
8. Remove the rubber bands and discard the used filter paper.
9. Predict, using the data just collected, how the next set of substances will react!
10. Repeat these steps for the final substances as well!! :)

Data Analysis:

1.  Most of these substances contain hydrogens bonds which is very apparent for 1-Butanol and n-pentane. Their overall weights were very similar, however the temperature change between the two was vastlly different. Can you say hydrogen bonds were the cause! Definitely! 1-Butanol contains hydrogen bonds, but n-pentane does not. This made it easier for n-pentane to evaporate compared to 1-Butanol.
2. Methanol had the weakest intermolecular forces out of the six tested. However, 1-Butanol had the strongest. We can see that methanol had the weakest bonds because of the change of temperature. Methanol changed 17.38 degrees. This shows that it had weak bonds, allowing it to evaporate more quickly than the other liquids. 1-Butanol had the strongest bonds because its temperature had a low change rate. It's temperature only went down by about 2.41 degrees. This means that it had stronger intermolecular forces which didn't allow it to evaporate as much or as quickly as methanol. So basically the lower the change the better and the stronger intermolecular force the substance has!
3. Alkanes! n-Hexane had the weakest intermolecular forces, and n-pentane had the strongest molecular forces. n-Hexane changed a total of 10.00 degrees, and n-pentane only changed 7.28 degrees.

Green-Ethanol & Red-Methanol

Red- 1-Propanol & Green- 1-Butanol

Red- n-Pentane & Green- n-Hexane