1. We got a mac and plugged the temperature probe into the mac so we could record the data.
2. We got the probes and wrapped a piece of filter paper over it and wrapped a rubber band around it to keep it to stay there.
3. Then we next put the 2 probes in different solutions such as methanol and ethanol for about 15 seconds then put them out over the countertop and it evaporated up the solution as the rest of the program finished running.
4. We next did the same thing, but put the probes in 2 different substances which were Propanol and Butanol. We repeated the steps with taping them to the edge of the countertop and let the program finish running. The last two ones that we did were pentane and hexane. We did the same thing but it was weird in the hexane, it dissolves rubber, so while the probe was soaking up in the hexane solution for a while, the rubber band started to dissolve.
Data Analysis:
1. Most of these substances contain hydrogen bonds which is very apparent for 1- Butanol and n-pentane. Their weights all together were pretty much the same, but the temperature change was very different. Hydrogen bonds were definitely the cause because 1- Butanol has hydrogen bonds, but n-pentane doesn't. That is why n-pentane evaporated the best.
2. Methanol had the weakest intermolecular forces out of all the ones that we tested. Where 1-Butanol was the strongest. Methanol had the weakest bonds because it's temperature change. Methanol changed 17.38 degrees, which is why it evaporated faster than all of the other solutions. 1- Butanol had a very low change rate, and that is why the bonds were so strong. So pretty much the lower the change in temperature, the stronger force it has.
3. Alkanes. n-hehane had the weakest intermolecular forces, and n-pentane had the strongest molecular forces. N-hexane changed 10.00 degrees, and n-pentane only changed 7.28 degrees.
Green- Ethanol, Red- Methanol
Red- 1-propanol, Green-1-Butaol
Red- n-pentane, Green- n-hexane
