We performed an experiment in chemistry where tissue paper soaked in various chemicals was wrapped around the end of a temperature probe.
The chemicals with stronger intermolecular forces had a lower drop in temperature (from room temperature to final, after most of the alcohol had evaporated off). For reference, two of the chemicals were ethanol with hydrogen bonding and n-pentane with only London dispersion forces.
My question is why.
Below are just my initial attempts to understand
My initial feeling was that the molecules with stronger intermolecular forces would take more energy to evaporate and would have a larger temperature change than those chemicals with weaker bonds, but we see the opposite in the data.
I was also thinking that maybe that went the other way: The chemicals with stronger forces had fewer molecules evaporate off, so the temperature drop was smaller. Is this more correct?