So, we did this experiment where we placed a graduated cylinder containing a small amount of air upside down into a beaker. We watched the bubble increase as temperature increased and vice versa.
When doing calculations, we used a low temperature along with the volume of air at that temperature to calculate nair, assuming that the vapor pressure of water was negligible at this temperature.
However, there was a question regarding vapor pressure: What would happen to the number of moles of air (observing volume) if the vapor pressure was not assumed negligible under 5oC, and the real vapor pressure was taken into affect?
I assumed that since vapor pressure is not assumed negligible, therefore increased, that the pressure of the water on the air within the graduated cylinder would cause the air volume to decrease, therefore "decreasing" the moles of air. However, apparently the vapor pressure taken into account increases moles of air.
How is this so?
Thanks in advance.