In this video, a pool of liquid nitrogen in a metal bowl can cool it enough so that oxygen from the air condenses at the bottom:
Thermodynamically, it seems that the bowl can't get cold enough. The bowl can't cool off below the temperature at which the nitrogen pressure in the air (80kPa, I got all the vapor pressure information form Air Liquide) equals the vapor pressure of the liquid nitrogen; at that point the rate of evaporation equals the rate of condensation from the pool. This happens at ~76K. This is also the threshold where oxygen can condense (vapor pressure of 20kPa). However, 76K is a lower bound. The actual temperature will be higher when you include condensation of water into/onto the bowl, convective/radiative heat transfer, and the fact that there is additional nitrogen/oxygen above the surface of the pool beyond the 80kPa used in the calculations. In the face of these calculations, why does it seem to work?
My reasoning is that it still gets cold enough for a mixture of nitrogen and oxygen to condense which has enough oxygen to burn the tissue paper, is this correct?