If a very small hole were poked in the tire, a tire filled with pure N2 would lose pressure less quickly than a tire filled with atmospheric air is NOT a potential advantage to inflating car tires with N2 instead of atmospheric air (79% N2, 20% O2, and 1% other gases including H2O, Ar, and CO2).
If a very small hole is poked in a tire, the gas would leak out in a process approximating effusion. The rate of effusion is inversely proportional to molecular weight according to Graham's law:
Since air contains both N2 (MW = 28 g/mol) and O2 (MW = 32 g/mol), oxygen will effuse more slowly. The choice, "tires filled with N2 weigh less than those filled with atmospheric air, leading to better fuel efficiency" is an advantage, since atmospheric air is more dense than pure N2 due to the presence of the heavier O2. It is true that water experiences stronger intermolecular forces than N2, therefore atmospheric air is more likely than N2 to condense as the pressure inside the tire increases. Finally, it is also true that corrosion occurs due to oxidation caused by molecular O2 present only in atmospheric air.
Two gases, each 1 L at STP, are allowed to spontaneously react in an insulated cylinder with a floating piston to form two new gaseous products such that total moles are constant before and after the reaction. Immediately after the completion of the reaction the volume of the cylinder was measured to be 1.82 L, therefore the reaction was endothermic.
If the reaction created the same number of moles of gas as it consumed, and the reaction remained at STP, the volume of the cylinder should have been 2 L. Since the eventual volume is less with the pressure equilibrated to atmospheric, the temperature of the reaction must have decreased, as would have been the case if the reaction was endothermic and consumed heat from the system in order to do chemical work. Had the reaction been exothermic, and the reaction given heat to the system, the end volume would have been greater than 2 L. If the reaction were isothermal, at STP, there would have been no change in volume. Finally, ΔS for the reaction could not have been negative, since the number of moles of gas did not change over the course of the reaction.