Originally Posted by
Rincewind8
The ideal gas law is:
pressure*Volume = mu(number of moles of gas)*R(Universal gas constant) *Temperature(in Kelvin)
Assuming the volume stays constant, p/T has to stay constant. So filling the tires at ~266ºK (20ºF) to a pressure of 102psi and then heating the air in the tires to room temperature of maybe 297ºK (75ºF) results in a pressure of 102psi*297/266=114psi.
Since there is always a safety margin, the tires should hold that pressure.
How big is that safety margin?
The way I'm reading it, the tires are only rated for less than 85 psi, so he's already over-inflating them. It seems like the extra 12 psi could blow them off.