the variation in gas pressure versus temperature is defined by the Gay-Lussac Law, which states that the pressure of a fixed mass of gas, held at constant volume, is directly proportional to its absolute temperature (i.e. in degrees Kelvin).
It doesn't matter what the gas is (air, nitrogen, helium, or whatever), provided it stays as a gas. If a tyre is inflated to 30psi at 20 degC (293degK), and the gas temperature is raised to 30degC (303degK), the pressure will rise to 30 x (303/293) = 31.03psi. In actual fact, the pressure at the higher temperature will be slightly below 31.03psi, because the tyre will have stretched ever so slightly as the pressure rises, so the contained volume will be slighly greater.
It doesn't matter what the gas is (air, nitrogen, helium, or whatever), provided it stays as a gas. If a tyre is inflated to 30psi at 20 degC (293degK), and the gas temperature is raised to 30degC (303degK), the pressure will rise to 30 x (303/293) = 31.03psi. In actual fact, the pressure at the higher temperature will be slightly below 31.03psi, because the tyre will have stretched ever so slightly as the pressure rises, so the contained volume will be slighly greater.