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Using the ideal gas law (PV=nRT), you can calculate what would happen by just raising the temperature. Note that the T is in degrees Kelvin, so you would have to convert from C. V is the volume, n is the number of molecules and R is the gas constant, so those values would not change in your scenaro. From that, you can use: P2 = P1 * (T2 / T1): P2 = 2 * (313/288) P2 = 2.17 bar Note that this won't be exactly what occurs, but it gives you a close approximation. ("Impurities" in air will cause variations in the pressure rise. Moisture probably has the biggest effect, and it will typically increase the pressure rise. This is one of the reasons why nitrogen is being touted as "better than air" for your car tires.) Also, please note that the air pressure recommendations are for *cold* tires (i.e., at outside air temperature), so don't adjust for what you think the tire temperature may go up to.

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