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A tire contains air at a pressure of 2 bar 15 degrees C If the tire's pressure is unchanged what will the air pressure in it be when the tire warms up to 40 degrees C as the car is driven?
Wiki User
∙ 15y ago
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.
Wiki User
∙ 15y ago
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