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09 /18/ 25, 1:15amLogin ] [ Contact Forum Admin ] [ Main index ] [ Post a new message ] [ Search | Check update time | Archives: 1234567[8]910 ]
Subject: Re: Tires


Author:
HRSkillern
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Date Posted: 04/ 3/ 03, 5:17am
In reply to: John Marquette 's message, "Tires" on 03/ 31/ 03, 12:00pm

Air is a "gas". Appying the "Ideal Gas Law" from your High School chemistry class, P = CrT

P = pressure exerted by the gas

C = constant

r = density of the gas = mass/volume

T = Temperature of the gas
you will arrive at the solution.
HRS

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[> [> Subject: Re: Tires


Author:
djnichols
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Date Posted: 04/ 3/ 03, 8:51am

Might be important to note that the temperature is measured in degrees Kelvin. To visualize the effects of the above formula, consider this:

Imagine the relatively small change from 32 degrees F (0 degrees C, 273 degrees K) to 68 degrees F (20 degrees C, 293 degrees K). That is a 7.3% change in temperature, which will get you a 7.3% change in pressure (100 psi to about 107 psi).

The previous statement of the Ideal Gas Law assumes that the volume is held constant. Not exactly true for tires but probably close enough.

-dennis

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