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What effect does the temperature of nitrogen gas have on the pressure it exerts?
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Nitrogen approximately follows the ideal gas law which gives the relation between pressure and temperature as pV= nRT, where p is the absolute pressure of the gas; V is the volume of the gas; n is the amount of substance of the gas in moles; R is the gas constant (which is 8.314472 J*K^-1*mol^-1 in SI units); and T is the absolute temperature.
Therefore from pV= nRT, we get p = nRT / V. So as the temperature increases, for the volume and amount of the gas remaining constant, the pressure exerted increases and as the temperature decreases, the pressure exerted decreases.
Posted by william1941 on October 26, 2010 at 12:41 AM (Answer #1)
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