helium gas, He (g), then R = 8.314 J K -1 mol -1.nitrogen gas, N 2(g), then R = 8.314 J K -1 mol -1.carbon dioxide gas, CO 2(g), then R = 8.314 J K -1 mol -1.If the experiment described above is done using: The gas constant R is very special because its value does not depend on the nature of the gas used. The pressure exerted by the gas in this volume is actually a measure of the energy of the gas particles, so the units of this Gas Constant, R, are most often expressed as Joules per Kelvin per mole, J K -1 mol -1. If we measure pressure in kilopascals (kPa), volume in litres (L), temperature in Kelvin (K) and the amount of gas in moles (mol), then we find that R = 8.314 and it has the units kPa L K -1 mol -1. Boyle's Law tells us that the volume of the gas (V) is inversely proportional to its pressure (P):.No ads = no money for us = no free stuff for you! Deriving the Ideal Gas Equation A gas which deviates from Ideal Gas behaviour is called a non-ideal gas.Under ordinary conditions, deviations from Ideal Gas behaviour are so slight that they can be neglected.at high pressures the gas molecules are forced closer together so that the volume of the gas molecules becomes significant compared to the volume the gas occupies.at low temperatures the gas molecules have less kinetic energy (move around less) so they do attract each other.Real Gases deviate from Ideal Gas Behaviour because:.
Pressure is due to the gas molecules colliding with the walls of the container.The volume of the molecules present is negligible compared to the total volume occupied by the gas.Gases consist of small particles (molecules) which are in continuous random motion.An Ideal Gas is modelled on the Kinetic Theory of Gases which has 4 basic postulates:.
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