What happens to the kinetic energy of particles of a gas when it comppressed in a cylinder.
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The kinetic energy can be written as
E= 1/2mv^2 where v= RMS VELOCITY of a gas particle so in ideal condition
PV=RT for 1 mole of gas ..and hence the RMS VELOCITY can be substituted as 3PV/M under root and hence when the pressure increases the volume decreases thus the whole function remains constant and hence the RMS VELOCITY Remains constant so the kinetic energy ..well if you increase pressure the mean free path decreases which allows gas molecule to collide at a faster rate but with the same energy...it just increases the frequency of collision with respect to the time
E= 1/2mv^2 where v= RMS VELOCITY of a gas particle so in ideal condition
PV=RT for 1 mole of gas ..and hence the RMS VELOCITY can be substituted as 3PV/M under root and hence when the pressure increases the volume decreases thus the whole function remains constant and hence the RMS VELOCITY Remains constant so the kinetic energy ..well if you increase pressure the mean free path decreases which allows gas molecule to collide at a faster rate but with the same energy...it just increases the frequency of collision with respect to the time
ssss10:
thanks
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It's interparticle is negligible
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