According to kinetic theory of gases , the root mean square velocity is directly proportional to:

Q. According to the kinetic theory of gases, the r.m.s velocity of gas molecules is directly proportional to :

Q.

According to pressure equation, PV=1/3 M Vrms².

=>nRT=1/3 M Vrms²

=> T directly proportional to M Vrms²

According to mean Kinetic energy,

KE(avg)=1/2 M Vrms²

=> KE(avg) directly proportional to M Vrms²

This means.. M Vrms² directly proportional to KE(avg) T

=> M Vrms² /T = KE(avg) × proportionality constant

So this means the avg Kinetic energy is inversely proportional to Absolute Temperature. But actually KE(avg) is directly proportional to T. Please clear my doubt

Q. According to the Kinetic Molecular Theory, temperature is directly proportional to:

Q. Use kinetic theory of gases to show that the average Kinetic energy of a molecule of an ideal gas is directly proportional to the absolute temperature of the gas.

Q. Assertion :$H_2$ and $O_2$ have same $RMS$ velocity at the same temperature. Reason: $RMS$ velocity of a gas molecule is directly proportional to the square root of $T$.