With respect to the given assertion and reason, Choose the correct option. Assertion [A]: With an increase in the temperature of a gas inside a container, its pressure also increases. Reason [R]: Upon heating, the kinetic energy of the gas particles increases, which in turn results in a greater force exerted on the walls of the container.
According to Charles's law, the volume of a gas is directly proportional to the number of molecules at constant temperature and pressure.
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