From the relation `p=1/3 mnc_(rms)^2` show that the mean kinetic energy of a molecule is the same for all types of gases.

Find out the molecular kinetic energy of 1 mol of an ideal gas . Is it equal for all gases?

At a constant temperature, a vessel of 1 litre capacity contains 10^(23)N_(2) molecules. If the rms velocity of the molecules be 10^(3)m//s , then determine the total kinetic energy of the molecules and the temperature of the gas.

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.

"The total kinetic energy of the molecules in an ideal gas with a volume V at pressure P and temperature T is equal to the total kinetic energy of the molecules present in the same volume of another ideal gas at the same pressure and at temperature 2T"-Justify the statement.

At 0^(@)C the kinetic energy of 1O_(2) molecule is 5.62xx10^(-14) erg. Determine avogadro's number.

According to the kinetic theory of gases, the average kinetic energies of O_(2) and N_(2) molecules are the same at a particular temperature. State whether the rms velocities of the molecules of the two gases at a given temperature will be the same or not.

Prove that c_(rms)=sqrt((2E)/(M)) [E=total kinetic energy of the molecules of 1 mol of a gas, M=molar mass of the gas, c_(rms)= root mean square velocity of gas molecule].

Light rays of wavelength lambda and lambda/2 are incident on a a photosensitive metal surface, IF the maximum kinetic energy of the emitted photoelectrons from the metal surface in 2nd case be 3 times the maximum kinetic energy of emitted photoelectrons in the 1st case then determine the work function of the metal.

If, at a given temperature, the totla kinetic energy of the molecules in unit volume of an ideal gas be E, show that the pressure of the gas, P=2//3E .