The distribution of speeds of molecules of a gas depends on
(i) temperature , (ii) volume
(iii) pressure , (iv) molecular mass

The mass of a gas does not depend upon its temperature or pressure.

The density of a gas depends up on its molar mass, pressure and temperature

Will the kinetic energy of molecules increase, decrease or remain same if : (i) the temperature is increased ? (ii) the pressure is decreased ? (iii) the volume is decreased ?

Maxwell and Boltzmann have shown that actual distribution of molecular speeds depends on temperature and molecular mass. At the same temperature which will move faster, N_2 or Cl_2 ?

According to Avogadro,s law, V = k_(4)T . The value of k_(4) (proportionality constant) depends upon (i) temperature (ii) pressure (iii) volume (iv) nature of gas

On which of the following factors does the average kinetic energy of gas molecules depends ? (i) Nature of the gas, (ii) absolute temperature, (iii) volume, what will be its value at the absolute zero ?

The relationship between volume and number of molecules of a gas at constant temperature and pressure is known as ........

Maxwell and Boltzmann have shown that actual distribution of molecular speeds depends, on temperature and molecular mass. What do you mean by most probable velocity?

There are N molecules of a gas in a containter. If this number is increased to 2N, what will be (i) pressure (ii) total energy (iii) rms speed of the gas ?