Hydrogen is heated in a vessel to a temperature of 10,000K. Let each molecule posses an average energy `E_(1)`. A few molecules escape into the atmosphere at 300 K. Due to collisions, their energy changes to `E_(2)`. Calculate ratio `E_(1)//E_(2)`.

Each molecule of nitrogen gas heated in a vessel to a temperature of 5000K has an average energy E_(1) . Some molecule of the gas escape into atmosphere at 300K. Due to collision with air molecules, average kinetic energy of the nitrogen molecule changes to E_(2) . Find the radio E_(1)//E_(2) .

Temperature of an ideal 'gas whose molecules have average kinetic energy 1 e V is

The average kinetic energy of H_(2) molecules at 300 K is E at the same temperature the average kinetic energy of O_(2) molecules is :

Two monoatomic gases are at absolute temperatures 300 K and 350 K respectively. Ratio of average kinetic energy of their molecules is

If the average kinetic energy of a molecule of hydrogen gas at 300 K is E , then the average kinetic energy of a molecule of nitrogen gas at the same temperature is

Average K.E. Of translation of a molecule of gas varies with temperature T of gas is

The average K.E. of hydrogen molecules at 27 °C is E. The average K.E. at 327 °C is