Chemistry Question Bank

For a monatomic gas kinetic energy = E. The relation with rms velocity is (a) 1/ 2 2E u m (b) 1 / 2 3E u 2m (c) 1 / 2 E u 2m (d) 1/ 2 E u 3m

Which one of the following statements is not true about the effect of an increase in temperature on the distribution of molecular speeds in a gas?

The root mean square velocity of an ideal gas at constant pressure varies with density (d) as

The average speed at temperature TºC of CH4(g) is 88 × 103 ms–1. What is the value of T ?

At what temperature most probable speed of O2 molecules have the same value of root mean square speed of O2 molecules at 300 K ?

The ratio between the root mean square velocity of H2 at 50 K and that of O2 at 800 K is

The ratio of the root mean square velocity to average velocity of a gas molecule at a particular temperature is

Which of the following gases would have the highest R.M.S. velocity at 25ºC ?

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

The root mean square speeds at STP for the gases H2, N2, O2 and HBr are in the order :

The temperature of the gas is raised from 27ºC to 927ºC, the root mean square velocity is (a) 927 / 27 times the earlier value

The ratio among most probable velocity, mean velocity and root mean square velocity is given by

Root mean square velocity of a gas molecule is proportional to

By which factor does the root mean square velocity of a gaseous molecule increases, when the temperature is increase from 273 K to 1092 K.

The rms speed of N2 Molecules in a gas sample can be changed by

Helium atom is two times heavier than a hydrogen molecule .At 298 K, the average kinetic energy of a helium atom is

According to kinetic theory of gases, for a diatomic molecule

Which is not true in case of an ideal gas ?

Based on kinetic theory of gases following laws can be proved

According to the kinetic theory of gases, in an ideal gas, between two successive collisions a gas molecule travels

As the temperature is raised from 20ºC to 40ºC, the average kinetic energy of neon atoms changes by a factor of which of the following ?

If a gas expands at constant temperature, it indicates that

Consider three one-litre flasks labeled A, B and C filled with the gases NO, NO2, and N2O, respectively, each at STP. In which flask do the molecules have the highest average kinetic energy?

At what temperature will the molar KE of 0.3 mol of He be the same as that of 0.4 mol of argon at 400 K ?

Which one of the following is not a correct postulate of kinetic theory of gases ?