The average kinetic energy of a helium atom at $30°C$ is:                                                                                           [MP PMT 2004]

1. Less than 1 eV

2. A few KeV

3. 50-60 eV

4. 13.6 eV

The average kinetic energy of a gas molecule can be determined by knowing:                                        [RPET 2000, MP PET 2010]

1. The number of molecules in the gas

2. The pressure of the gas only

3. The temperature of the gas only

4. None  of the above is enough by itself

One liter of gas A and two liters of gas B, both having the same temperature 100$°$C and the same pressure 2.5 bar will have the ratio of average kinetic energies of their molecules as:

1. 1:1       

2. 1:2     

3. 1:4       

4. 4:1

The kinetic energy of one gram molecule of a gas at standard temperature and pressure is: (R = 8.31 J/mol-K)

1. 0.56 $\times {10}^4<mspace\; width="1em"></mspace>J$             

2. $1.3\times {10}^2<mspace\; width="1em"></mspace>J$

3. $2.7\times {10}^2<mspace\; width="1em"></mspace>J$                 

4. $3.4\times {10}^3<mspace\; width="1em"></mspace>J$

Gases exert pressure on the walls of containing vessel because  the gas molecules:

1. Possess momentum

2. collide with each other

3. have finite volume

4. obey gas laws