At what temperature, is the root mean square velocity of gaseous hydrogen molecules equal to that of oxygen molecules at 47$°$C:[MP PET 1997, 2000; RPET 1999; AIEEE 2002; J & K CET 2004; Kerala PET 2010]

1. 20 K           

2. 80 K           

3. - 73 K             

4. 3 K

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

Volume, pressure, and temperature of an ideal gas are \(V,\) \(P,\) and \(T\) respectively. If the mass of its molecule is \(m,\) then its density is:
[\(k\)=Boltzmann's constant]

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

On \(0^{\circ}\text{C}\), the pressure measured by the barometer is \(760\) mm.  What will be pressure at \(100^{\circ}\text{C}\)?
1. \(760~\text{mm}\)
2. \(730~\text{mm}\)
3. \(780~\text{mm}\)
4. None of these

By what percentage, should the pressure of a given mass of gas be increased, so as to decrease its volume by 10% at a constant temperature?

1. 5%     

2. 7.2 %       

3. 12.5%         

4. 11.1%

In the adjacent V-T diagram, what is the relation between $P_{1<mspace\; width="1em"></mspace>}and<mspace\; width="1em"></mspace>P_2$ ?

1. $P_2=P_1$                               

2. $P_2>P_1$

3. $P_2<P_1$                                 

4. cannot be predicated
 

Which one of the following graph is correct at constant pressure?

1.		2.
3.		4.

The root-mean-square velocity of the molecules in a sample of helium is $\frac{5}{7}th$ of that of the molecules in a sample of hydrogen.  If the temperature of the hydrogen gas is 0$°$C, that of the helium sample is about:

1. 0$°$C       

2. 5.6$°$C      

3. 273$°$C         

4. 100$°$C

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