The temperature of a sample of gas is raised from 127ºC to 527ºC. The average kinetic energy of the gas$-$

(1) Does not changes                         

(2) Is doubled

(3) Is halved                                     

(4) Cannot be calculated 

A helium atom is two times heavier than a hydrogen molecule at 298 K, the average kinetic energy of helium is

(1) Two times that of hydrogen molecules

(2) Same as that of hydrogen molecules

(3) Four times that of hydrogen molecules

(4) Half that of hydrogen molecules

The ratio of average molecular kinetic energy of ${\mathrm{UF}}_6$ to that of ${\mathrm{H}}_2$, both at 300 K is$-$

(1) 1 : 1                       

(2) 7 : 2

(3) 176 : 1                   

(4) 2 : 7

A mono atomic gas diatomic gas and triatomic gas are mixed, taking one mole of each ${\mathrm{C}}_{\mathrm{p}}/{\mathrm{C}}_{\mathrm{v}}$ for the mixture is$-$

(1) 1.40                               

(2) 1.428

(3) 1.67                               

(4) 1.33

According to kinetic theory of gases, for a diatomic molecule

(1) The pressure exerted by the gas is proportional to the mean velocity of the molecule.

(2) The pressure exerted by the gas is proportional to the root mean square velocity of the molecule.

(3) The root mean square velocity of the molecule is inversely proportional to the temperature.

(4) The mean translational kinetic energy of the molecule is proportional to the absolute temperature.

The values of vander waals constant ‘a’ for the gases ${\mathrm{O}}_2$, ${\mathrm{N}}_2$, ${\mathrm{NH}}_3$ and ${\mathrm{CH}}_4$ are 1.36, 1.39, 4.17 and 2.253 ${\mathrm{lit}}^2$ atom mol^-2 respectively. The gas which can most easily be liquefied is$-$

(A) ${\mathrm{O}}_2$                                 

(B) ${\mathrm{N}}_2$

(C) ${\mathrm{NH}}_3$                              

(D) ${\mathrm{CH}}_4$

At low pressure, the vander waals equation is written as :

(1) $\mathrm{Z}=1-\frac{\mathrm{a}}{\mathrm{RTV}}$                                 

(2) $\mathrm{Z}=1-\frac{\mathrm{RTV}}{\mathrm{a}}$

(3) $\mathrm{Z}=1+\frac{\mathrm{a}}{\mathrm{RTV}}$                                 

(4) $\mathrm{Z}=1+\frac{\mathrm{RTV}}{\mathrm{a}}$

X ml of ${\mathrm{H}}_2$ gas effuses through a hole in a container in 5 seconds. The time taken for the effusion of the same volume of the gas specified below under ideal condition is

(1) 10 seconds : $\mathrm{He}$                          

(2) 20 seconds : ${\mathrm{O}}_2$

(3) 25 seconds : $\mathrm{CO}$                          

(4) 55 seconds : ${\mathrm{CO}}_2$

A gas mixture consists of 2 moles of oxygen and 4 moles of a argon at temperature T. Neglecting all vibrational modes, the total internal energy of the system is –

(1) 4RT                         

(2) 5RT

(3) 15RT                       

(4) 11RT

Given reaction : $\mathrm{C}\left(\mathrm{s}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\to <mspace\; width="1em"></mspace>\mathrm{CO}\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{H}}_2\left(\mathrm{g}\right)$. Calculate the volume at STP from 48 gm of carbon and excess ${\mathrm{H}}_2\mathrm{O}-$

(A) 179.2 lit.                           

(B) 89.6 lit.

(C) 44.8 lit.                             

(D) 22.4 lit.