56 g of nitrogen and 96 g of oxygen are mixed iso-thermally and a total pressure of 10 atm. The partial pressures of oxygen and nitrogen (in atm) are respectively

1.  4, 6

2.  5, 5

3.  6, 4

4.  8, 2

A bottle of dry ammonia and a bottle of dry hydrogen chloride connected through a long tube are opened simultaneously at both ends, the white ammonium chloride ring first formed will be

1.  at the centre of the tube

2.  near the hydrogen chloride bottle

3.  near the ammonia bottle

4.  throughout the length of the tube 

If a  gas expands at a constant temperature 

i.  the pressure decreases

ii.  the kinetic energy of the molecules remains the same

iii.  the kinetic energy of the molecules decreases

iv.  the number of molecules of the gas increase

1.  i, ii

2.  i, ii, iii

3.  i, ii, iv

4.  ii, iii

At what temperature the RMS velocity of gas shown at $50°$c will be doubled?

1.  626 K

2.  1019$°\mathrm{C}$

3.  21 K

4.  1019 K

The density of gas A is twice that of B and the molecular weight of A is half of that of B. The Ratio of partial pressures of ${\mathrm{P}}_{\mathrm{A}} \mathrm{and} {\mathrm{P}}_{\mathrm{B}}$ is

1.  $\frac{1}{4}$

2.  $\frac{4}{1}$

3.  $\frac{2}{1}$

4.  $\frac{1}{2}$

6.4 grams of $\mathrm{a}$ $\mathrm{gas}, \mathrm{at}$ $0°\mathrm{C}$ and 0.99 atm pressure occupies a volume of 2.241 L. The correct statement about this gas is-

[Molecular mass of gas A =64]

1.  The gas is ideal

2.  The gas is real with intermolecular attraction

3.  The gas is real without intermolecular repulsion

4.  The gas is real with intermolecular repulsion greater than intermolecular attraction

The density of a gas is 1.964 g ${\mathrm{dm}}^{-3}$ at 273 K and 76 cm Hg. The gas is-

1.  ${\mathrm{CH}}_4$

2.  ${\mathrm{C}}_2{\mathrm{H}}_6$

3.  ${\mathrm{CO}}_2$

4.  Xe

Two gas bulbs A and B are connected by a tube having a stopcock. Bulb A has a volume of 100 mL and contains hydrogen. After opening the gas from bulb A to the evacuated bulb B, the pressure falls down by 40%. The volume (mL) of B must be

1.  167

2.  67

3.  125

4.  200

At $27°\mathrm{C}$, 500 mL of helium diffuses in 30 minutes. What is the time (in hours) taken for 1000 mL of $S{O}_2$ to diffuse under same experimental conditions?

1.  240

2.  3

3.  2

4.  4

Containers A and B have same gases. The pressure, volume and temperature of A are all twice that of B, then the ratio of number of molecules of A and B are

1.  1 : 2

2.  2 :1

3.  1 : 4

4.  3:2