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 

In Haber's process, 30 L of dihydrogen and 30 L of dinitrogen were taken for the reaction which yielded only 50% of the expected product. What is the composition of the gaseous mixture under afore-said conditions in the end?

1.  $20 \mathrm{L} {\mathrm{NH}}_3, 25 \mathrm{L} {\mathrm{N}}_2, 15 \mathrm{L} {\mathrm{H}}_2$

2.  $20 \mathrm{L} {\mathrm{NH}}_3, 20 \mathrm{L} {\mathrm{N}}_2, 20 \mathrm{L} {\mathrm{H}}_2$

3.  $10 \mathrm{L} {\mathrm{NH}}_3, 25 \mathrm{L} {\mathrm{N}}_2, 15 \mathrm{L} {\mathrm{H}}_2$

4.  $20 \mathrm{L} {\mathrm{NH}}_3, 10 \mathrm{L} {\mathrm{N}}_2, 30 \mathrm{L} {\mathrm{H}}_2$

If the rms velocity of a gas at 100 K is ${10}^4 \mathrm{cm} {\sec }^{-1}$, what is the temperature $\left(\mathrm{in} °\mathrm{C}\right)$ at which the rms velocity will be $3\times {10}^4 \mathrm{cm} {\sec }^{-1}$?

1.  900

2.  627

3.  327

4.  1217 

A solution has a 1 : 4 mole ratio of pentane to hexane. The vapour pressures of the hydrocarbons at 20$°$C are 400 mm Hg for pentane and 120 mm hg for hexane. The mole fraction of pentane in the vapour phase would be

1. 0.200

2. 0.549

3. 0.454

4. 0.478

The temperature at which rate of diffusion of $N_2$ would be 1.625 times the rate of diffusion of $S{O}_2 at 50°\mathrm{C\; is\; : }$

1. 110 K

2. 173 K

3. 373 K

4. 273 K