The compressibility factor for 1 mol of a van der Waals gas at $0°\mathrm{C}$ and 100 atmospheric pressure is found to be 0.5. The volume of gas is-

1. 2.0224 L

2. 1.4666 L

3. 0.8542 L

4. 0.1119 L

4 grams of an ideal gas occupies 5.6035 liters of volume at 546 K and 2 atm pressure. What is its molecular weight?

1. 4

2. 16

3. 32

4. 64

The kinetic energy of 4 moles of nitrogen gas at 127$°$C is ......... Kcals. (R=2 cal $mo{l}^{-1} K^{-1}$)

1. 4400

2. 3200

3. 4800

4. 1524

A gaseous mixture contains 56 g of $N_2, 44 g of C{O}_2 and 16 g of C{H}_4.$ The pressure of mixture is 720 mm of Hg. The partial pressure of methane is

1. 75 mm

2. 160 mm

3. 180 mm

4. 215 mm

At $25°C and 730 mm pressure, 380 mL of dry$ oxygen was collected. If the temperature is constant, what volume will the oxygen occupy at 760 mm pressure?

1. 365 mL

2. 2 mL

3. 10 mL

4. 20 mL

At a certain pressure, volume of a gas at $27°$C is 20 litre. If the pressure and temperature are doubled, its volume will be

1. 20 liter

2. 40 liter

3. 8.2 liter

4. 10.9 liter

A gas has double the average velocity of $S{O}_2$ gas at any temperature. The gas may be

1. $C{O}_2$

2. $C_2{H}_4$

3. $C{H}_4$

4. $O_2$

The densities of two gases are in the ratio of 1:16. The ratio of their rates of diffusion is

1. 16 : 1

2. 4 : 1

3. 1 : 4

4. 1 : 16

The critical temperature of the water is higher than that of ${\mathrm{O}}_2$ because the ${\mathrm{H}}_2\mathrm{O}$ molecule has

1.  fewer electrons than ${\mathrm{O}}_2$

2.  two covalent bonds

3.  V-shape

4.  dipole moment

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