The partial pressure of a dry gas is:

1. less than that of wet gas

2. greater than that of wet gas

3. equal to that of wet gas

4. none of the above

Partial pressure of Hydrogen in a flask containing 2 gm of H₂ and 32 gm of SO₂ is:

1. 1/16 of total pressure

2. 1/2 of total pressure

3. 2/3 of total pressure

4. 1/8 of total pressure

Which among the following mixtures of gases at room temperature does not obey Dalton's law of partial pressure-

1. He and O₂

2. NH₃ and HCl

3. H₂ and He

4. N₂ and He

For the reaction, N₂ O₅  (g)→2NO₂ (g) + 0.5 O₂ (g),

Calculate the mole fraction of N₂ O₅ (g) decomposed at a constant volume and temperature if the initial pressure is 600 mm Hg and the pressure at any time is 960 mm Hg.  Assume ideal gas behaviour.

The partial pressure of H₂ in a flask containing 2 g of H₂, 14 g of N_2, and 16 g of O₂ is-

1. 1/2 of the total pressure

2. 1/3 of the total pressure

3. 1/4 of the total pressure

4. 1/16 of the total pressure

Equal weights of methane and oxygen are mixed in an empty container at 25°C. The fraction of the total pressure exerted by oxygen is- 

1. 1/3

2. 1/2

3. 2/3

4. $\frac{1}{3}\times \frac{273}{298}$  

In a flask of volume V litres, 0.2 mol of oxygen, 0.4 mol of nitrogen, 0.1 mol of ammonia and 0.3 mol of helium are enclosed at ${27}^{o}C$. If the total pressure exerted by these non-reacting gases is one atmosphere, the partial pressure exerted by nitrogen is-

1. 1 atm

2. 0.1 atm

3. 0.2 atm

4. 0.4 atm

Equal weights of ethane and hydrogen are mixed in an empty container at 25°C. The fraction of the total pressure exerted by hydrogen is- 

1. 1 : 2

2. 1 : 1

3. 1 : 16

4. 15 : 16

A gaseous mixture contains 56 g of N₂, 44 g of CO₂ and 16 g of CH₄. The total pressure of the mixture is 720 mm Hg. The partial pressure of CH₄ is-

1. 180 mm

2. 360 mm

3. 540 mm

4. 720 mm

A closed vessel contains equal number of nitrogen and oxygen molecules at pressure of P mm. If nitrogen is removed from the system, then the pressure will be

(1) $\mathrm{P}$                              

(2) $2\mathrm{P}$

(3) $\mathrm{P}/2$                           

(4) ${\mathrm{P}}^2$