The compressibility of a gas is less than unity at STP. Therefore:

(1) V_m > 22.4 litre                           

(2) V_m < 22.4 litre

(3) V_m = 22.4 litre                           

(4) V_m = 44.8 litre

The numerical value of C_p-C_v for one mole of the ideal gas is equal to:

1. R             

2. R/M

3. M/R         

4. None of the above

In which case is the rate of diffusion highest if all are present in the same container at the same temperature:

1. 4 g H₂

2. 32 g O₂

3. 22 g CO₂

4. 56 g N₂

Partial pressure of Hydrogen in 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

At high pressure, the compressibility factor 'Z' is equal to -

1.  Unity

$2.$ $1-\frac{\mathrm{Pb}}{\mathrm{RT}}$
$3.$ $1+\frac{\mathrm{Pb}}{\mathrm{RT}}$

4.  Zero

The density of O₂(g) is maximum at:-

1. STP

2. 273 K and 2 atm 

3. 546 K and 1 atm

4. 546 K and 2 atm

A gas diffuses four time quickly as oxygen. The molecular weight of gas is:

1. 2

2. 4

3. 8

4. 16

If density of vapours of a substance of molar mass 18 gm / mole at 1 atm pressure and 500 K is 0.36 kg m^–3 , then value of Z for the vapours is : (Take R = 0.082 L atm mole K^–1)

(1) $\frac{41}{50}$

(2) $\frac{50}{41}$

(3) 1.1

(4) 0.9

A sample of water gas has a composition by volume of 50% H₂, 45% CO and 5% CO₂. Calculate the volume in litre at S.T.P. of water gas which on treatment with excess of stream will produce 5 litre H₂. The equation for the reaction is : CO + H₂O $\stackrel{}{\to }$ CO₂+ H₂

(1) 4.263 Litre

(2) 5.263 Litre

(3) 6.263 Litre

(4) 7.263 Litre

A 2 m long tube closed at one end is lowered vertically into' water until the closed end is flush with the water surface. See figure below. Calculate the water level height in the tube. (Barometric pressure –1 atm =10 m of hydrostatic water head, Temperature = 25°C, Density of, water = 1.00 g/ml. Neglect water vapour pressure).

(1) 1.01 m

(2) 0.29 m

(3) 1.71^–m

(4) 0.92 m