In van der Waal's equation of state for a non-ideal gas, the term that accounts for the intermolecular force is-

1. V-b

2. (P+a/V²)

3. RT

4. (RT)^-1

The gas among the following that can be most readily liquified is-

( Value of 'a' for NH₃ = 4.17, CO₂ = 3.59, SO₂ = 6.71, Cl₂ = 6.49)

1. NH₃

2. Cl₂

3. SO₂

4. CO₂

Van der Waals parameter 'a' signifies -

1.The magnitude of intermolecular attractive forces.

2. The magnitude of intermolecular repulsive forces.

3. The volume of a gas molecule.

4. All of the above.

The unit of van der Waals' constant 'b' is -

1. cm³ mol^-1

2. litre mol^-1

3. m³ mol^-1

4. All of the above

For one mole of van der Waal's gas when b=0 and T=300 K, the PV vs. 1/V plot is shown below.

The value of the van der Waal's constant 'a' (atm. ${\mathrm{litre}}^2$ ${\mathrm{mol}}^{-2}$) is-

1. 1.0

2. 4.5

3. 1.5

4. 3.0

At moderate pressure, the van der Waal's equation becomes:

1. PV_m = RT

2. P(V_m-b) = RT

3. (P+a/V²_m) (V_m )= RT

4. P = RT/V_m + a/V²_m

If pressure is in atmosphere and volume in dm³ , then the unit of 'a' is-

1. $\mathrm{atm}$ ${\mathrm{dm}}^6$ ${\mathrm{mol}}^{-2}$

2. $\mathrm{atm}$ ${\mathrm{dm}}^4$ ${\mathrm{mol}}^{-2}$

3. $\mathrm{atm}$ ${\mathrm{dm}}^3$ ${\mathrm{mol}}^{-3}$

4. ${\mathrm{atm}}^{-1}$ ${\mathrm{dm}}^4$ ${\mathrm{mol}}^{-2}$

Van der Waals equation at low pressure is -

1. PV = RT - Pb

2. PV = RT - $\frac{\mathrm{a}}{\mathrm{V}}$

3. PV = RT + $\frac{\mathrm{a}}{\mathrm{v}}$

4. PV = RT + Pb

At lower temperature, all gases except H₂ and He show:

1. Negative deviation

2. Positive deviation

3. Positive and negative deviation

4. None of the above

The ratio a/b (the terms used in van der Waals' equation) has the unit-

1. atm litre mol^-1                           

2. atm dm³ mol^-1

3. dyne cm mol^-1                           

4. All of the above