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

At relatively high pressure, van der Waals' equation reduces to-

1. PV = RT

2. PV = RT + a/v

3. PV = RT + Pb

4. PV = RT - a/V²

The unit of van der Waals' constant 'a' is:

1. atm litre² mol-²                       

2. dyne cm⁴ mol^-2

3. newton m⁴ mol^-2                     

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 these 

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

In the case of hydrogen and helium the van der Waals' forces are-

1. Strong                 

2. Very strong

3. Weak                   

4. None of the above

In van der Waals' equation of state of the gas, the constant 'b' is a measure of:

1. Intermolecular collisions per unit volume

2. Intermolecular attraction

3. Volume occupied by molecules

4. Intermolecular repulsions

The van der Waals' equation for real gas is:

1. (P + a/V²)(V-b) = RT

2. (P+n²a/V²)(V-nb) = nRT

3. \(P=\frac{nRT}{V-nb}-\frac{an^2}{V^2}\)

4. All of the above

At high pressure, Vander Waal gas equation is reduced to (For 1 mole of gas)

1. Z = 1- a/RTV

2. PV = RT +Pb

3. PV = RT +a/V

4. Z = 1- Pb/RT

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