Real Gases

Q. Consider the following graph and identify how many statements are correct for real gas

(i) At point $A,Z$ approaches one and gas shows ideal behavior
(ii) For curve $AB,Z<1$, force of attraction increases on increasing pressure
(iii) At point $B$, value of compressibility factor is minimum
(iv) For the curve $BC,Z<1$, force of repulsion increases on increasing pressure
(v) At point $C,Z=1$, force of attraction are not equal to force of repulsions
(vi) At the curve $‘C{D}^{\prime },Z>1$, gas is more difficult to compress

Q.

A real gas most closely approaches the behaviour of an ideal gas at

1. 15 atm and 200 K

2. 1 atm and 273 K

3. 15 atm and 500 K

4. 0.5 atm and 500 K

Q.

In Van der Waal's equation of state of the gas law, the constant 'b' is a measure of

1. Volume occupied by the molecules

2. Intermolecular attraction

3. Intermolecular repulsions

4. Intermolecular collisions per unit volume

Q.

Calculate the pressure of one mole of nitrogen gas in a 10 L cylinder at ${50}^{\circ }C$ using the Van der Waal's equation.Also find the value of ideal gas pressure.(Van der Waal's constants a and b for nitrogen are $1.4L^{2}atmmo{l}^{-2}and0.04L^{2}mo{l}^{-1}$ respectively) .

1. 2.18 atm

2. 2.652 atm

3. None of these

4. 2.965 atm

Q.

For one mole of a Van der Waals gas when b = 0 and T = 300 K, then pV vs. $\frac{1}{V}$ plot is shown in figure. The value of the Van der Waals constant "a" $(atm{L}^{2}mo{l}^{-2}$)is___.

1. 3.0

2. 1.0

3. 4.5

4. 1.5

Q.

Which of the given sets of temperature and pressure will cause a gas to exhibit the greatest deviation from ideal gas behavior

1. 100° C and 4 atm

2. 100° C and 2 atm

3. -100° C and 4 atm

4. 0° C and 2 atm

Q.

Gas deviates from ideal gas nature because molecules

1. Attract each other

2. Contain covalent bond

3. Are colourless

4. Show Brownian movement

Q.

At extremely low pressure van der Waal’s equation can be expressed as

1. 

2. 

3. 

4. 

Q.

At high temperature, van der Waal’s equation can be expressed as

1. 

2. 

3. 

4. 

Q.

For one mole of a van der Waal's gas when b =o and T = 300 K, the PV vs $\frac{1}{V}$ plot is shown below. The value of the Van der Waal's constant "a" ($atm{L}^{2}mo{l}^{-2}$) is

1. 3.0

2. 1.0

3. 4.5

4. 1.5