Behaviour of Real Gases

The pressure exerted by 1 mole of CO₂ at 273 K, is 34.98 atm. Assuming that volume occupied by CO₂ molecules is negligible, the value of van der Waals' constant for attraction of CO₂ gas is :

In Van der Waal’s equation of state for a non-ideal gas, the term that accounts for intermolecular forces is:

Van der Waal’s real gas, act as an ideal gas, at which conditions ?

At which one of the following temperature – pressure conditions the deviation of a gas from ideal behaviour is expected to be minimum ?

When deviation is more in the behaviour of a gas from the ideal gas equation PV = nRT ?

According to kinetic theory, the gas particles occupy a negligible fraction of the total volume of the gas. This assumption is responsible for the volume correction in the ideal gas equation of real gases.

Mentions two assumptions of kinetic theory of gases, which are responsible for the volume correction in the ideal gas equation of real gases.

Explain the factors responsible for the volume correction in the ideal gas equation of real gases.

The isotherms of a gas are shown below :

Among the following,

(i) At ${\mathrm{T}}_1$, the gas cannot be liquefied

(ii) At point $\mathrm{B}$, liquid starts to appear at ${\mathrm{T}}_2$

(ii) ${\mathrm{T}}_{\mathrm{C}}$ is the highest temperature at which the gas can be liquefied

(iv) At point $\mathrm{A}$, a small increase in pressure condenses the whole system to a liquid

The correct statements are :

Which of the following expressions is correct between the van der Waals constant $\mathrm{b}$ and the radius $\mathrm{r}$ of spherical molecules?

For an ideal gas, the compressibility factor is

For one mole of a van der Waals' gas, the compressibility factor $Z=\left(\frac{pV}{RT}\right)$ at a fixed volume will certainly decrease, if
[Given : " a " and " b " are standard parameters for van der Waals' gas]
 

The pressure $\left(\mathrm{p}\right)$ and volume $\left(\mathrm{V}\right)$ isotherm of a van der Waals' gas, at the temperature at which it undergoes gas to liquid transition, is correctly represented by

$\frac{{\mathrm{n}}^2\mathrm{a}}{{\mathrm{v}}^2}$ is also called internal _____ of the gas where $\text{'}\mathrm{a}\text{'}$ is a measure of force of attraction between gas molecule.

Which of the following represents a plot of compressibility factor $\left(\mathrm{Z}\right)$ vs pressure $\left(\mathrm{P}\right)$ at room temperature for ${\mathrm{O}}_2?$

Under which of the following conditions does a gas deviate the most from ideal behaviour?

Write invalid Assumptions of Kinetic Theory for Real Gases which are questionable.

For real gases, as pressure increases, the volume of a gas becomes very small and approaches zero.

For one mole of a van der Waals gas when $\mathrm{b}=0$ and $\mathrm{T}=300 \mathrm{K}$, the $\mathrm{PV} \mathrm{vs} \mathrm{I}/\mathrm{V}$ plot is shown below. The value of the van der Waals constant $\text{'}\mathrm{a}\text{'} (\mathrm{atm}. {\mathrm{litre}}^2 {\mathrm{mol}}^{-2})$is