Find the answer please quickly to the given question

Dear Student,

To which extent a gas can be liquified depends upon its critical temperature and Vander waals forces of attraction.
That is greater the critical temperature, more easily the gas will be liquified.
Below is the critical temperature of these gases :

NH₃=406K
Cl₂=417K
SO₂=430K
CO₂=304K
 
Now, below given is the Vander waals equation :
$$\begin{gathered} (\mathrm{P}+\frac{{\mathrm{n}}^2\mathrm{a}}{{\mathrm{V}}^2}) (\mathrm{V}-\mathrm{nb})=\mathrm{nRT} (\mathrm{For} \mathrm{n} \mathrm{number} \mathrm{of} \mathrm{moles}) \\ \mathrm{where} \mathrm{P} \mathrm{is} \mathrm{pressure}, \mathrm{V} \mathrm{is} \mathrm{volume}, \mathrm{R} \mathrm{is} \mathrm{universal} \mathrm{gas} \mathrm{constant} \\ \mathrm{and} \mathrm{T} \mathrm{is} \mathrm{temperature}. \\ \mathrm{a} \mathrm{and} \mathrm{b} \mathrm{are} \mathrm{Vander} \mathrm{waals} \mathrm{correction} \mathrm{that} \mathrm{is} \mathrm{Vander} \mathrm{waals} \mathrm{force} \\ \mathrm{of} \mathrm{attraction} \mathrm{constant}. \\ \text{'}\mathrm{a}\text{'} \mathrm{is} \mathrm{basically} \mathrm{said} \mathrm{to} \mathrm{be} \mathrm{measure} \mathrm{of} \mathrm{intermolecular} \mathrm{force}. \end{gathered}$$

Liquifaction of gases is directly proportional to 'a'(intermolecular force) which means greater the value of
'a', greater will be liquifaction of gases.That is large value of 'a' coefficients indicates relatively strong
intermolecular force of attraction. And value of 'a' is greater for SO₂ gas in comparison to Cl_​2 gas
,therefore SO₂ will be liquified more easily.
For SO₂,
value of a=6.71
For Cl₂,
value of a=6.49

From here we can say that SO₂ will liquified more easily in comparison to Cl₂.

Hence the correct option will be (3)

Regards