Question

Which gas can be easily liquefied given 'a' for $ N{{H}_{3}}=4.17,C{{O}_{2}}=3.59,S{{O}_{2}}=6.71,C{{l}_{2}}=6.49 $
(A) $ N{{H}_{3}} $
(B) $ C{{O}_{2}} $
(C) $ S{{O}_{2}} $
(D) $ C{{l}_{2}} $

Answer 1

Hint: A liquefied gas is a gas that has been cooled or compressed to become a liquid. Liquid air, liquefied natural gas, and liquefied petroleum gas are examples of liquefied gases. The physical conversion of a gas to a liquid form is known as liquefaction (condensation). Gas liquefaction is a complex process that employs a variety of compressions and expansions to produce high pressures and extremely low temperatures, such as turboexpanders.

Complete answer:
The Van der Waals equation is a state equation in chemistry and thermodynamics that generalises the ideal gas law based on reasonable reasons why actual gases do not behave ideally.
 $ \left( P+a\dfrac{{{n}^{2}}}{{{V}^{2}}} \right)(V-nb)=nRT $
The van der Waals constants are the constants a and b. They are the pressure and volume correction factors in the ideal gas equation, which adjust two real-world properties: the excluded volume of gas particles and the attraction force between gas molecules. The ideal gas law PV=nRT is proposed by the van der Waals equation of state when the value of these constants approaches zero.
Now, a and b are correction constants, or Van der Waals force of attraction constants, according to van der Waals equation.
Intermolecular attraction is compensated for using ′ a ′. The attraction between molecules lowers the pressure of actual gas, causing the molecules to slow down and reduce collisions with the wall. The higher the value of a, the stronger the attraction between molecules and the easier the gas will compress.
'a' is also stated to be the unit of intermolecular attraction force.
We now know that the stronger the intermolecular interaction, the simpler it is to liquify.
As a result, easily liquefiable gas is more valuable.
Sulfur dioxide is easily liquefiable in this environment.
Hence option C is correct.

Note:
Claude's method, in which the gas is allowed to expand isentropically twice in two chambers, may likewise liquefy air. As it passes through an expansion turbine, the gas has to work while expanding. Because the turbine would be destroyed if the gas converts into liquid, it is not yet liquid. By expanding the air to supercritical pressures, commercial air liquefaction facilities avoid this difficulty. Isenthalpic expansion in a thermal expansion valve is used to complete the liquefaction process.