Question

Answer + Explain why other options are incorrect

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Answer 1

Answer:

I think the answer is option D

MARK ME AS BRAINEST

Answer 2

Answer:

(a) is the correct answer of the question

(a) Measure of effective size of gas molecules

Explanation:

The Van der Waals constant b in a corrected equation for real gases represents: measure of effective size of gas molecules

Repulsive interactions are short-range  interactions and are significant when  molecules are almost in contact. This is the  situation at high pressure. The repulsive forces  cause the molecules to behave as small but impenetrable spheres. The volume occupied by the molecules also becomes significant because instead of moving in volume V, these are now restricted to volume (V–nb) where nb is approximately the total volume occupied by the molecules themselves.

[This part is given in NCERT Chemistry 11th, States of matter chapter ; Pg 151]

The Van der Waals constant 'a' is magnitude of attractive forces among gas molecules.

Free volume is V - nb

We cannot find the difference of pressure and volume as both are of different units.

Hope it helps!