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Set-I: O2, CO2, H2, He for 'b' values. Set-II: CH4, O2, H2 for 'a' values. Value of van der Waals constant 'b' increases with increase in molecular volume. Clearly, the increasing order of molecular volume (size of molecule) is:

1. He < H2 < O2 < CO2
2. Value of 'a' increases with increase in intermolecular attraction. CH4 is a polar molecule, thus, it will possess highest value of 'a'. O2 and H2, both are non-polar molecules. The van der Waals force α molecular mass. Hence, the correct order of value of 'b' is: CH4 > O2 > H2.
3. From the given options, (c) is most suitable.
4. Given nCO = nN2

Correct answer: He < H2 < O2 < CO2

Solution

The van der Waals constant 'b' is related to the molecular volume, which increases with molecular size. Among the given molecules, He < H2 < O2 < CO2 is the correct increasing order of molecular volume.

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