For real gases,the relation between P,V and T | vedclass

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(A) $(i)$ The van der Waals constant $'a'$ represents the magnitude of intermolecular forces of attraction. Larger molecules with more electrons exhib

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$(i) CO_2, (ii) H_2$

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(A) $(i)$ The van der Waals constant $'a'$ represents the magnitude of intermolecular forces of attraction. Larger molecules with more electrons exhibit stronger van der Waals forces. Comparing the given gases,$CO_2$ has the highest molecular mass and number of electrons,thus it has the highest value of $'a'$.$(ii)$ The van der Waals constant $'b'$ represents the excluded volume,which is proportional to the size of the gas molecules. Among the given gases,$H_2$ is the smallest molecule,therefore it has the lowest value of $'b'$.Thus,the correct answer is $(i) CO_2, (ii) H_2$.

For real gases,the relation between $P$,$V$ and $T$ is given by the van der Waals equation,$(P + \frac{an^2}{V^2})(V - nb) = nRT$. For the following gases $CH_4, CO_2, O_2, H_2$,which gas will have $(i)$ highest value of $'a'$ $(ii)$ lowest value of $'b'$?

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