States of Matter 1 Question 32
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32. The value of van der Waals’ constant $a$ for the gases $\mathrm{O}{2}, \mathrm{~N}{2}$, $\mathrm{NH}{3}$ and $\mathrm{CH}{4}$ are $1.360,1.390,4.170$ and $2.253 \mathrm{~L}^{2}$ atm $\mathrm{mol}^{-2}$ respectively. The gas which can most easily be liquefied is
======= ####32. The value of van der Waals’ constant $a$ for the gases $\mathrm{O}{2}, \mathrm{~N}{2}$, $\mathrm{NH}{3}$ and $\mathrm{CH}{4}$ are $1.360,1.390,4.170$ and $2.253 \mathrm{~L}^{2}$ atm $\mathrm{mol}^{-2}$ respectively. The gas which can most easily be liquefied is
3e0f7ab6f6a50373c3f2dbda6ca2533482a77bed (a) $\mathrm{O}_{2}$
(b) $\mathrm{N}_{2}$
(c) $\mathrm{NH}_{3}$
(d) $\mathrm{CH}_{4}$
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Solution:
- The ease of liquefication of a gas depends on their intermolecular force of attraction which in turn is measured in terms of van der Waals’ constant $a$. Hence, higher the value of $a$, greater the intermolecular force of attraction, easier the liquefication.
In the present case, $\mathrm{NH}_{3}$ has highest $a$, can most easily be liquefied.
