The van der Waals equation for one mole of a real gas can be written as $\left(P + \dfrac{a}{V^{2}}\right)\left(V – b\right) = RT$ . For the gases ${H}_{2}$ , $N{H}_{3}$ , and $C{H}_{4}$ , the value of 'a' $barL^{– 2}mol^{– 2}$ are 0.2453, 4.170 and 2.253 respectively.
Which of the following can be inferred from the 'a' values?

Question

The van der Waals equation for one mole of a real gas can be written as

\left(P + \dfrac{a}{V^{2}}\right)\left(V – b\right) = RT

. For the gases

{H}_{2}

,

N{H}_{3}

, and

C{H}_{4}

, the value of 'a'

barL^{– 2}mol^{– 2}

are 0.2453, 4.170 and 2.253 respectively.
Which of the following can be inferred from the 'a' values?

Quantrex Academy · Accepted Answer

Correct answer: A. N H _ 3 can be most easily liquified

Van der Wall's constant 'a' gives information about force of attraction between gaseous molecules. Higher the value of 'a' higher will be force of attraction, and easier the liquefaction of gas. Order of intermolecular force of attraction = H _ 2 < C H _ 4 < N H _ 3

The van der Waals equation for one mole of a real gas can be...

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