$a$ and $b$ are van der Waal's constants for gases. Chlorine is more easily liquefied than ethane because

\begin{matrix} Value of a & Value of b C l_{2} > C_{2} H_{6} & C l_{2} < C_{2} H_{6} \end{matrix}

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\begin{matrix} Value of a & Value of b C l_{2} < C_{2} H_{6} & C l_{2} < C_{2} H_{6} \end{matrix}

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\begin{matrix} Value of a & Value of b C l_{2} > C_{2} H_{6} & C l_{2} > C_{2} H_{6} \end{matrix}

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\begin{matrix} Value of a & Value of b C l_{2} < C_{2} H_{6} & C l_{2} > C_{2} H_{6} \end{matrix}

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Solution

The correct option is A $\begin{matrix} Value of a & Value of b C l_{2} > C_{2} H_{6} & C l_{2} < C_{2} H_{6} \end{matrix}$
If gas is more easily liquefied, then attractive force is large.
Thus, $a (C l_{2}) > a (C_{2} H_{6})$
Also, effective volume is smaller if gas is easily liquefied.
Thus, $b (C l_{2}) < b (C_{2} H_{6})$

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Chlorine is more easily liquefied than ethane because ("a” and "b" are van der waals constants for gases).

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