$' a'$ and $' b'$ are van der Waals constants of gases, Chlorine is more easily liquefied than ethane because

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$a$ for ${Cl}_{2} < a$ for $C_{2} H_{6}$ but $b$ for $C_{2} H_{6}$ but $b$ for ${Cl}_{2} > b$ for $C_{2} H_{6}$

$a$ for ${Cl}_{2} > a$ for $C_{2} H_{6}$ but $b$ for ${Cl}_{2} < b$ for $C_{2} H_{6}$

$a$ and $b$ for ${Cl}_{2} > a$ and $b$ for $C_{2} H_{6}$

$a$ and $b$ for ${Cl}_{2} < a$ and $b$ for $C_{2} H_{6}$

answer is A.

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Detailed Solution

The van der Waals constant a is measure of forces of attraction between gaseous molecules. Larger the value of a, the more easily the gas can be liquefied. Since ${Cl}_{2}$ is more easily liquefied than ethane, it follows that $a ({Cl}_{2}) > a (C_{2} H_{6})$ .

The van der Waals constant b is a measure of effective volume occupied by gaseous molecules. Larger the size of the molecule, larger the value of b, Since $C_{2} H_{6}$ seems to be larger in size than ${Cl}_{2}$ , it follows that $b ({Cl}_{2}) < b (C_{2} H_{6})$ .