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NH₃ gas is liquefied more easily than N₂. Hence,

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van der waals' constants a and b of NH₃ > that of N₂

van der waals' constant a and b of NH₃ < that of N₂

$a ({NH}_{3}) > a (N_{2}) but b ({NH}_{3}) < b (N_{2})$

$a ({NH}_{3}) < a (N_{2}) but b ({NH}_{3}) > b (N_{2})$

answer is A.

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Detailed Solution

If a gas is liquefied, it means volume is decreased and attractive force exists. a is a measure of attractive force and b the co-volume hence,

$a ({NH}_{3}) > a (N_{2}) and b ({NH}_{3}) > b (N_{2})$

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