• # question_answer Consider the following table : Gas $a/(k\,Pa\,d{{m}^{6}}\,mo{{l}^{-1}})$ $b/(\,d{{m}^{3}}\,mo{{l}^{-1}})$ A 642.32 0.05196 B 155.21 0.04136 C 431.91 0.05196 D 155.21 0.4382 a and b are vander waals constant. The correct statement about the gases is:                                                                                     [JEE Main 10-4-2019 Morning] A) Gas C will occupy lesser volume than gas A; gas B will be lesser compressible than gas DB) Gas C will occupy more volume than gas A; gas B will be lesser compressible than gas DC) Gas C will occupy more volume than gas A; gas B will be more compressible than gas DD) Gas C will occupy lesser volume than gas A; gas B will be more compressible than gas D

Correct Answer: C

Solution :

$\bullet$ Gas A and C have same value of 'b' but different value of 'a' so gas having higher value of 'a' have more force of attraction so molecules will be more closer hence occupy less volume. $\bullet$Gas B and D have same value of 'a' but different value of 'b' so gas having lesser value of 'b' will be more compressible. so option [c] is correct.

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