question_answer

The van der Waals constants for two gases are as follows : Gas        \[a\,(atm\,{{L}^{2}}\,mo{{l}^{-2}})\]       \[b\,(L\,mo{{l}^{-1}})\] X                             1.39                     0.0391 Y                              3.59                     0.0427 Which of them is more easily liquefiable and which has greater molecular size?

Answer:

                Greater the value of 'a', more easily the gas is liquefiable. Similarly, greater the value of 'b', greater is the molecular size. Hence, gas Y will be more easily liquefiable and will have greater molecular size.