well buddy got that Cl and Ar one... we jz answered absent mindedly... c Cl exists in the form of molecules whereas Ar is monoatomic. and as we know vanderwaal forces don't make a big difference in cmparison to covalent bonds...so the boiling point of Cl2 is more....
PROGRESS ISN'T MADE BY EARLY RISERS OR HARD WORKERS, BUT BY LAZY PEOPLE TRYING TO FIND EASIER WAY TO DO THE SAME.....SO BE LAZZZZYY!!!!
see i hav an answer 4 the fact that cl2 is more easily liquifiable than Ar see my explaination is similar to svj & goes like this .....
Ar having very weak intermolucular vander waals forces does not show large deviations from ideal behaviour at room tempareture indicating it has a low boyle tempareture . cl2 on the other hand has covalent bonds and other forces ..... making it have a very high boyle tempareture (tempareture at which ideal behaviour is obeyed over a series of pressure ) and so it shows large deviations from ideal behaviour more easily liquifiable gases have a high boyle tempareture . REASON 4 TIS - coz if i gas liquifies that means it is deviating from ideal behaviour as an ideal gas has no intermolecular forces it cant be liquified so only at high temparetures a gas like cl2 is at bound state and obeys ideal gas laws ok so at room temp u can easily liquify it .
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