A) a for \[C{{l}_{2}}>a\] a for \[{{C}_{2}}{{H}_{6}}\] but b for \[C{{l}_{2}}<b\]for \[{{C}_{2}}{{H}_{6}}\]
B) a and b for \[C{{l}_{2}}>a\] and b for \[{{C}_{2}}{{H}_{6}}\]
C) a and b for \[C{{l}_{2}}<a\] a and b for \[{{C}_{2}}{{H}_{6}}\]
D) a for \[C{{l}_{2}}<a\] for \[{{C}_{2}}{{H}_{6}}\] but b for \[C{{l}_{2}}>b\] for \[{{C}_{2}}{{H}_{6}}\]
Correct Answer: A
Solution :
The van der Waals constant a is a measure of forces of attraction between gaseous molecules. Larger the value of a, the more easily the gas can be liquefied. Since \[C{{l}_{2}}\] is more easily liquefied than ethane, it follows that \[a(C{{l}_{2}})>a({{C}_{2}}{{H}_{6}})\] 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 \[C{{l}_{2}},\] it follows that \[b(C{{l}_{2}})<b({{C}_{2}}{{H}_{6}}).\]
You need to login to perform this action.
You will be redirected in
3 sec
