Match List-I with List-II with the corresponding boiling points.
|
List-I Compound Name |
List-II Boiling Point |
|
(A) $CH_3CH_2OH$ |
(I) 373K |
|
(B) $CH_3OCH_3$ |
(II) 348K |
|
(C) $H_2O$ |
(III) 351K |
|
(D) $CH_3CH_2OCH_2CH_3$ |
(IV) 248K |
Choose the correct answer from the options given below:
Answer & explanation
Correct answer: option 1
The correct answer is Option (1) → (A)-(III), (B)-(IV), (C)-(I), (D)-(II)
|
List-I Compound Name |
List-II Boiling Point |
|
(A) $CH_3CH_2OH$ |
(III) 351K |
|
(B) $CH_3OCH_3$ |
(IV) 248K |
|
(C) $H_2O$ |
(I) 373K |
|
(D) $CH_3CH_2OCH_2CH_3$ |
(II) 348K |
Core Concept
Boiling point depends on intermolecular forces like hydrogen bonding and molecular size.
Detailed Explanation
Compound A: $CH_3CH_2OH$
Ethanol shows intermolecular hydrogen bonding due to -OH group, giving it a relatively high boiling point around 351 K.
Hence (A) matches with (III).
Compound B: $CH_3OCH_3$
Dimethyl ether cannot form intermolecular hydrogen bonding. It only has dipole-dipole forces and thus has a low boiling point around 248 K.
Hence (B) matches with (IV).
Compound C: $H_2O$
Water forms extensive hydrogen bonding networks leading to a very high boiling point of 373 K.
Hence (C) matches with (I).
Compound D: $CH_3CH_2OCH_2CH_3$
Diethyl ether is larger than dimethyl ether and has stronger dispersion forces but still lacks hydrogen bonding. Its boiling point is around 348 K.
Hence (D) matches with (II).