Advertisements
Advertisements
प्रश्न
Arrange the following in increasing order of boiling points:
(CH3)3 N, C2 H5 OH, C2 H5 NH2
उत्तर
This increasing order of boiling points can be explained by intermolecular hydrogen bonding. Tertiary amines, cannot engage in hydrogen bonding because they have no hydrogen atom bonded to the nitrogen atom, while primary amine undergoes intermolecular hydrogen bonding. But in the case of alcohol, the extent of hydrogen bonding is more as compared to amines because of a more electronegative oxygen atom in alcohol.
(CH3)3N<C2H5NH2<C2H5OH
APPEARS IN
संबंधित प्रश्न
8 g of glucose, C6H12O6 (Molar Mass = 180 g mol−1) is dissolved in 1 kg of water in a sauce pan. At what temperature will this solution boil?
(Kb for water = 0.52 K kg mol−1, boiling point of pure water = 373.15 K)
Define the term Colligative properties
Arrange the following increasing order of their boiling point:
CH3CH2OH, CH3CHO, CH3–O–CH3
0.450 g of urea (mol. wt. 60) in 22.5 g of water show 0.170°C of elevation in boiling point. The molal elevation constant of water is:
Which of the following aqueous solutions should have the highest boiling point?
Why is it not possible to obtain pure ethanol by fractional distillation? What general name is given to binary mixtures which show deviation from Raoult’s law and whose components cannot be separated by fractional distillation. How many types of such mixtures are there?
AB2 is 10% dissociated in water to A2+ and B−. The boiling point of a 10.0 molal aqueous solution of AB2 is ______°C. (Round off to the Nearest Integer).
[Given: Molal elevation constant of water Kb = 0.5 K kg mol−1 boiling point of pure water = 100°C]
Boiling point of a 2% aqueous solution of a non-volatile solute A is equal to the boiling point of 8% aqueous solution of a non-volatile solute B. The relation between molecular weights of A and B is ______.
If the molality of a dilute solution is doubled, the value of the molal elevation constant (Kb) will be ______.
Calculate the boiling point elevation for a solution prepared by adding 10 g of MgCl2 to 200 g of water, assuming MgCl2 is completely dissociated.
(Kb for Water = 0.512 K kg mol−1, Molar mass MgCl2 = 95 g mol−1)
