Question

Liquid ammonia is used in refrigerators because:
(A) it has dipole moment
(B) it has high solubility in water
(C) of its basicity
(D) it has high heat of evaporation

Answer 1

HInt: It is profoundly solvent in water. The ammonia atom has a three-sided bipyramidal shape as anticipated by VSEPR hypothesis with a tentatively decided bond point of $ {106.7^0}C. $

Complete Step By Step Solution:
Ammonia is a lackluster gas with a distinctively impactful smell. It is lighter than air, its thickness being $ 0.589 $ occasions that of air. It is handily condensed because of the solid hydrogen holding between atoms; the fluid bubbles at $ - {33.3^0}C{{ }}( - {27.94^0}F) $ , and sticks to white crystals at $ - {77.7^0}C{{ }}\left( { - {{107.86}^0}F} \right) $ . At high temperature and within the sight of a reasonable impetus, ammonia is disintegrated into its constituent components. Decay of ammonia is a somewhat endothermic cycle requiring 5.5 kcal/mol of smelling salts, and yields hydrogen and nitrogen gas. Smelling salts can likewise be utilized as a wellspring of hydrogen for corrosive power devices if the unreacted ammonia can be eliminated. Ruthenium and Platinum impetuses were discovered to be the most dynamic.
Fluid ammonia goes about as a refrigerant in ice plants. Vanishing of a fluid necessities heat energy. At the point when fluid smelling salts vaporizes, it retains huge amounts of warmth without changing its temperature. Thus, ammonia is generally utilized as a refrigerant.
Henceforth the right choice is (D).

Additional Information:
Dissolvable properties
Ammonia promptly breaks up in water. In a fluid arrangement, it tends to be ousted by bubbling. The fluid arrangement of smelling salts is essential. The greatest grouping of ammonia in water (a soaked arrangement) has a thickness of $ 0.880{{ }}g/c{m^3} $ .
Ignition
Ammonia doesn't consume promptly or support ignition, besides under restricted fuel-to-air combinations of $ 15-25\% $ air. At the point when blended in with oxygen, it ignites with a pale yellowish-green fire. Start happens when chlorine is passed into smelling salts, framing nitrogen and hydrogen chloride; in the event that chlorine is available in overabundance, at that point the exceptionally unstable nitrogen trichloride is likewise shaped.

Note:
The focal nitrogen molecule of smelling salts has five external electrons with an extra electron from every hydrogen iota. This gives a sum of eight electrons, or four electron matches that are orchestrated tetrahedrally. Three of these electron sets are utilized as bond sets, which leaves one solitary pair of electrons.