What is Ammonia Used For?

A chemical reaction of ammonia is the addition reaction of ammonia, the most common is the reaction with water.

Ammonia is the use of non-shared electron couples on nitrogen atoms through the formation of covalent bonds, the addition of ionic-dipole electrostatic interactions, or the addition of ammonia molecules to other molecules or ions through hydrogen bonding. The most common ammonia reaction is the reaction with water.

Ammonia has a very large solubility in water, and water and ammonia have a strong tendency to combine. (Ammonia is soluble in 700 volumes of ammonia in 1 volume of water at 20 ° C and 1 atmosphere). The free constant of ammonia hydrate (ammonium hydroxide) in aqueous solution (at 25 ° C) is 1.65 × 10 ^-5 , which can be seen as a weak electrolyte. The phase diagram of the NH ₃ · H ₂ O system indicates that NH ₃ · H ₂ O exists in the solid state below -80 ° C, and 2NH ₃ · H ₂ O compounds also exist in these cases. Ammonia easily reacts with strong acids to form ammonium salts, as shown in equation (2). Solid, weakly acidic ammonium salts readily decompose into ammonia and free acids. Included in the ammoniation reaction are complexes (known as amines) formed with many metal ions, especially transition metal ions. All kinds of molecules that can act as electron acceptors (Lewis acid) can undergo ammoniation. The reaction of ammonia with such substances as sulfur trioxide, sulfur dioxide, silicon tetrafluoride and boron trifluoride is typical. ^[1]

Most of the chemical reactions of ammonia can be divided into three major categories: (1) addition reactions, commonly referred to as ammoniation; (2) displacement reactions, commonly referred to as ammonolysis; (3) oxidation-reduction reactions.

Ammonia hydrolysis

Ammonialysis reactions include reactions in which one amino group (-NH2), one imino group (-NH), or one nitrogen group (-N) replaces one or more atoms or groups in the reaction molecule.

- Ammonia synthesis oxidation-reduction

These reactions can be subdivided into those that change the oxidation state of nitrogen atoms and release elemental hydrogen. An example of the first type is the catalytic oxidation of ammonia in the air to form nitrogen oxides. When there is no catalyst, ammonia burns in oxygen to produce nitrogen. One example is the reduction of hot metal oxides such as copper oxide by ammonia, and another example is the reaction of ammonia with chlorine. The second type of ammonia oxidation-reduction reaction can be exemplified by the reaction of an active metal with ammonia.