Question

What is the equivalent mass of nitrogen in $ N{H_3} $ for following reactions
$ {N_2} + 3{H_2} $ gives $ 2N{H_3} $ ?

Answer 1

Hint: The molecular weight of the solute divided by the valence of the solute gives the equivalent weight of a solution. In an acid-base analysis, such as titration, equivalent weight is used to determine the mass of a chemical that reacts with one atom of hydrogen.
Equivalent mass of $ N = \dfrac{{Molar{\text{ mass}}}}{{{n_f}}} $
 $ {n_f} = $ Valency.

Complete answer:
The given reaction is:
 $ {N_2} + 3{H_2} \to 2N{H_3} $
Here the oxidation state of $ N $ in $ {N_2} $ is $ 0 $ . Whereas, the oxidation state of $ N $ in $ N{H_3} $ is $ - 3 $ .
Hence, we can say that $ 3 $ electrons are accepted by $ N $ .
Therefore, the valence factor of $ N $ is $ 3 $ .
Using the formula of Equivalent mass,
Equivalent mass of $ N = \dfrac{{Molar{\text{ mass}}}}{{{n_f}}} $
Substituting the values, we get
Equivalent mass of $ N = \dfrac{{14}}{3} $
Equivalent mass of $ N \Rightarrow 4.67 $

Additional Information:
The given reaction is a combination reaction as nitrogen and hydrogen combine to form ammonia. A combination reaction is a reaction in which one compound is formed by mixing two reactants. A synthesis reaction is another name for a combination reaction. The formation of new bonds is involved in combination reactions, and this process releases a lot of energy in the form of heat. Hence, they are exothermic in nature.

Note:
Atomic weight is the average value of all the masses of a chemical element's naturally occurring isotopes, while valency is the atom's combining capacity. An atomic mass unit is a measure of equal weight.