Question

Write balanced chemical equations for each of the following:
(i) When excess of ammonia is treated with chlorine.
(ii) An equation to illustrate the reducing nature of ammonia.

Answer 1

(i) Reaction when excess of ammonia $\left({\mathrm{NH}}_3\right)$ is treated with chlorine:

• Ammonium chloride $\left({\mathrm{NH}}_4\mathrm{Cl}\right)$ is formed along with the liberation of nitrogen when excess of ammonia is treated with chlorine. The balanced chemical equation is:
• $8{\mathrm{NH}}_3\left(\mathrm{g}\right)+3{\mathrm{Cl}}_2\left(\mathrm{g}\right)⟶6{\mathrm{NH}}_4\mathrm{Cl}\left(\mathrm{g}\right)+{\mathrm{N}}_2\left(\mathrm{g}\right)\uparrow$

(ii) Reducing nature of ammonia:

• Copper (II) oxide $\left(\mathrm{CuO}\right)$ is reduced to metallic copper using ammonia.
• $3\mathrm{CuO}\left(\mathrm{s}\right)+2{\mathrm{NH}}_3\left(\mathrm{g}\right)⟶3\mathrm{Cu}\left(\mathrm{s}\right)+3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)+{\mathrm{N}}_2\left(\mathrm{g}\right)\uparrow$