Question

Complete and balance the following equation and also state the type of reaction that is taking place:

$\mathrm{KBr}+{\mathrm{Cl}}_2\stackrel{}{\to }$

Answer 1

Displacement reaction:

• It is a chemical reaction in which an element replaces another element in a compound and takes its place.
• The most reactive metal occupies the top position in the series whereas the least reactive metal is at the bottom of the series.
• For example when potassium bromide$\left(\mathrm{KBr}\right)$ reacts with chlorine gas$\left({\mathrm{Cl}}_2\right)$ it forms potassium chloride$\left(\mathrm{KCl}\right)$ along with bromine gas$\left({\mathrm{Br}}_2\right)$.
• $\underset{\mathrm{Potassium}\mathrm{bromide}}{2\mathrm{KBr}\left(\mathrm{aq}\right)}+\underset{\mathrm{Chlorine}\mathrm{gas}}{{\mathrm{Cl}}_2\left(\mathrm{g}\right)}\stackrel{}{\to }\underset{\mathrm{Potassium}\mathrm{chloride}}{2\mathrm{KCl}\left(\mathrm{s}\right)}+\underset{\mathrm{Bromine}}{{\mathrm{Br}}_2\left(\mathrm{g}\right)}$
• It is the displacement of a less reactive non-metal by a more reactive non-metal.