What is the half-life for the decomposition of NOCl when the concentration of NOCl is 0.15 M? The rate constant for this second-order reaction is \({\bf{8}}{\bf{.0 \times 1}}{{\bf{0}}^{{\bf{ - 8}}}}\)L/mol/s.

The reaction involved the effective collision of two reactants to produce the desired products. Reactions can be natural, which occur in the surrounding environment, whereas it can be artificially done in the laboratory to form a desired required product.

The reaction rate can be defined as the speed of reaction to produce the products. The reaction rate can be slow, fast or moderate. The reaction can take less than a millisecond to produce products, or it can take years to produce the desired product.

The half-life period can be defined as the time period at which half the concentration of the reactants gets converted into a product.

The half-life period of the second-order decomposition of the NOCl is:

\({\bf{Half - life period = }}\frac{{\left( {\bf{A}} \right){\bf{^\circ }}}}{{{\bf{2k}}}}\)

Where \(\left( {\bf{A}} \right){\bf{^\circ }}\) = initial concentration of reactant

K = Rate constant

Initial concentration of reactant,\(\left( {\bf{A}} \right){\bf{^\circ }}\) =0.15 M

Rate constant for the decomposition of NOCl =\({\bf{8}}{\bf{.0 \times 1}}{{\bf{0}}^{{\bf{ - 8}}}}\) L/mol/s

\({\bf{Half - life period = }}\frac{{{\bf{0}}{\bf{.15}}}}{{{\bf{2 \times }}\left( {{\bf{8}}{\bf{.0 \times 1}}{{\bf{0}}^{{\bf{ - 8}}}}{\bf{yea}}{{\bf{r}}^{{\bf{ - 1}}}}} \right)}}\)

Half-life period = 93750000 years.

Therefore, the half-life period of the second-order decomposition of the NOCl is 93750000 years which has a rate constant is \({\bf{8}}{\bf{.0 \times 1}}{{\bf{0}}^{{\bf{ - 8}}}}\)L/mol/s.