The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by a two step process shown below :

O₃(g) + Cl$${^ \bullet }$$ (g) $$ \to $$ O₂(g) + ClO$${^ \bullet }$$ (g) . . . . . .(i)

k_i = 5.2 × 10⁹ L mol⁻¹ s⁻¹

ClO$${^ \bullet }$$(g) + O$${^ \bullet }$$(g) $$ \to $$ O₂(g) + Cl$${^ \bullet }$$ (g) . . . . . . (ii)

k_ii = 2.6 × 10¹⁰ L mol⁻¹ s⁻¹

The closest rate constant for the overall reaction O₃(g) + O$${^ \bullet }$$ (g) $$ \to $$ 2 O₂(g) is :

Decomposition of H₂O₂ follows a first order reaction. In fifty minutes the concentration of H₂O₂ decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of H₂O₂ reaches 0.05 M, the rate of formation of O₂ will be :

Higher order (>3) reactions are rare due to

For the non – stoichiometre reaction 2A + B $$\to$$ C + D, the following kinetic data were obtained in three separate experiments, all at 298 K. The rate law for the formation of C is: