Solution: Ozone decomposes to oxygen according to the equation 2O3 (g) ⟶ 3 O2 (g). Write the equation that relates the rate expressions for this reaction in terms of the disappearance of O3 and the formation of oxygen.

We’re being asked to write the rate expression in terms of a) the rate of disappearance of O₃ and b) rate of formation of O₂ for the following reaction: 

2O_{3 (g)} ⟶ 3 O_{2 (g).}

Recall that for a reaction aA → bB, the rate of a reaction is given by:

$\boxed{\mathbf{Rate}\mathbf{=}\mathbf{-}\frac{\mathbf{1}}{\mathbf{a}}\frac{\mathbf{\Delta }\mathbf{\left[}\mathbf{A}\mathbf{\right]}}{\mathbf{\Delta t}}\mathbf{=}\frac{\mathbf{1}}{\mathbf{b}}\frac{\mathbf{\Delta }\mathbf{\left[}\mathbf{B}\mathbf{\right]}}{\mathbf{\Delta t}}}$

where:

Δ[A] = change in concentration of reactants or products (in mol/L or M), [A]_final – [A]_initial

Δt = change in time, t_final – t_initial

a, b = stoichiometric coefficients from balanced equation