Eq. No.	Reaction Equations	Reaction Rate Constants (k_i) (cm³/molecules*s)	Initial Concentrations of C_i (molecules/cm³)	Reaction Expression (r)
1	$O_{2} + h v (s u n l i g h t) \to 2 O^{*}$	k₁ = 1.03 × 10⁻⁹⁴	O₂ = 2.00 × 10¹⁷	r₁ = k₁ [O₂]
2	$O^{*} + O^{2} + M \to O_{3} + M$	k₂ = 5.92 × 10⁻³⁴	O = 1.00 × 10⁻⁶	r₂ = k₂ [O₂] [O]
3	$O_{3} + h v (s u n l i g h t) \to O_{2} + O^{*}$	k₃ = 4.38 × 10⁻²⁶	O₃ = 5.00 × 10¹²	r₃ = k₃ [O₃]
4	$C l + O_{3} \to C l O + O_{2}$	k₄ = 1.22 × 10⁻¹¹	Cl = 6.46 × 10⁴	r₄ = k₄ [O₃] [Cl]
5	$C l O + O \to C l + O_{2}$	k₅ = 3.80 × 10⁻¹¹	ClO = 7.22 × 10⁷	r₅ = k₅ [O] [ClO]
6	$C l O + C l O + M \to {(C l O)}_{2} + M$	k₆ = 2.16 × 10⁻³²	(ClO)₂ = 1.00 × 10⁻⁶	r₆ = k₆ [ClO]²
7	${(C l O)}_{2} + h v (s u n l i g h t) \to C l + C l O O$	k₇ = 8.53 × 10⁻¹⁵	(ClO)₂ = 1.00 × 10⁻⁶	r₇ = k₇ [(ClO)₂]
8	$C l O O + M \to C l + O_{2} + M$	k₈ = 6.51 × 10⁻¹³	ClOO = 1.00 × 10⁻⁶	r₈ = k₈ [ClOO]
9	$N O + O_{3} \to N O_{2} + O_{2}$	k₉ = 1.78 × 10⁻¹⁴	NO = 1.00 × 10⁹	r₉ = k₉ [O₃] [NO]
10	$N O_{2} + O \to N O + O_{2}$	k₁₀ = 1.05 × 10⁻¹¹	NO₂ = 1.00 × 10⁹	r₁₀ = k₁₀ [NO₂] [O]
11	$N O_{2} + O_{3} \to N O + 2 O_{2}$	k₁₁ = 1.00 × 10⁻¹⁸	NO₂ = 1.00 × 10⁹	r₁₁ = k₁₁[NO₂] [O₃]
12	$B r + O_{3} \to B r O + O_{2}$	k₁₂ = 1.18 × 10⁻¹²	Br = 3.2 × 10⁵	r₁₂ = k₁₂ [Br] [O₃]
13	$B r O + C l O \to B r C l + O_{2}$	k₁₃ = 1.02 × 10⁻¹²	BrO = 6.4 × 10⁶	r₁₃ = k₁₃ [BrO] [ClO]
14	$B r C l + h v (s u n l i g h t) \to Br + C l$	k₁₄ = 1.06 × 10⁻⁸	BrCl = 1.00 × 10⁻⁶	r₁₄ = k₁₄ [Br] [Cl]