The reaction mechanisms for oxidation of CH₃CCl₂ and CCl₃CH₂ radicals, formed in the atmospheric degradation of CH₃CCl₃ have been elucidated. The primary oxidation products from these radicals are CH₃CClO and CCl₃CHO, respectively. Absolute rate constants for the reaction of hydroxyl radicals with CH₃CCl₃ have been measured in 1 atm of Argon at 359, 376, and 402 K using pulse radiolysis combined with UV kinetic spectroscopy giving 𝓀(OH + CH₃CCl₃) = (5.4 ± 3) 10⁻¹² exp(−3570 ± 890/RT) cm³ molecule⁻¹ s⁻¹. A value of this rate constant of 1.3 × 10⁻¹⁴ cm³ molecule⁻¹ s⁻¹ at 298 K was calculated using this Arrhenius expression. A relative rate technique was utilized to provide rate data for the OH + CH₃ CCl₃ reaction as well as the reaction of OH with the primary oxidation products. Values of the relative rate constants at 298 K are: 𝓀(OH + CH₃CCl₃) = (1.09 ± 0.35) × 10⁻¹⁴, 𝓀(OH + CH₃CClO) = (0.91 ± 0.32) × 10⁻¹⁴, 𝓀(OH + CCl₃CHO) = (178 ± 31) × 10⁻¹⁴, 𝓀(OH + CCl₂O) < 0.1 × 10⁻¹⁴; all in units of cm³ molecule⁻¹ s⁻¹. The effect of chlorine substitution on the reactivity of organic compounds towards OH radicals is discussed.