Relative rate techniques were used to study the kinetics of the reactions of Cl atoms and OH radicals with ethylene glycol diacetate, CH ₃C(O)O(CH₂)₂OC(O)CH₃, in 700 Torr of N₂/O₂ diluent at 296 K. The rate constants measured were k(Cl + CH₃C(O)O(CH₂)₂OC(O)CH₃) = (5.7 ± 1.1) × 10^-12 and k(OH + CH₃C(O) O(CH₂)₂OC(O)CH₃) = (2.36 ± 0.34) × 10^-12 cm³ molecule^-1 s^-1. Product studies of the Cl atom initiated oxidation of ethylene glycol diacetate in the absence of NO in 700 Torr of O₂/N₂ diluent at 296 K show the primary products to be CH₃C(O)OC(O)CH₂OC(O)CH ₃, CH₃C(O)OC(O)H, and CH₃C(O)OH. Product studies of the Cl atom initiated oxidation of ethylene glycol diacetate in the presence of NO in 700 Torr of O₂/N₂ diluent at 296 K show the primary products to be CH₃C(O)OC(O)H and CH₃C(O)OH. The CH₃C-(O)OCH₂O radical is formed during the Cl atom initiated oxidation of ethylene glycol diacetate, and two loss mechanisms were identified: reaction with O₂ to give CH₃C(O)OC(O)H and α-ester rearrangement to give CH₃C(O)OH and HC(O) radicals. The reaction of CH₃C(O)OCH₂O₂ with NO gives chemically activated CH₃C(O)OCH₂O radicals which are more likely to undergo decomposition via the α-ester rearrangement than CH ₃C(O)OCH₂O radicals produced in the peroxy radical self-reaction.