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The initial rate of oxidation of benzaldehyde in benzene solution in the absence of catalysts and inhibitors is given by the relation (-d[O 2 ]/d t ) = ([ R H] 2 [O 2 ])/( b [ R H] 2 + c [O 2 ]). The reciprocals of the constants b and c vary with temperature according to the Arrhenius equation, the corresponding activation energies being 6.0 ± 0.5 and 17.5 ± 1.0 kcal/mole respectively. The difficulty of interpreting the relation in terms of the mechanism proposed by Bolland & Gee (1946) for photochemical and peroxide catalyzed oxidations is pointed out. It is suggested that this kinetic behaviour is of widespread occurrence in uncatalyzed oxidations.

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