By Bernard Lewis

Combustion, Flames and Explosions of Gases, 3rd variation presents the chemist, physicist, and engineer with the medical foundation for figuring out combustion phenomena.

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Example text

First and third limits are partly extra­ polated. First limit is subject to erratic changes. reactions I to III must be supplemented by suitable equations describing the process of diffusion, adsorption, and surface recombination of H, O, and OH. Russian work has shown2»4 that in general it is possible to neg­ lect the diffusion of O and OH because of the high rates of their gas phase reactions. These authors have studied the first explosion limit ex­ tensively and have been able to obtain satisfaòtory correlations between experiment and theory.

Thus, kinetically the effect of oxygen is substantially that of a diluent. A quantitative calculation based on equation (10) shows similarly the incompatibility of reaction (b) with data of the authors1 on the relation between the rate of water formation and the mole fractions of hydrogen and oxygen. 4-cm. KCl-coated spherical vessel at 530°C, show that the percentage change of the reaction rate as a function of ratio of hydrogen to oxygen remains sensibly constant over a considerable range of pressure (500 to 800 mm.

The explanation of this effect on the basis of the proposed mechanism is as follows. According to reaction (XII), for every 2H0 2 's destroyed at the surface, 1H 2 0 2 is formed. If H 2 0 2 is destroyed solely by reaction (VII), then for every H 2 0 2 released from the wall, 1H0 2 is regenerated to H since OH always reacts by reaction (I) to form H. In this case the explosion condition is no longer 2fc2 = fc6 [M] e but 3fc2 = fc6[M]e. (21) If H 2 0 2 is destroyed solely by reaction (V), its destruction is ac­ complished without changing the H or H 0 2 concentrations, and the ex­ plosion condition is again 2fc2 = fc6[M]c.

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Combustion, Flames and Explosions of Gases by Bernard Lewis
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