By Bernard Lewis
Combustion, Flames and Explosions of Gases, 3rd variation presents the chemist, physicist, and engineer with the clinical foundation for figuring out combustion phenomena.
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Additional info for Combustion, Flames and Explosions of Gases
The boundary of the peninsula region is described by an equation representing a combination of both chain-breaking mechanisms. This equation is of second or higher order with respect to [M], which at temperatures sufficiently above the tip reduces to either equation (2) or (4). At the tip itself the values of the coefficients are such that the equa tion has only one real root. Experimental facts concerning the junction of first and second explo sion limits are illustrated in Fig. 2. The experimental points were deter mined by either the withdrawal method or heating method.
1 \^EL 600 0 200 PRESSURE, MM. Hg 400 600 800 FIG. 7. Initial reaction rates of mixtures of 2H2 + 0 2 . Curves calculated from equations (35), (36), (42)-(47). Experimental rates X Vessel coated with KC1. Δ Vessel coated with BaCl2. O Vessel coated with K2B407. D Vessel coated with K2B204 -f- KOH. • Vessel coated with Na2W04. The 8-cm. 9-cm. BaCLr and Na2W04-coated vessel were quartz. All the other vessels were Pyrex. 49 1. THE THERMAL REACTION of pressure and mixture composition on the rate. The partial pressure of oxygen was held constant at 100 mm.
In the calculations, therefore, it is allowable to use the latter diameter. The effect of vessel diameter may be gaged from Fig. 4-cm. vessel is also included. The rate data of Fig. 10 approach the third explosion limit in the region of water inhibition, and the higher reaction rates drop considerably below the theoretical curve. This is explained if it is granted that a small amount of water was formed during the manipula tion period. 4 mm. 7 mm. Hg will cause the rate to 15 C. F, Cullis and C.
Combustion, Flames and Explosions of Gases by Bernard Lewis