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An introduction to chemical kinetics by Michel Soustelle

By Michel Soustelle

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Definition A chain reaction is a reaction in which a small number of elementary steps are repeated a large number of times following each other through a small number of intermediate species that are constantly formed and destroyed. 2. R2b] in hydrogen bromide synthesis). By extension, a simple linear reaction consisting of a large number of steps very close to each other is also called a chain reaction. 5) are also considered to be chain Reaction Mechanisms and Elementary Steps 35 reactions. Each step is very similar to the previous step because each time just a small entity is added in the molecular chain.

This ratio does not vary with the extent of the reaction. This ratio is not useful for gaseous phases because all the gases have the same molar volume. It is interesting, however, in the case of solid–solid reactions such as, for example, the expansion coefficient of an oxide with respect to its metal. The volumetric speed of a single-zone reaction is the speed of the reaction per unit of volume (the areal speed will be used for 2D zones). 11b] The volumetric speed (areal speed) is thus expressed in moles per second and m3 (moles per second and m2).

2. Free radicals Free radicals are unstable molecules; the instability is due to the presence of unpaired or extremely available electrons. For instance, the pyrolysis of tetraethyl lead releases ethyl radicals: Pb(C2H5)4 = Pb(C2H5)2 + 2 C2H5. R6] The tert-butyl peroxide is a compound formed from a relatively weak central bond O–O: (CH3)3COOC(CH3)3. It is thus a product that, even at ordinary temperature, tends to break down slowly. It therefore generates free radicals: (CH3)3CO°, that are likely to initiate reactions.

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