Page 206 - Instant notes
P. 206

F6
                   THE KINETICS OF REAL SYSTEMS



        Key Notes
                                A chain reaction occurs when a reaction intermediate generated
                                in one step reacts with another species to generate another
                                reaction intermediate. A chain reaction mechanism typically
                                contains several types of elementary reaction steps including
                                initiation, propagation, branching and termination. Mechanisms
                                containing many branching reactions may lead to explosions.
                                Chain branching explosions can arise when an elementary
                                reaction produces more reaction intermediates than are
                                consumed, each of which then instigate further chain branching
                                reactions resulting in a catastrophic accelerated increase in
                                reaction rate. Whether explosion or smooth reaction occurs
                                depends on exact conditions of temperature and pressure.
                                In the lock and key hypothesis of enzyme action, enzyme and
                                substrate are in equilibrium with an enzyme-substrate complex
                                (ES) which can proceed through to products. The Michaelis-
                                Menten equation for the rate of formation of products is
                                v=k 2 [E] 0 [S]/(K M +[S]), where [E] 0  is total enzyme present and K M
                                is the Michaelis constant. The enzyme released from the ES
                                complex is available for further reaction and is therefore a
                                catalyst.
                                A Lineweaver-Burke plot is a linear relationship used to analyze
                                kinetic data on enzyme catalyzed reactions. The reciprocal of the
                                rate of reaction (1/v) is plotted against the reciprocal of substrate
                                concentration (1/[S]) for experiments with the same initial
                                enzyme concentration. The y-axis intercept of the plot is 1/v max
                                and the gradient is K M /v max .
         Related topics         Rate law determination (F2)   Rate laws in action (F5)
                                Formulation of rate laws (F4)




                                     Chain reactions

        In many complex reaction systems, the product of one elementary reaction step is the
        reactant in the next elementary reaction step, and so on. Such systems are called chain
        reactions and the reactive intermediates responsible for the propagation of the reaction
        are called  chain carriers.  Important  examples of such processes include combustion
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