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Depending on how many molecules come together, a reaction can be unimolecular, bimolecular or even trimolecular. The kinetic order of any elementary reaction or reaction step is equal to its molecularity, and the rate equation of an elementary reaction can therefore be determined by inspection, from the molecularity. [1]
It breaks down an apparently unimolecular reaction into two elementary steps, with a rate constant for each elementary step. The rate law and rate equation for the entire reaction can be derived from the rate equations and rate constants for the two steps. The Lindemann mechanism is used to model gas phase decomposition or isomerization reactions
The unimolecular nucleophilic substitution (S N 1) reaction is a substitution reaction in organic chemistry. The Hughes-Ingold symbol of the mechanism expresses two properties—"S N " stands for " nucleophilic substitution ", and the "1" says that the rate-determining step is unimolecular .
In chemistry, a reaction mechanism is the step by step sequence of elementary reactions by which overall chemical reaction occurs. [1] A chemical mechanism is a theoretical conjecture that tries to describe in detail what takes place at each stage of an overall chemical reaction. The detailed steps of a reaction are not observable in most cases.
Unimolecular ion decomposition is the fragmentation of a gas phase ion in a reaction with a molecularity of one. [1] Ions with sufficient internal energy may fragment in a mass spectrometer, which in some cases may degrade the mass spectrometer performance, but in other cases, such as tandem mass spectrometry, the fragmentation can reveal information about the structure of the ion.
An elementary reaction is a chemical reaction in which one or more chemical species react directly to form products in a single reaction step and with a single transition state. In practice, a reaction is assumed to be elementary if no reaction intermediates have been detected or need to be postulated to describe the reaction on a molecular ...
The Rice–Ramsperger–Kassel–Marcus (RRKM) theory is a theory of chemical reactivity. [1] [2] [3] It was developed by Rice and Ramsperger in 1927 [4] and Kassel in 1928 [5] (RRK theory [6]) and generalized (into the RRKM theory) in 1952 by Marcus [7] who took the transition state theory developed by Eyring in 1935 into account.
The apparent unimolecular rate constant k cat is also called turnover number, and denotes the maximum number of enzymatic reactions catalysed per second. The Michaelis–Menten equation [ 10 ] describes how the (initial) reaction rate v 0 depends on the position of the substrate-binding equilibrium and the rate constant k 2 .