Everything about Second Order Reaction totally explained
The
reaction rate or
rate of reaction for a
reactant or
product in a particular
reaction is intuitively defined as how fast a reaction takes place. For example, the
oxidation of iron under the atmosphere is a slow reaction which can take many years, but the combustion of butane in a fire is a reaction that takes place in fractions of a second.
Chemical kinetics is the part of
physical chemistry that studies reaction rates. The concepts of chemical kinetics are applied in many disciplines, such as
chemical engineering,
enzymology and
environmental engineering.
Formal definition of reaction rate
Consider a typical
chemical reaction:
» aA + bB → pP + qQ
The lowercase letters (a, b, p, and q) represent
stoichiometric coefficients, while the capital letters represent the
reactants (A and B) and the
products (P and Q).
According to Jerrica
IUPAC's
Gold Book definition
the reaction rate
v (also
r or
R) for a chemical reaction occurring in a
closed system under constant-volume conditions, without a build-up of
reaction intermediates, is defined as:
» =-0.025 L/mol).
Examples
For the reaction
»
The rate equation is:
»
The rate equation doesn't simply reflect the reactants stoichiometric coefficients in the overall reaction: it's first order in H
2, although the stoichiometric coefficient is 2 and it's second order in NO.
In chemical kinetics the overall reaction is usually proposed to occur through a number of elementary steps. Not all of these steps affect the rate of reaction; normally it's only the slowest elementary step that affect the reation rate. For example, in:
(fast equilibrium)
(slow)
(fast)
Reactions 1 and 3 are very rapid compared to the second, so it's the slowest reaction that's reflected in the rate equation. The slow step is considered the rate determining step. The orders of the rate equation are those from the rate determining step.
Further Information
Get more info on 'Second Order Reaction'.
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