Reaction rate constant
For a reaction between reactants A and B to form product C
the reaction rate is often found to have the form:
Here k(T) is the reaction rate constant that depends on temperature. [A] and [B] are the concentrations of substance A in moles per volume of solution assuming the reaction is taking place throughout the volume of the solution. (For a reaction taking place at a boundary one would use instead moles of A or B per unit area).
The exponents m and n are called partial orders of reaction and are not generally equal to the stoichiometric coefficients a and b. Instead they depend on the reaction mechanism and can be determined experimentally.
and the reaction rate by
where Ea is the activation energy, and R is the gas constant. Since at temperature T the molecules have energies according to a Boltzmann distribution, one can expect the proportion of collisions with energy greater than Ea to vary with e−Ea/RT. A is the pre-exponential factor, or frequency factor (not to be confused here with the reactant A).
- For order (m + n), the rate coefficient has units of mol1−(m+n)·L(m+n)−1·s−1
- For order zero, the rate coefficient has units of mol·L−1·s−1 (or M·s−1)
- For order one, the rate coefficient has units of s−1
- For order two, the rate coefficient has units of L·mol−1·s−1 (or M−1·s−1)
- And for order three, the rate coefficient has units of L2·mol−2·s−1 (or M−2·s−1)
Plasma and gases
Calculation of rate constants of the processes of generation and relaxation of electronically and vibrationally excited particles are of significant importance. It is used, for example, in the computer simulation of processes in plasma chemistry or microelectronics. First-principle based models should be used for such calculation. It can be done with the help of computer simulation software.
- Blauch, David. "Differential Rate Laws". Chemical Kinetics.
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