Table of Content
Definition What is a Reaction Mechanism? Complex Reaction Approximation Equilibrium ApproximationSteady State Approximation
What is the Steady State Approximation?
Steady-State Approximation which is also called the quasi-steady-state approximation consists of the assumption that the rates of changes in the concentration of all reactive intermediates are negligibly small. This is generally a good approximation if the concentrations of the intermediates are small since small variables have small time derivatives if they do not oscillate rapidly.
Chemical kinetics, involving the study of the rate of a reaction and rate law, is a very important part of physical chemistry. Knowledge of free energy changes involved in a given process tells us whether the process will occur or not.
But to decide the speed of a reaction, we need the help of chemical kinetics and rate law. The steady-state approximation technique is used to decide the exact rate of a reaction.
What is a Reaction Mechanism?
The mechanism of a reaction is the explanation of how a reaction takes place. For example, we might find out which bonds are broken, what happens in the transition state, and whether the reaction takes place in one or more than one stages. Often it is possible to think of several mechanisms for a single reaction.
Working out a mechanism for a reaction can be very challenging, and fascinating. A reaction that appears straightforward from its chemical equation may have a very complex mechanism.
For example,
CH3COCH3 + I2 → CH3COCH3 + HI
The equation actually shows that one mole of propanone will react with one mole of Iodine to give one mole of iodopropane. But, this actually involves a very complex three-step mechanism.
By looking at the reaction, we will not be able to decide the rate of the reaction.
The chemical equation tells us nothing definite about the rate or mechanism of a reaction. It is also seen that, when the rate is decided, it is not always that the three steps leading to the reaction take place at the same rate. One step may be very fast, while the other may take a much longer time to complete. So, “The slowest step in a reaction determines the rate of the reaction.”
Each step in a chemical reaction is called an elementary step. The rate law of a reaction is determined by the rate-determining step, so there may be substances in the elementary step, that do not appear in the rate law. Also, many substances may be made and used during the course of the reaction. These compounds, which appear in between the reaction, are intermediates.
- Intermediates are a structure formed in one elementary step but consumed during a later step of the mechanism.
- These intermediates, or change in the intermediates, though the reaction is actually not taken into account, when writing the rate law.
- Steady-state approximation deals with the fact that there is no change in state variables, like entropy, temperature, pressure etc, in the intermediate step.
- So, the steady-state approximation actually deals with the fact that the change in the intermediates does not affect the rate of a reaction. It is very important to keep in mind that a balanced chemical equation and a reaction mechanism are two different expressions.
- A rate law can be written from a mechanism, never from a balanced chemical equation. Because many reaction pathways occur very rapidly, it can be difficult to determine mechanisms.
- So, when an intermediate is formed in a reaction, it is consumed immediately. Thus, it does not affect the rate of the reaction. Therefore, it is not necessary to take this into account in the rate law.
Approximations for Complex Reactions
After a reaction has been found complex, we always look into the kinetic data, and a mechanism is suggested for a complex reaction.
In dealing with the progress and mechanism of a chemical reaction, we come across many concepts like reaction coordinate and activated complex. A reaction coordinate is defined as a function of all the coordinates in the space of all species taking part in a reaction. It is a measure of the progress of a given reaction along the path of minimum potential energy at any instant, beginning with the reactant molecules and terminating the product molecules. At a point where the reaction coordinate has the maximum potential energy, is located the activated complex.
At this point, the atoms of the reactants have a configuration of maximum energy of mutual repulsion. Two approximations are generally used for elucidating the mechanism of a complex reaction. These are
- Equilibrium approximation
- Steady-state approximation
Equilibrium Approximation
Consider a reaction in which reactant R changes to the product, p through the formation of a series of consecutive intermediates, I1, I2, I3 ……….In, as follows.
Reactants I1 → I2 → I3……..In
The whole reaction sequence may be described in terms of a single coordinate composing the coordinates of the individual steps.
In order to derive the rate equation for the reaction, we assume that the rate-determining step exists. This rate-determining step is the slowest in a sequence of steps. It is further assumed that all the steps preceding the rate-determining step are in equilibrium.
Steady-State Approximation
In cases where the reactants are investigated under such conditions that the slowest rate-determining step does not exist, one assumes the steady-state approximation, for the transient, or short-lived, intermediate species.
Reactants I1 → I2 → I3……..In
The rate of formation of an intermediate is equal to the rate of its decomposition so that
Steady-state approximation is used to check the consistency of the rate law.
