Mechanism of the reaction
(1) Reaction making use of first order consecutive reactions
(i) In this kind of reactions, the reactions from the stable intermediate compound before they are finally converted into products.
(ii) For instance, reactants (R) are first converted to intermediate (I) which is then converted to product (P) as
![787_Mechanism of reaction.png](https://www.expertsmind.com/../CMSImages/787_Mechanism of reaction.png)
Thus, the reaction takes place in two steps, both of which are of the first order that is
Step I : ![781_Mechanism of reaction1.png](https://www.expertsmind.com/../CMSImages/781_Mechanism of reaction1.png)
This means that I is obtained by step I and consumed by step II. In the above given reactions, each stage will have its own rate and rate constant reactant concentration will always decrease and product concentration will always increase as which is shown in figure
![78_Mechanism of reaction2.png](https://www.expertsmind.com/../CMSImages/78_Mechanism of reaction2.png)
(2) Reaction involving slow step : When a reaction occurs by a sequence of steps and one of the step is quite slow, then rate determining step is slow step. For instance in the reaction
; , if k1<<k2 then I is converted into the products as soon as it is formed, we get the conclusion as follows
![1551_Mechanism of reaction4.png](https://www.expertsmind.com/../CMSImages/1551_Mechanism of reaction4.png)
(3) Parallel reactions : In these type of reactions the reactants are more reactive, which can have different orders of the reactions taking place simultaneously. For example, in a system containing NO2 and SO2, NO2 is consumed in the following two reactions,
![894_Mechanism of reaction5.png](https://www.expertsmind.com/CMSImages/894_Mechanism%20of%20reaction5.png)
The rate at which the NO2 disappears will be sum of the rates of the two reactions i.e.,
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