Integrated Rate Laws
(a) Zero Order Reactions
Examples of zero order reactions:
Generally, decomposition of gases on metal surfaces at high concentrations follow zero order kinetics.
(b) First order Reactions:
First order growth reaction:
For bacterial multiplication of virus growth use following concept
Examples of 1st order reaction:
(c) Second order Reactions:
Second order reaction is determined by the variation of two concentration terms or rate of the reaction is proportional to the second power of the concentration of a single substance.
They are of two types:
1. When the concentration of the reactants is same,
2. When the concentration of the reactants is different,
(d) Pseudo first order reaction:
A second order (or of higher order) reactions can be converted into a first order reaction if the other reactant is taken in large access. Such first order reactions are known as pseudo first order reactions.
For A + B → Products Rate = K[A]1[B]1
Now if 'B' is taken in large access
'b' is very large can be taken as constant
K1 is pseudo first order rate.
K1 will have units of first order.
K will have units of second order.