A reaction is said to be of third order if the rate is determined by the three terms of concentration variation. To put it another way, the minimum number of molecules required for the reaction is three.
3rd Order Reaction Derivation
Only equations of the 1st order have the exponential decay that leads to a constant of natural time.
A third-order reaction has time dependence expressed as:
Third-order reaction equation:
d[A]/dt = -k[A]^{3}.
This integrates up, to give: T = 1/( 2k[A]^{2}) this is evaluated at the two times in question.
You can see that the time to go to half the concentration depends on the concentration, unlike the case of first order where the time to half the concentration is independent of that.
If the 3rd order reaction has time dependence given by:
d[A]/dt = -k[A] * [B]^{2}
or d[A]/dt = -k[A][B][C]
And[ B] and[ C] are altered only marginally, so you have a pseudo-1st-order reaction which then has a definable half-life.
The reason the 1st order reaction gives a half-life is that when the equation integrates it produces a logarithmic function that produces a quotient when subtracted and the starting quantities cancel by division.
Three different cases may occur in the third-order reaction.
Equal concentrations: The concentrations of all three species are equivalent.
A + A + A → Products
There are two species of equal concentrations, and one with specific.
A + A + B → Products
-dx/dt = k[A]^{2}[B]
Both three species have dissimilar amounts.
A + B + C → Products
-dx/dt = k[A][B][C]
The reaction order is determined from the slowest reaction step.
It is an experimental value
Below are some examples of fractional order:
(i) COCl_{2} → CO + Cl_{2}
rate = k[COCl]^{3/2}
Therefore Order = 3/2 = 1.5
(ii) H_{2} + Br_{2} → 2H Br
Rate = k[H_{2}]^{1}[Br_{2}]^{1/2}
Therefore Order = 1.5
(iii) CH_{3}CHO → CH_{4} + CO
Rate = k[CH_{3}CHO]^{3/2}
Therefore Order = 3/2 = 1.5
Higher - order reactions [ > 3] are very unusual because many molecules have very little chance of experiencing effective collisions.
2O_{3} → 3O_{2}
Rate = k[O_{3}]^{2} ⋅ [O_{2}]^{-1}
Third Order Reaction Examples
Let us understand the nitric oxide-chloride reaction
2 NO +Cl2 → 2 NOCl
Then Rate, R= k[NO]2 [Cl2]
Order of above reaction is equal to addition of exponent of nitric oxide and chloride Order = 2 + 1 = 3.
Let us consider the nitric oxide-oxygen reaction
2 NO + O2 → 2 NO2 R= k[NO]2 [O2]
Therefore Order = 2 + 1 = 3.
1. What is the Rate Law for a Third-Order Reaction?
Ans. Reaction Order and Rate Constant Units
Reaction Order | Units of k |
Zero | mol/L/s |
First | s^{-1} |
Second | L/mol/s |
Third | mol^{-1} L^{2} s^{-1} |
2. Why are Third-Order Reactions Unlikely?
Ans. This type of reaction is very unusual because to create a reaction, all three reactants have to collide with each other simultaneously, with sufficient energy and proper orientation. There are three ways to react to termolecular reactions, and they all come in the third order.
3. How Many Orders of Reaction are There?
Ans. Reaction orders which define their kinetics may be allocated to chemical reactions. Order types are zero-, first-order, second-order, or mixed-order. At a constant rate a zero-order reaction proceeds. A reaction rate at first order depends on the concentration of one of the reactants.