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Parallel and Sequential Reactions


Table of Content


Parallel and Sequential  Reactions

Parallel or Competing Reaction 

The reactions in which a substance reacts or decomposes in more than one way are called parallel or side reactions.



If we assume that both  of them are first order, we get.

-\frac{d[A]}{dt} = (k_1 +k_2) [A] =k_{av}[A]

k1 = fractional yield of B × kav

k2 = fractional yield of C × kav

If k1 >  k2 then

A → B main and

Parallel or Competing ReactionA → C is side reaction

Let after a definite interval x mol/litre of B and y mol/litre of C are formed.

\frac{x}{y} =\frac{k_1}{k_2}


\frac{\frac{d[B]}{dt}}{\frac{d[C]}{dt}} =\frac{k_1}{k_2}

This means that irrespective of how much time is elapsed, the ratio of concentration of B to that  of C from the start (assuming no B  and C in the beginning ) is a constant equal to k1/k2.

pLOT FOR Parallel or Competing Reaction

Refer to the following video for parallel reactions:

Example of Parallel Reactions



Consecutive or Sequential  Reactions 

This reaction is defined as that reaction which proceeds from reactants to final products through one or more intermediate stages. The overall reaction is a result of several successive or consecutive steps.

A → B → C and so on

Example of Sequential Reactions

  • Decomposition of ethylene oxide

(CH2)2\overset{k_1}{\rightarrow} CH3CHO

CH3CHO \overset{k_2}{\rightarrow} CO + CH4

  • The pyrolysis of acetone

(CH3)2CO \overset{k_1}{\rightarrow} CH4 + CH2 =C=O                                  

CH2 =C=O \overset{k_2}{\rightarrow} C2H4 + CO

Consecutive or Sequential  Reactions For the reaction


-\frac{d[A]}{dt} = k_1[A]…....(i)

\frac{d[B]}{dt} = k_1[A]-K_2[B]…......(ii)

\frac{d[C]}{dt} = k_2[B]….......(iii)

Integrating equation (i), we get


Now we shall integrate equation (ii) and find the concentration of B related to time t.

Integration of the above equation is not possible as we are not able to separate the two variables, [B] and t. Therefore we multiply equation (4) by an integrating factor e^{-k_1t}, on both the sides of the equation.

Integrating with in the limits 0 to t.

Now in order to find [C], substitute equation (vi) in equation (iii), we get 

Bmax and tmax:     

We can also attempt to find the time when [B] becomes maximum. For this we differentiate equation (vi)  and   find d[B]/dt & equate it to zero.

Substituting  equation (vii)  in equation (vi)

Question 1: 

Parallel  reactions take place in

a. more than one way

b. more than one step

c. in one way but more than one step 

d. in one step but more than one way

Question 2: 

Sequential reactions have 

a. more than one way to proceed toward product 

b. more than one step

c. no intermediate

d. catalyst

Question 3: 

Which one of the following statements is correct?

a. parallel reactions are also known as consecutive reactions

b. Competingreactions  have more than one step

c. Sequential reactions are also called consecutive reactions

d. Consecutive reactions do not have intermediates. 

Question 4: 

Decomposition of ethylene oxide is 

a. parallel reaction

b. competing reaction

c.both parallel as well as competing reaction

d. sequential reaction

Q.1 Q.2 Q.3 Q.4
a b c d

Related Resources

To read more, Buy study materials of Chemical Kinetics comprising study notes, revision notes, video lectures, previous year solved questions etc. Also browse for more study materials on Chemistry here.

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