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Only a few reactions are simple or straight forward, $i . e .$ purely first, second or third order reactions. But in most of the reactions, the interpretation of variety of data becomes difficult due to several other reactions taking place simultaneously alongwith the main reaction and thus smooth progress of the reaction is disturbed. Such reactions includes the following different types. The reactions in which a substance reacts or decomposes in more than one way, are called parallel or competing or side reaction. The reactions which take place exclusively on the walls of containing vessels are known as surface reactions. The reactions in which the products of chemical change react together to form the original reactants are called reversible reactions or opposing reactions or counter reactions. The reactions which proceeds from reactants to final products through one or more intermediate stages are called consecutive reactions.

The decomposition of NH3 on platinum surface takes place following rate law:

dxdt=KNH3H2-1

 

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Important Questions on Chemical Kinetics

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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
The rate constant for the first order reaction is 60 s-1. How much time will it take to reduce the concentration of the reactant to 116 th value?
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
For a zero - order reaction with rate constant k, the slope of the plot reactant concentration against time is
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
The half-life period of a first-order reaction is 15 minutes. The amount of substance left after one hour will be
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
The rate of a first-order reaction is 0.04 mol l-1s-1 at 10 second and 0.03 mol l-1s-1 at 20 seconds after initiation of the reaction. The half-life period of the reaction is:
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
If 50 % of a reaction occurs in 100 second and 75 % of the reaction occurs in 200 second, the order of this reaction is:
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction

The given plots represent the variation of the concentration of a reactant R with time for two different reactions (i) and (ii). The respective orders of the reaction are
(i) Question Image

(ii) Question Image

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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
A first-order reaction has a specific reaction rate 10-2sec-1⁡. How much time will it take for 20 g the reactant to reduce to 5 g?
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A flask contains a mixture of compounds A and B. Both compounds decompose by first-order kinetics. The half-lives for A and B are 300 s and 180 s, respectively. If the concentrations of A and B are equal initially, the time required for the concentration of A to be four times that of B (in s) is : (Use ln 2=0.693)
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
It takes 1h for a first order reaction to go to 50% completion. The total time required for the same reaction to reach 87.5%  completion will be
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
The rate constant for a first order reaction is 7.0×10-4 s-1. If initial concentration of the reactant is 0.080 M, what is the half-life of the reaction?
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
If the rate constant for a first order reaction is k, the time (t) required for the completion of 99% of the reaction is given by
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
The reaction 2N2O5g→4NO2g+O2(g) follows first order kinetics. The pressure of a vessel containing only N2O5 was found to increase from 50 mm Hg to 87.5 mm Hg in 30 min. The pressure exerted by the gases after 60 min. Will be (Assume temperature remains constant) :
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The rate constant of a first order reaction is 231×10-5 s-1. How long will 4 g of this reactant reduce to 2 g?
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Decomposition of H2O2 follows a first order reaction. In fifty minutes the concentration of H 2 O 2 decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of H2O2 reaches 0.05 M , the rate of formation of O2 will be:
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
It is true that:
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
The half-life for a zero order reaction having 0.02 M initial concentration of reactant is 100 s. The rate constant (in mol L-1s-1) for the reaction is
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The rate constant for a first order reaction is 4.606×10–3 s–1. The time required to reduce 2.0 g of the reactant to 0.2 g is :
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
Under what condition the order of the reaction,

2HI→H2g+I2g, is zero
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
When initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction is:
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Chemistry>Physical Chemistry>Chemical Kinetics>Order of a reaction
The rate constant of the reaction A⟶B is 0.6×10-3 mole per liter per second. If the initial concentration of A is 5 M, then the concentration of B after 20 minutes is: