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कर्नाटक बोर्ड पी.यू.सी.पीयूसी विज्ञान 2nd PUC Class 12

Why is the probability of reaction with molecularity higher than three very rare?

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प्रश्न

Why is the probability of reaction with molecularity higher than three very rare?

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उत्तर

The probability of more than three molecules colliding simultaneously is very small. Hence possibility of molecularity being three is very low.

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अध्याय 4: Chemical Kinetics - Exercises [पृष्ठ ५६]

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एनसीईआरटी एक्झांप्लर Chemistry Exemplar [English] Class 12
अध्याय 4 Chemical Kinetics
Exercises | Q III. 46. | पृष्ठ ५६

संबंधित प्रश्न

For the first order thermal decomposition reaction, the following data were obtained:

Time / sec               Totalpressure / atm

0                              0.30

300                          0.50

Calculate the rate constant

(Given: log 2 = 0.301, log3 = 0.4771, log 4 = 0.6021)


The conversion of molecules X to Y follows second order kinetics. If concentration of X is increased to three times how will it affect the rate of formation of Y?


From the rate expression for the following reaction, determine the order of reaction and the dimension of the rate constant.

\[\ce{3NO_{(g)} -> N2O_{(g)}}\] Rate = k[NO]2


A reaction is first order in A and second order in B. How is the rate affected when the concentrations of both A and B are doubled?


Define the following term:

Pseudo first-order reaction


Molecularity of a reaction _____________.


Consider a first order gas phase decomposition reaction given below :
\[\ce{A(g) -> B(g) + C(g)}\]
The initial pressure of the system before decomposition of A was pi. After lapse of time ‘t’, total pressure of the system increased by x units and became ‘pt’ The rate constant k for the reaction is given as ______.


Which of the following statements is not correct about order of a reaction.


Compounds ‘A’ and ‘B’ react according to the following chemical equation.
\[\ce{A(g) + 2B(g) -> 2C(g)}\]
Concentration of either ‘A’ or ‘B’ were changed keeping the concentrations of one of the reactants constant and rates were measured as a function of initial concentration. Following results were obtained. Choose the correct option for the rate equations for this reaction.

Experiment Initial
concentration
of [A]/mol L–¹
Initial
concentration
of [B]/mol L–¹
Initial rate of
formation of
[C]/mol L–¹ s–¹
1. 0.30 0.30 0.10
2. 0.30 0.60 0.40
3. 0.60 0.30 0.20

Why can’t molecularity of any reaction be equal to zero?


Why molecularity is applicable only for elementary reactions and order is applicable for elementary as well as complex reactions?


Use Molecular Orbital theory to determine the bond order in each of species, [He2j+ and [He2]2+?


A catalyst in a reaction changes which of the following?


The role of a catalyst is to change


In the presence of a catalyst, the heat evolved or absorbed during the reaction.


The number of molecules of the reactants taking part in a single step of the reaction is indicative of ______.


Identify the order of reaction from the following unit for its rate constant:

L mol–1 s–1


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)


Assertion (A): Order of reaction is applicable to elementary as well as complex reactions.

Reason (R): For a complex reaction, molecularity has no meaning.


A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is reduced to half?


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