Question Pool Chemical Kinetics

Chemical Kinetics - SAMAGRA Question Pool & Answers | Class 12

Kerala Syllabus SAMAGRA SCERT SAMAGRA Question Pool for Class 12 Chemistry Chemical Kinetics

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Qn 1.

Rate law for the reaction A + 2B ⎯→ C is found to be Rate = k [A][B] Concentration of reactant ‘B’ is doubled, keeping the concentration of ‘A’ constant, the value of rate constant will be______.

(i) the same (ii) doubled (iii) quadrupled (iv) halved



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Qn 2.

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

(i) The order of a reaction can be a fractional number.

(ii) Order of a reaction is experimentally determined quantity.

(iii) The order of a reaction is always equal to the sum of the stoichiometric coefficients of reactants in the balanced chemical equation for a reaction.

(iv) The order of a reaction is the sum of the powers of molar concentration of the reactants in the rate law expression



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Qn 3.

The role of a catalyst is to change ______________.

(i) gibbs energy of reaction. (ii) enthalpy of reaction. (iii) activation energy of reaction. (iv) equilibrium constant



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Qn 4.

The unit of rate constant of a first order reaction is........



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Qn 5.

Write two examples of  zero order reactions?



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Qn 6.

All collisions between reactant species do not lead to th formation of products.why



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Qn 7.

How did you determine the order of a complex reaction ?



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Qn 8.

The equation which gives relation between temperature and rateconstant is ...........



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Qn 9.

1) Find out the order of the reaction from the following rate equation ,R=K [A][B]

2) What is the unit of rate constant



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Qn 10.

Distinguish between order and molecularity?



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Qn 11.

Molecularity greater than three is very rare why?



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Qn 12.

What is a zero order reaction ? Give an example?



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Qn 13.

The rate determining step of a complex reaction is ...........................



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Qn 14.

The rate constant of a reaction is doubled when the temperature is increased from 270C to 370C.Calculate its activation energy?



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Qn 15.

Half life of a firstorder reaction is 10s. Calculate its rate constant?



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Qn 16.

What is half life period? Show that half life of a first order reaction does not depends on the initial concentration?



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Qn 17.

A first order reaction is 90% completed in 20minutes .calculate the rate constant of the reaction?



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Qn 18.

In a reaction A+B-----> C, the rate is doubled when the concentration of A is doubled and the rate is increased to four times when the concentration of B is doubled.Find the rate law and also the order of the reaction?



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Qn 19.

A certain reaction is second order withrepect to the reactant A and first order with respect to B.

1) write the rate equation?

2) what is the overall order?

3) what happens to rate if concentration of both A and B are doubled?



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Qn 20.

If units of rate and rateconstants are same, then order of the reaction is ...............



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Qn 21.

How does the catalyst increase the rate of a chemical reaction?



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Qn 22.

Ester hyrolysis in acid medium is a pseudofirst order reaction .Justify?



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Qn 23.

Order of radioactive disintegration is

      (a)  Zero                    (b) First                  (c) Second                    (d)  Third



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Qn 24.

A catalyst increases the rate of a chemical reaction by

      (a)  increasing the activation energy      (b)  decreasing the activation energy     

      (c)  reacting with reactants                     (d)  reacting with products     



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Qn 25.

Unit of rate constant for zero order reaction is

      (a)   mole L – 1 s – 1     (b)  mole L – 1 s     (c) mole 2 L – 2 s – 1      (d)  s – 1       


 



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Qn 26.

The substance with initial concentration of  ‘a’ mole L – 1 proceeds according to zero order kinetics.

The time it takes for the completion of the reaction is ( k = rate constant).

      (a)  k / a                          (b)  a / k                       (c)   k / 2a                   (d)  a / 2k



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Qn 27.

For the reaction 2 A +  B    →  3 C  +  D, which of the following does not express the reaction rate?

     (a) d[D] / dt               (b) – d[A] / 2dt        (c)  –  d[C] / 3dt          (d)   – d[B] / dt 



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