Quiz  /  Chemical Kinetics Class 12 MCQ Questions With Answers

  • 1. 
    What is the rate law for this mechanism?

  • rate = k[A][B]2
  • rate = [B][X]
  • rate = [A]0.5[B]1.5
  • rate = [W][Y][Z]

  • 2. 
    What is the theory which explains how chemical reaction occurs?

  • Diffusion
  • Big Bang
  • Collusion
  • Evalusion

  • 3. 
    The following data were measured for the reactionBF3(g) + NH3(g) ⟶ F3BNH3(g)What is the rate when [BF3] = 0.100 M and [NH3] = 0.500 M ?

  • .01704 M/s
  • .0852 M/s
  • .1704 M/s
  • .852 M/s

  • 4. 
    A possible rate law for a third overall order of a reaction is __________________

  • Rate = k [A]2[B]2
  • Rate = k [A][B]3
  • Rate = k [A]3 [B]
  • Rate = k [A]2[B]

  • 5. 
    For an elementary reaction 2A + B →C + D, the molecularity is

  • zero
  • one
  • two
  • three

  • 6. 
    The time in which half of the substance has reacted is

  • Half life period
  • Full life time
  • Both 1,2
  • None of the above

  • 7. 
    What letter represents the activation energy?

  • A
  • B
  • C
  • D

  • 8. 
    Consider the following rate law: Rate = k[A]n[B]mHow are the exponents n and m determined?

  • by using balanced chemical equation
  • By using the subscripts for the formulas
  • By educated guess
  • By experiment

  • 9. 
    Given the following rate law, rate = k[A]2[B]if [A] were doubled, what must happen to [B] to keep the rate constant?

  • [B] must quadruple
  • [B] must double
  • [B] must be havled
  • [B] must be quartered

  • 10. 
    Which of the following is NOT a factor affecting reaction rate?

  • temperature
  • catalysts
  • particle size
  • polarity

  • 11. 
    The time taken for 10% completion of a first order reaction is 20 mins .Then for 19% completion ,the reaction will take

  • 50 mins
  • 30 mins
  • 40 mins
  • 60 mins

  • 12. 
    The following data were measured for the reaction BF3(g) + NH3(g) ⟶ F3BNH3(g)What is the rate law for the reaction?

  • rate = k[NH3]
  • rate = k[BF3]2[NH3]
  • rate = k[BF3][NH3]
  • rate = k[BF3][NH3]2

  • 13. 
    Decreasing the particle size increases the reaction rate because

  • It makes particles move faster
  • It increases the likelihood of collisions with the correct geometry
  • It decreases the surface area available to react
  • It increases the number of collisions

  • 14. 
    A first order reaction is 50% completed in 1.26×1014 s .How much time would it take for 100% completion ?

  • 1.26×1015 s
  • 2.52×1014 s
  • 2.52×1028 s
  • infinite

  • 15. 
    Arrhenius equation is

  • k = AeEa/RT
  • k = Ae-Ea/RT
  • k = AeRT/Ea
  • k = Ae-RT/Ea

  • 16. 
    Reaction rate means...

  • amount of product formed
  • speed of reaction
  • concentration of reacting particles
  • combining reactants with products

  • 17. 
    Which of the following best describes why increasing temperature increase reaction rate?

  • Activation energy is reduced.
  • Collisions become more frequent.
  • Collisions become more energetic.
  • Collisions become more frequent and more energetic.

  • 18. 
    Rate = k[A]The rate constant in the rate law above is 0.5 L/mol·s. If the initial concentration of A is 0.1 M, how long will it take for [A] to drop to 0.025 M?

  • 0.7 s
  • 1.4 s
  • 2.8 s
  • There is not enough information given.

  • 19. 
    The catalyst alters the rate of a chemical reaction by,

  • providing an alternative pathway with a lower Ea
  • changing the products formed in the direction of the reaction
  • providing a surface on which the molecules react
  • increasing the frequencies of collisions between molecules

  • 20. 
    Units of rate is _______-

  • M/s
  • mol/s
  • m.s
  • s/M

  • 21. 
    Given the following balanced equation : 2NO(g) + Cl2(g) → 2NOCl(g)If the rate of disappearance of Cl2 is 4.84 x 10-2 Ms-1, what is the rate of disappearance of NO?

  • 1.45 x 10-2 Ms-1
  • 2.42 x 10-2 Ms-1
  • 3.67 x 10-2 Ms-1
  • 9.68 x 10-2 Ms-1

  • 22. 
    Fora reaction,A+B —> Product; the rate law is given by, r =k [ A]1/2 [B]2. What is the order of the reaction?

  • 1
  • 1.5
  • 2
  • 2.5

  • 23. 
    What is the energy needed for reactant particles to change into products?

  • Potential
  • Kinetic
  • Activation
  • Conversion

  • 24. 
    The addition of a catalyst to this reaction would cause a change in which of the indicated energy differences?

  • I
  • II
  • III
  • I and II

  • 25. 
    Which species is the catalyst in this reaction mechanism?

  • R
  • W
  • X
  • There is no catalyst.

  • 26. 
    The iodide ion reacts with hypochlorite ion in the following way:OCl- + I- ⟶ OI- + Cl-.This rapid reaction gives the rate data shown. What is the rate law?

  • rate = [OCl-]2[I-]
  • rate = [OCl-][I-]2
  • rate = [OCl-][I-]
  • rate = [OCl-]

  • 27. 
    Identify the order from the following rate constant : k =9.3×10-3 L mol-1s-1

  • second order
  • first order
  • zero order
  • third order
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