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Chemical Kinetics - Two Marks Study Materials

12th Standard EM

    Reg.No. :


Time : 00:45:00 Hrs
Total Marks : 30
    15 x 2 = 30
  1. Define average rate and instantaneous rate

  2. Define rate law and rate constant

  3. Derive integrated rate law for a zero order reaction A\(\longrightarrow \) product

  4. Define half life of a reaction. Show that for a first order reaction half life is independent of initial concentration

  5. What is an elementary reaction? Give the differences between order and molecularity of a reaction

  6. Explain the rate determining step with an example.

  7. Describe the graphical representation of first order reaction.

  8. Write the rate law for the following reactions.
    (a) A reaction that is 3/2 order in x and zero order in y.
    (b) A reaction that is second order in NO and first order in Br2.

  9. Explain the effect of catalyst on reaction rate with an example

  10. The rate law for a reaction of A, B and C has been found to be rate =k[A]2[B][L]3/2 How would the rate of reaction change when
    (i) Concentration of [L] is quadrupled
    (ii) Concentration of both [A] and [B] are doubled
    (iii) Concentration of [A] is halved
    (iv) Concentration of [A] is reduced to \(\left( 1/3 \right) \) and concentration of [L] is quadrupled.

  11. The reaction A + 2B ⟶ C obeys the rate equation. Rate = \(K{ \left[ A \right] }^{ \frac { 1 }{ 2 } }{ \left[ B \right] }^{ \frac { 3 }{ 2 } }\) What is the order of the reaction?

  12. For the reaction
    Cl2 (g) + 2NO (g) ⟶ 2NOCI(g)
    The rate law is expressed as
    rate = K[Cl2] [NO]2
    What is the overall order of this reaction

  13. Consider the oxidation of nitric oxide to form NO2
    2NO(g) + O2(g) ➝2NO (g)
    (a). Express the rate of the reaction in terms of changes in the concentration of NO,O2 and NO2.
    (b). At a particular instant, when [O2] is decreasing at 0.2 mol L−1s−1 at what rate is [NO2] increasing at that instant?

  14. What is the order with respect to each of the reactant and overall order of the following reactions?
    a) 5Br-(aq)+BrO3-(aq)+6H+(aq) ➝3Br2(l)+3H2O(l)
    The experimental rate law is
    Rate = k [Br−][BrO3][H+]2
    b) CH3CHO(g)\(\overset { \Delta }{ \longrightarrow } \) CH4(g)+CO(g) the experimental rate law is
    Rate =K[CH3CHO]\(\frac{3}{2}\)

  15. The rate of the reaction X+2y⇾ product is 4x10-3 mol L-1S-1, if [X]=[Y]=0.2M and rate constant at 400K is 2x10-2s-1, What is the overall order of the reaction


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