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Chemical Kinetics 2 Mark Book Back Question Paper With Answer Key

12th Standard

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Chemistry

Time : 00:30:00 Hrs
Total Marks : 26

    2 Marks 

    13 x 2 = 26
  1. Explain the effect of catalyst on reaction rate with an example.

  2. Explain briefly the collision theory of bimolecular reactions.

  3. Write Arrhenius equation and explains the terms involved.

  4. The decomposition of Cl2O7 at 500K in the gas phase to Cl2 and O2 is a first order reaction. After 1 minute at 500K, the pressure of Cl2O7 falls from 0.08 to 0.04 atm. Calculate the rate constant in s-1

  5. A gas phase reaction has energy of activation 200 kJ mol-1. If the frequency factor of the reaction is 1.6 x 1013s-1. Calculate the rate constant at 600 K.(e-40.09 = 3.8 x 10-48)

  6. For the reaction 2x+y ⟶ L find the rate law from the following data. 

    [x]
    (min)
    [y]
    (min)
    rate
    (ms-1)
    0.2 0.02 0.15
    0.4 0.02 0.30
    0.4 0.08 1.20
  7. A zero order reaction is 20% complete in 20 minutes. Calculate the value of the rate constant. In what time will the reaction be 80% complete?

  8. The activation energy of a reaction is 22.5 k Cal mol-1 and the value of rate constant at 40°C is 1.8 x 10-5s-1. Calculate the frequency factor, A.

  9. From the following data, show that the decomposition of hydrogen peroxide is a reaction of the first order:

    t(min) 0 10 20
    V(ml) 46.1 29.8 19.3

    Where t is the time in minutes and V is the volume of standard KMnO4 solution required for titrating the same volume of the reaction mixture.

  10. Consider the oxidation of nitric oxide to form NO2
    2NO(g) + O2(g) ➝2NO2(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?

  11. 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]\(\frac{3}{2}\)

  12. The rate of the reaction X + 2y→ product is 4 x 10-3 mol L-1S-1, if [X] = [Y] = 0.2M and rate constant at 400K is 2 x 10-2s-1, What is the overall order of the reaction.

  13. Rate constant k of a reaction varies with temperature T according to the following Arrhenius equation  \(\log K=\log A-\frac { { E }_{ a } }{ 2.303R } \left( \frac { 1 }{ T } \right) \)Where Ea is the activation energy. When a graph is plotted for log k Vs \(\frac{1}{T}\) a straight line with a slope of -4000K is obtained. Calculate the activation energy.

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