Loyola College M.Sc. Chemistry April 2007 Chemical Kinetics Question Paper PDF Download

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LM 53

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

FOURTH SEMESTER – APRIL 2007

CH :4807– CHEMICAL KINETICS

 

 

 

Date & Time : 16.04.2007/9.00-12.00      Dept. No.                                                      Max. : 100 Marks

 

 

Part A

 

Answer ALL the questions.                                                    (10 x 2 = 20 Marks)

  1. Explain electrostriction.
  2. The rate of a reaction between X and Y– has been investigated in aqueous solution at 300 K and the second order rate constant (k20 ) at zero ionic strength is found to be 0.681 M-1 s-1. When ionic strength of the medium (m) is 1.60 x 10-3 M,  the second order rate constant (k2) is 0.901 M-1 s-1.  Predict the charge on X.
  3. Show that collision theory of activation is less than the energy of activation calculated using the Arrhenius equation.
  4. Write down the expression for the rate constant of a reaction between two linear molecules forming a non-linear transition state on the basis of ARRT.
  5. The pKa for the dissociation of phenol in water at 250C is 9.85. The r value for the dissociation H2O + X-C6H4OH à X-C6H4O– + H3O+ is 2.00. If  s–p values of –CH3 is –0.31, determine pKa for the dissociation of p-methyl phenol in water at this temperature.
  6. What are Skrabal plots?
  7. For the reaction 2NO(g) + O2(g) à2NO2(g), the observed rate of the reaction decreases with increase in temperature.
  8. What is the significance of “Hammett acidity functions”??
  9. In a typical Stern-Volmer plot graph of F0/F (Y-axis) versus the concentration of quencher gave a straight line with slope = 640 l/mol and the rate constant of quenching is 1010 l mol-1 s-1. Calculate the Stern-Volmer constant and the life time.
  10. Mention any four relaxation techniques employed for the study of kinetics of fast reactions.

PART – B

 

Answer ANY EIGHT questions                                            (8 x 5 = 40 Marks)

 

  1. Using the Collision theory of reaction rates, derive the expression for the Collision number between two different molecules A and B
  2. Calculate the rotational partition function for CO2 in the standard state of 103 mol m-3 at 250  The carbon-oxygen distance is 1.16 x 10-10 m
  3. Explain the need for activation energy based upon potential energy surfaces.
  4. If the rate constant at high pressures for the isomerization of cyclopropane is 2 x 10-4 s-1 and that at low pressures is 5.14 x 10-6 torr-1 s-1, below what pressure will the isomerization be for all practical purposes a second order  reaction?
  5. Discus the double-sphere model for the influence of dielectric constant on the rate of an ion-ion reaction
  6. Heckt and Conrad measured the rate constant (k2) of the reaction of methyl iodide and sodium ethoxide in ethanol as 2.45 x 10-4 M-1 s-1 at 285 K.  If Ea = 85.20 kJ/mol.  Calculate DG#, DH# and DS# of the reaction.   (kB=1.37 x 10-23 J molecule-1)
  7. How is surface area of a solid deermined using BET equation.
  8. For an enzyme catalyzed reaction, KM = 25 x 10-3 Calculate the rate of the reaction if the limiting rate is 0.64 M s-1 and the  the initial substrate concentration of 4.32 x 10-6 M.
  9. Represent all the possible steps in a bimolecular photophysical process. Indicate the rate expression for each step.
  10. For the following parallel first order reaction,  the rate constants of the two parallel paths are 3.75 and 4.65 s-1  Calculate the percentage yield of B and also the overall half life of the reaction.                 B

A

C

  1. Discuss the principle of flash photolysis.
  2. Explain Bronsted catalytic law.

 

PART – C

Answer ANY FOUR questions                                              (4 x 10 = 40 Marks)

 

  1. a) How will you determine the order of a reaction using dimensionless parameters?
  2. b) The volume of activation for a certain reaction is – 4 x 10-6 m3 mol-1 at 300 K.  Calculate the pressure required to double the rate constant if the initial pressure is 105
  3. a) Calculate the number of collisions per second in 1 cm3 of oxygen at  270C and 101.3 kPa pressure given the molecular radius of oxygen to be 1.46 x 10-8 cm
  4. b) Explain the influence of internal pressure on the rate of a reaction between neutral molecules in solutions
  5. Explain the kinetics of bimolecular surface reactions with a specific example. Derive the relevant rate law for each mechanism.
  6. Explain any two of the following: a) Evaluation of kinetic parameters for an enzymatic reaction b) kinetics of chain reactions  c) van’ Hoff intermediates
    1. a) Derive an expression for relaxation time for a I order reaction.
    2. b) Outline the salient features of the kinetics of explosive reactions.
    3. For the oxidation of aresenous acid by enneamolbdomanganate (IV) in perchloric acid medium, the following data were obtained: (i) Under constant [HClO4], the second order rate constants were fairly constant. (ii) Presence of acrylonitrile  has no effect on the rate of the reaction (iii) It was found that the graph of kobs against [H+]2 was found to be curved passing through origin  (iv) The rate of the reaction was found to be unaffected by the increase of the ionic strength of the medium (vi) The entropy of activation was –5 J K-1 mol-1.  Propose a suitable mechanism to account for the above data, write the rate expression, and explain your answer.

 

 

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