Loyola College M.Sc. Chemistry April 2007 Thermodynamics & Statistical Mechanics Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

LM 34

SECOND SEMESTER – APRIL 2007

CH 2810 – THERMODYNAMICS AND STATISTICAL MECHANICS

 

Date & Time: 21/04/2007 / 1:00 – 4:00    Dept. No.                                            Max. : 100 Marks

 

 

PART A

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

  1. Calculate the fugacity of H2 at 1000C and 300 atm. The density of H2 at the above conditions is 16.79 g dm-3.
  2. Show that mi (Chemical potential) = (dH/dni)P,S,,nj
  3. A 4.84 molal aqueous solution of a non-volatile solute has a vapour pressure of 18.5 mm of

Hg at 250C.  At the same temperature the vapour pressure of the pure water is 23.6 mm of Hg.  Assuming that the water vapour behaves ideally, calculate the activity and the activity coefficient of water (g x) in the given solution.

  1. The equilibrium constant for the reaction, C(s)+CO2(g) Û2CO(g) is 4.28 x 10-3 atm at 1200 K. If the partial pressure of CO2 is 1.2 atm, calculate partial pressure of CO.
  2. What is Onsager theory?
  3. State Sterling’s approximation and hence evaluate ln N!, when N = 1030
  4. What is the significance of partition function?
  5. Using equipartition principle, evaluate CV for PH3(g) if R=2 cal K-1 mol-1.
  6. Calculate the number of ways of distributing three particles among four energy levels if the particles obey Pauli’s exclusion principle.
  7. What is thermionic emission?

 

PART – B

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

  1. Explain the significances of the Ellingham Diagram.

 

  1. Draw and explain the phase diagram of a three component system consisting of two solids (B and C) and water with the formation of a salt hydrate (B.nH2O)

 

  1. Calculate the fugacity of H2 at 200 atm and 300 K if the fugacity at 25 atm and 300 K is 25.2 atm. The van der Waals constants are a=0.245 l2 atm mol-2 and b = 2.67×10-2 l mol-1

 

  1. The dissociation of N2O4(g) takes place according to the equation, N2O4(g) Û 2NO2(g). At 300 K, 0.92 g of N2O4 contained in a flask of 1.64 litre capacity was found to have a total pressure of 137 mm of Hg.  (i) Calculate the degree of dissociation at this temperature and pressure (ii) Calculate the value of KP at the above conditions.

 

  1. Explain the determination of activity coefficient of using solubility product.

 

  1. Write a note on entropy production and entropy flow in the open system using the principles of non-equilibrium thermodynamics.

 

 

  1. Explain how partition functions are separated?

 

  1. Two of the energy levels of a molecule are e1 = 6 x 10-21 J and e2 = 8.4 x 10-21 J, the corresponding degeneracies being g1 = 3, g2=5. What is the ratio of the distribution numbers in an assembly of molecules at 3000 K?
  2. The vibrational frequency of Cl2 molecule is 1.66 x 1013 s-1. Calculate Qvib and the vibrational partition function at 300 K
  3. Compare the three statistical distributions.
  4. Calculate the equilibrium constant for the reaction S2(g) à 2S at 2000 K. The dissociation energy is 429.7 kJ mol-1 and the free energy function at 2000 K for S(g) and S2(g) are – 191.4 and –265.5 J K-1 mol-1.

 

  1. Show that the rotational energy of a diatomic molecule is equal to RT.

 

PART – C

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

  1. a) How will you determine the activity coefficient of the solvent knowing the activity of the solute?                                                                                                                                (5)

 

  1. b) Consider a hypothetical solute in 1 kg of water. The volume V(ml) at 250C  and 1 atm is represented as, V = 1000.38 + 20.563 m2 + 2.024 m22 – 0.24 m23 . Derive the expression for the partial molal volume of the solute and calculate its value at 1 molal solution.                                                                                                                                                                     (5)
  2. a) Explain Lever Rule                                                                                                                   (3)
  3. b) Using the principle of microscopic reversibility, prove the Onsager’s reciprocal relation.                                                                                                                                                             (7)
  4. For the reaction 2HCl(g)+1/2 O2(g) ó   H2O(g) + Cl2(g),     DH0298 K = -57.2 kJ mol-1,

DG0298 K = -38.07 kJ mol-1.  Compute the value of KP at 500 K. CP (HCl) (J K-1 mol-1) =

28.16 + 1.8 x 10-3 T, CP (O2) (J K-1 mol-1) = 25.48 + 13.6 x 10-3 T, CP (H2O) (J K-1 mol-1) =

30.21 + 9.92 x 10-3 T and CP (Cl2) (J K-1 mol-1) = 31.71 + 10.12 x 10-3 T

 

  1. a) Write Sackur-Tetrode equation and explain its significance                                              (5)
  2. b) Show that the translational energy is equal to 3/2 RT.                                                              (5)

 

  1. Explain the salient features of Debye’s theory of heat capacity of solids. Compare it with Einstein’s theory.

 

  1. Explain an two of the following:
  2. a) Statistical formulation of ARRT
  1. Bose-Einstein distribution law
  2. Residual entropy

 

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