M.Sc Chemistry Thermodynamics & Statistical Mechanics Question Paper 2009

Loyola College M.Sc. Chemistry April 2009 Thermodynamics & Statistical Mechanics Question Paper PDF Download

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WD 33

     LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

SECOND SEMESTER – April 2009

          CH 2816 / 2810 / 2800 – THERMODYNAMICS AND STATISTICAL MECHANICS

 

 

 

Date & Time: 24/04/2009 / 1:00 – 4:00  Dept. No.                                                   Max. : 100 Marks

 

 

PART A

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

  1. How does chemical potential vary with pressure?
  2. State any one of the formulations of Konowaloff’s rule.
  3. For the reaction, NH4HS(s) = NH3(g) + H2S(g), the equilibrium pressure at 298 K was found to be 0.67 atm.  Calculate KP of the reaction at 298 K.
  4. The vapour pressures of pure A and B at 250C are 250 mm of Hg and 400 mm of Hg respectively. A solution in which the mole fraction of A is 0.7 has a vapour pressure of 100 mm of Hg at 250 Calculate the activity coefficient (gx) of A in the given solution.
  5. Give the basic postulates of irreversible thermodynamics.
  6. What is Stirling’s approximation? Evaluate ln N! when N = 1040
  7. Calculate the number of ways of distributing 5 particles among 6 energy levels if the particles are a ) electrons b) Bosons
  8. What is the approximate value of ∆So for the reaction,  35Cl35Cl(g) + 37Cl37Cl(g) à  2 35Cl37Cl assuming that any difference in the molar masses, moments of inertia and vibrational energy levels are negligible for the isotopes?
  9. A system consisting of two energy states separated by 2×10-23 J has a ratio of particles in each state of 51/49, what is the temperature of the system?
  10. “Einstein’s introduction of quantisation accounted for the heat capacity of solids at room temperatures.” Explain.

 

PART – B

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

  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).
  2. A 1:2 salt has a solubility of 1.545 x 10-5 moles lit-1 at 250 Calculate its mean ionic activity coefficient (a) in the absence of any electrolyte and  b) in the presence of 0.01 M BaCl2.
  3. The dissociation of N2O4(g) takes place according to the equation, N2O4(g) Û 2NO2(g). 548 g of N2O4 when heated was found to occupy a volume of 600 ml at 323 K and at a pressure of 850 mm of Hg.  Calculate the value of KP at the above conditions.
  4. Explain the entropy production when current is flowing through a wire.
  5. Show that the phenomenological coefficients must satisfy the following conditions:

L11>0, L22>0 and (L12 + L21)2 < 4 L11 L22

 

  1. Calculate the fugacity of H2 at 1000C and at 300 atm for a van der Waals gas. (a=0.2244 dm6 atm mol-2,

b = 0.0266 dm3 mol-1 and V = 0.119 dm3 mol-1 )

  1. Derive an expression for molecular translational partition function.
  2. Calculate the value of molecular vibrational partition function for N3(g) at 298 K. w1 = 1800 cm-1, w2 = 500 cm-1, g2 = 2 and w3 = 1200 cm-1.
  3. Calculate the rotational contribution to entropy for O2(g) at 250 C( I = 1.937 x 10-46 kg m2)
  4. Compare Debye’s theory of heat capacity of solids with Einstein’s theory.
  5. Calculate the equilibrium constant for the reaction C6H5CH2CH3 ó C6H5CH=CH2 + H2 at 500 K from the following data:  G0-H0/T for         H2 is -27.947 cal K-1 mole-1, for styrene    – 74.44 cal K-1 mole-1 and for ethyl bnzene – 79.64 cal K-1 mole-1.  (∆H0f)0 for Styrene and ethyl benzene are 40.34 and 13.917 k cal/ mol respectively.
  6. Write Sackur-Tetrode equation and deduce the factors affecting Stransl.

PART – C

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

  1. a) Derive Gibbs-Duhem equations.                                                                     (6)
  2. b) When a solute is dissolved in 1 Kg of water, the volume V(ml) at 250C and 1 atm is represented as, V = 1000.3 + 20.7 m2 + 2.5 m22. Calculate the partial molal volume of the solute and that of the solvent in 1 molal solution.                                              (5)
  3. a) A gas obeys the equation of state P(V-b)=RT. For this gas b = 0.0391 dm3 mol-1. Calculate the fugacity coefficient at 1000 K and 100 atm pressure.                                      (3)
  4. b) How is Onsager’s reciprocal relationship verified experimentally by thermoelectric method?                                                                                                                      (7)
  5. For the reaction H2S(g)+3/2 O2(g) ó H2O(g) + SO2(g),     DH0298 K = -518.62 kJ mol-1,            DG0298 K = -495.95 kJ mol-1.  Compute the value of KP at 773 K from the CP data in J K-1 mol-1  CP (H2S) = 26.722 + 23.87 x 10-3 T, CP (O2)= 25.51 + 13.62 x 10-3 T, CP (H2O) = 30.21 + 9.93 x 10-3             T and CP (SO2) = 25.72 + 57.92 x 10-3 T
  6. a) Explain the theory of reaction rates using statistical mechanics. (5)
  7. b) Derive an expression for Evib for a harmonic oscillator and show that it reduces to RT at moderate temperatures                                                                                                            (5)
  8. Derive Fermi-Dirac distribution law and show that the Maxwell-Boltzmann distribution law is the classical limit of Fermi-Dirac distribution law             (6+4)
  9. a) Deduce the equation of state for 1 mole of an ideal gas using the definition of partition function and its relation to pressure of the gas                         (6)
  10. b) Explain the properties of liquid helium using the appropriate statistical distribution.(4)

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