Loyola College Thermodynamics Question Papers

Loyola College M.Sc. Chemistry April 2015 Thermodynamics Question Paper PDF Download

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Loyola College M.Sc. Chemistry April 2008 Thermodynamics Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 51

SECOND SEMESTER – APRIL 2008

CH 2800 – THERMODYNAMICS

 

 

 

Date : 21/04/2008            Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

                                                                      PART – A

Answer all questions.                                      (10 ´ 2 = 20 marks)

 

  1. Show that chemical potential mI = ½p,s,hj
  2. State the thermodynamic condition for a system to be in phase equilibrium.
  3. The density of N2(g) at 273 K and at 1.013 ´ 105 pascal pressure is 1.25g/l. Calculate the fugacity of N2 at 0° C and 100 atm pressure.   (1 atm = 1.013 ´ 105 pascal)
  4. Deduce the expression for the mean activity coefficient (g±) in a terms of molality and activity of the solute for the solution of Ce2(SO4)3.
  5. The dissociation pressure (p) of Ag2O(s) to form Ag(s) and O2(g) is given by the equation

log10P = –   + 3.5 where p is in atmosphere.

Evaluate the decomposition temperature of Ag2O(s).

  1. What is meant by residual entropy?
  2. Deduce the relation between entropy and thermodynamic probability.
  3. Calculate the ratio of translational partition function for He(g) to Ne(g) at 25°C, 1 atm. pressure.
  4. Calculate the number of ways of distributing 5 particles among six energy levels if they obey Pauli’s exclusion principle.
  5. What are macro and microstates?

 

PART – B

Answer any EIGHT questions                                    (5 ´ 8 = 40 marks)

 

  1. Explain how the activity of a system depends on (i) Temperature (ii) pressure
  2. The volume of sodium bromide – water solution as a function of molality (m) at constant temperature and pressure is given by the expression

V = 1003 + 23.2 m + 2.2 m3/2 – 0.18 m2

Determine the partial molal v9olumes of NaBr and H2O for a 0.25 m solution.

  1. Draw the phase diagram of a three component system with two solids (A, B) and liquid (C ),  explain in which both the solids form salt hydrate.

 

 

 

 

 

 

 

 

  1. Derive an expression for for a gas with the equation of state.

where B, C are constants which are functions of temperature only.

  1. Derive Gibb’s-Duhem equation.
  2. Explain how absolute entropy of a gas like Cl2 at 300 K be determine using III law of thermodynamics.
  3. Write Sackukr-Tetrode equation and explain the terms. What is its use?
  4. Evaluate the rotational partition function for CO(g) at 27°

(I = 14.5 ´ 10-47 kg m2).

  1. How is equilibrium constant of a reaction calculated using statistical mechanics.
  2. The electronic ground state of monoatomic gas is four fold degenerate and the first electronic excited state is 400 cm-1 above the ground level. Evaluate the electronic partition function at 2000 K if the first excited state is two fold degenerate.
  3. Derive an expression for (Cv)vib of a gaseous system.
  4. Compare the three statistical distributions and explain.

 

 

PART – C

Answer any FOUR questions.                                                            (4 ´ 10 = 40 marks)

23.(a) Derive any two Maxwell equations.

(b) Draw the phase diagram of a simple eutectic system and explain.

24.(a) Derive expressions for q, DG, DH for isothermal reversible expansion of a

vander Waal’s gas.

(b) The equilibrium constant of a reaction at 273 K is 108 and 106 at 310 K.
Evaluate DH° for the reaction and mention the assumption involved.

  1. Explain how the activity coefficient be evaluated using EMF method with a suitable example.
  2. State the postulates of Maxwell-Boltzmann distribution and deduce an expression for most probable distribution.
  3. Explain Debye’s theory of heat capacity of solids and compare it with other theories.
  4. Explain any two of the following.

(a) Separation of partition function

(b)Statistical formulation of ARRT

(c)Application of Quantum Statistics with reference to thermionic emission

(d)Equipartition principle

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Loyola College B.Sc. Physics Nov 2008 Thermodynamics Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – PHYSICS

CC 08

 

THIRD SEMESTER – November 2008

PH 3503 – THERMODYNAMICS

 

 

 

Date : 08-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

 

SECTION-A

Answer ALL the questions                                               (10×2=20)

 

  1. State the principle of equipartition of energy.
  2. Define Brownian Motion.
  3. Define the heat capacity of a substance.
  4. Given C V of an ideal gas is 2R, where R is the gas constant.

Determine the adiabatic exponent g = C P / CV.

  1. Define intensive variables and give examples.
  2. 6 J of heat is supplied to a system and the internal energy of the

system decreases by 3 J. Find the work done.

  1. Write down the Gibbs – Helmholtz equation.
  2. Define phase transition. Give an example.
  3. Define thermodynamic probability.
  4. State Wein’s displacement law.

 

SECTION-B

Answer Any Four questions.                                            (4×7.5=30)

 

11) (a) Define mean free path. [2]

(b) Obtain an expression for the mean free path. State your

assumptions clearly. [5.5]

12) Explain the process of liquefying hydrogen.

13) From the first law of thermodynamics, obtain the relation:

                                P  P

14) Obtain the Maxwell’s thermodynamic relations.

15) (a) Define microstates and macrostates. [3]

(b) How will you distribute 3 particles among 4 states under

Maxwell-Boltzmann and Bose-Einstein statistics? [4.5]

 

SECTION-C

Answer Any Four questions                                             (4×12.5=50)

 

16) Discuss Langevin’s theory of Brownian motion.

17) (a) Discuss Clement-Desormes method to determine the ratio of

specific heats. [8]

(b) Describe the properties of He I and He II [4.5]

18) (a) Obtain the Clausius inequality. [8.5]

(b) Calculate the entropy change when 5 Kg of water is heated from

to  . Assume that the specific heat capacity has a

Constant value of 4200 J/Kg-K. [4]

19) Explain Joule-Kelvin effect. Obtain an expression for the Joule-Kelvin

coefficient. Discuss the significance of the various terms in it.

20) Obtain the Bose-Einstein distribution for an ideal Bose gas. State the

various assumptions made.

 

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Loyola College B.Sc. Physics April 2009 Thermodynamics Question Paper PDF Download

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         LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – PHYSICS

XC 12

THIRD SEMESTER – April 2009

PH 3503 – THERMODYNAMICS

 

 

 

Date & Time: 05/05/2009 / 1:00 – 4:00  Dept. No.                                                 Max. : 100 Marks

 

 

SECTION – A

Answer all the questions.                                                                    10 × 2 = 20 Marks

 

  1. What do you mean by transport phenomena?
  2. State the law of equipartition of energy in a gas.
  3. What is superfluidity?
  4. Distinguish between isothermal and adiabatic changes.
  5. State first law of thermodynamics.
  6. What do you mean by enthalpy?
  7. Define temperature of inversion. Mention its importance.
  8. State the relation between Gibbs and Helmholtz function.
  9. What is thermodynamic probability?
  10. Define phase space.

SECTION – B

Answer any four questions.                                                               4 × 7.5 = 30 Marks

 

  1. Sketch the Maxwell velocity distribution curve. Describe an experiment to verify Maxwell’s distribution law.
  2. (a) Derive Mayer’s relation.                                                         (5 marks)
    • Calculate the specific heat capacity of air at constant volume if

Cp=961.4Jkg-1 K-1  and density is 1.293kg/m3 at NTP.           (2.5 marks)

  1. Using first law of thermodynamics arrive at the equations for isothermal and adiabatic changes.
  2. (a) Establish Clausius latent heat equation.                                  (4 marks)
    • Calculate the change in entropy when 0.002 kg of water at 273 K is heated to 373 K.Given specific heat capacity of water = 4200Jkg-1 K-1 . (3.5 marks)
  3. Define solar constant. Describe an experiment to determine it. (2 + 5.5 marks)

 

SECTION-C

Answer any four questions.                                                               4×12.5 = 50 Marks

 

  1. Derive an expression for the thermal conductivity of a gas, Explain how the thermal conductivity varies with pressure and temperature.
  2. (a) Describe in detail the Clement and Desormes method of finding the ratio of specific heat capacities of air, giving the simple theory of the method.                      (8.5 marks)
  • Explain Linde’s method of liquefying air. (4 marks)
    1. (a) Discuss the concept of entropy. Find the change in entropy in both reversible and irreversible processes.                                                                    (8.5 marks)

(b)        Derive Clausius inequality relation.                                                    (4 marks)

  1. Derive the Maxwell’s thermodynamic relations.
  2. Establish Maxwell-Boltzman distribution law. Apply it to an ideal monoatomic gas to find the average energy of the molecule. (7.5 + 5 marks)

 

 

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Loyola College B.Sc. Physics Nov 2010 Thermodynamics Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION – PHYSICS

THIRD SEMESTER – NOVEMBER 2010

PH 3505/PH 3503 – THERMODYNAMICS

 

 

 

Date : 02-11-10                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

SECTION – A

Answer ALL the questions                                                                                         (10×2=20)

 

  1. Define the mean free path and the mean free time.
  2. Calculate the r.m.s. velocity for oxygen molecules at . Given mass of

oxygen is 5.31x and the Boltzmann’s constant k= 1.38x J/K.

  1. Write down the equation of state for an ideal gas when it undergoes a (i) reversible isothermal and (ii) adiabatic changes.
  2. What is super fluidity?
  3. The internal energy of an ideal gas does not change with its volume. Why?
  4. State the second law of thermodynamics.
  5. Define the molar heat of transformation and give its unit.
  6. State Ehrenfest’s classification of phase transitions.
  7. Define thermodynamic probability.
  8. Classify the following particles according to the statistics they obey:
  9. i) electrons     ii) photons  iii) protons and   iv) helium-4.

 

SECTION – B

 

Answer Any FOUR the questions                                                                  (4×7.5=30)

 

  1. Obtain the expression for the pressure of an ideal gas, from the kinetic

theory of gases, and hence the ideal equation of state.                                   (5+2.5)

  1. Describe Linde’s process for the liquefaction of air.
  2. a)What are intensive and extensive variables? Give examples.                            (3)
  3. b) Obtain the equation of state for an ideal gas undergoing an adiabatic process. (4.5)
  4. Obtain the following expression for the Joule-Kelvin coefficient,.
  5. a) Define phase space.                                                                                                 (1.5)
  6. b) In how many ways can 3 particles be distributed among 4 states according

to the three statistics.                                                                                         (2+2+2)

SECTION – C

 

Answer Any FOUR questions                                                                             (4×12.5=50)

 

  1. a) What is Brownian motion?                                                                                         (2)
  2.      b) Discuss the Langevin’s theory of Brownian motion.                                               (10.5)
  3. a) Explain Clement and Desormes method for determining.            (9.5)
  4. b) Given = 20.3J/mol.-K and R =8.3J/mol.-K, calculate the ratio

of specific  heats.                                                                                                          (3)

  1. a) Derive the Clausius-Clayperon equation involving the latent heat.                      (6)
  2. b) Derive the Clausius inequality.                      (6.5)
  3. a) Obtain the expression for the change in the entropy of an ideal gas.                      (7.5)
  4. b) One mole of an ideal gas occupies 10 liters of volume at 4 atm.

The gas is heated at constant volume till its pressure is 8atm. Then it is

allowed to expand at constant pressure. If its final volume is 40 liters,

calculate the change in its entropy.

Given = 3 cal/mol-K and R = 2 cal/mole-K.                                                                  (5)

  1. For an ideal Bose gas, obtain the Bose-Einstein distribution for the number of

particles  in each energy level.

 

 

 

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Loyola College B.Sc. Physics April 2011 Thermodynamics Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – PHYSICS

THIRD SEMESTER – APRIL 2011

PH 3505/PH 3503 – THERMODYNAMICS

 

 

 

Date : 25-04-2011              Dept. No.                                                  Max. : 100 Marks

Time : 1:00 – 4:00

 

SECTION – A

Answer ALL the questions                                                                                                 (10×2=20)

 

  1. Give the dimensions of coefficient of viscosity.
  2. State the principle of equipartition of energy.
  3. Define the molar heat capacities for a gas.
  4. Define super fluidity.
  5. 7 J of heat is supplied to a system and the internal energy of the system decreases by 4 J.

Find the work done.

  1. Define enthalpy.
  2. Write down the Gibbs – Helmholtz equation.
  3. What is phase transition? Give an example.
  4. Define thermodynamic probability.
  5. Define Solar constant.

 

SECTION – B

 

Answer Any FOUR the questions                                                                               (4×7.5=30)

 

  1. Obtain the expression for the pressure of an ideal gas, from the kinetic theory of gases,

and hence the ideal  gas equation of state.                                                              (5+2.5)

  1. Explain the process of liquefying hydrogen.
  2. a) State the second law of thermodynamics.
  3. b) From the first law of thermodynamics, obtain the relation:

(2.5+5)

  1. Obtain the Maxwell’s thermodynamic equations.
  2. (a) Define microstates and macro states.

(b) How will you distribute 3 particles among 4 states under Maxwell-Boltzmann,

and Bose-Einstein statistics?                                                                                            (3.5+4)

 

 

 

SECTION – C

 

 

Answer Any Four the questions                                                                                      (4×12.5=50)

 

  1. Obtain the Maxwell’s speed distribution for the molecules of an ideal gas.

 

  1. (a) Discuss Clement-Desormes method to determine the ratio of specific heats.

 

(b) List any two properties of He I and of He II.                                                                     (8.5+4)

 

  1. (a) Obtain the Clausius inequality.

 

(b) One mole of an ideal gas expands isothermally to four times its initial volume.

Calculate the entropy change in terms of  R, the gas constant.                             (8.5+4)

 

  1. a) Explain Joule-Kelvin effect. Obtain an expression for the Joule-Kelvin coefficient.

Discuss the significance of the various terms in it.

 

  1. b) Explain Eherenfest classification of phase transitions.                                     (9+3.5)

 

  1. Derive the Planck’s law of black body radiation from Bose – Einstein statistics.

 

 

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Loyola College B.Sc. Physics April 2012 Thermodynamics Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – PHYSICS

THIRD SEMESTER – APRIL 2012

PH 3505/PH 3503 – THERMODYNAMICS

 

 

 

Date : 26-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

Answer ALL the questions:                                                                                             (10×2=20)

 

  1. Define Brownian Motion.
  2. Give the unit of thermal conductivity.
  3. Write down the equations of state for an ideal gas when it undergoes a

reversible isothermal and adiabatic changes.

  1. Define super fluidity.
  2. Given of an ideal gas is 2R, where R is the gas constant, determine the adiabatic

exponent  .

  1. State the 2nd law of thermodynamics.
  2. Write down the Gibbs – Helmholtz equation.
  3. Define phase transition. Give an example.
  4. Define microstates and macrostates.
  5. Classify the following particles according to the statistics they obey:
  6. i) electrons        ii) photons    iii) protons and        iv) helium-4.

 

PART – B

 

Answer Any FOUR questions:                                                                                  (4×7.5=30)

 

  1. Obtain an expression for the coefficient of thermal conductivity of a gas, on the basis of

kinetic theory of gases.

  1. Describe Linde’s process for the liquefaction of air.
  2. a) Write the first law of thermodynamics. What does it signify?  (2+5.5)
  3. b) One mole of oxygen, initially at 17°C, is adiabatically compressed so that its pressure

becomes 10 times the initial value. Find its final temperature and the work done.

  1. Obtain the Maxwell’s thermodynamic relations.
  2. a) Define thermodynamic probability. (2+5.5)
  3. b) Obtain an expression for the solar constant in terms of the Sun’s

temperature, its radius, the mean Sun-Earth distance etc.

 

 

PART – C

 

Answer Any FOUR questions:                                                                                   (4×12.5=50)

 

  1. Discuss Langevin’s theory of Brownian motion.
  2. a) Discuss Clement-Desormes method to determine the ratio of specific heats.
  3. b) Describe the properties of He I and He II.                                                           (8+4.5)
  4. a) Define reversible and irreversible processes.
  5. b) Obtain the Clausius inequality.                                                                                     (4+8.5)
  6. Explain Joule-Kelvin effect. Obtain an expression for the Joule-Kelvin coefficient.

Discuss the significance of the various terms in it.

  1. Obtain the Maxwell-Boltzmann distribution for an ideal gas.

 

 

 

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Loyola College B.Sc. Physics Nov 2012 Thermodynamics Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – PHYSICS

THIRD SEMESTER – NOVEMBER 2012

PH 3505/3503 – THERMODYNAMICS

 

 

 

Date : 05/11/2012             Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

Answer ALL questions.                                                                                          (10 × 2 = 20 marks)

  1. State the law of equipartition of energy in a gas.
  2. If the density of nitrogen is 1.25g/litre at NTP, calculate the rms velocity of its molecules.
  3. Distinguish between adiabatic and isothermal changes.
  4. What is meant by superfluidity?
  5. Define intensive and extensive variables with examples.
  6. Give Clausius statement of second law of thermodynamics.
  7. Define Helmholtz and Gibbs functions.
  8. What is Joule-Kelvin effect? Give its most important application.
  9. What do you mean by micro and macro states?
  10. What do you understand by black body radiation?

 

PART – B

Answer any FOUR questions.                                                                         (4 × 7.5 = 30 marks)

  1. (a) Define mean free path.     (2)

(b) Derive an expression for the mean free path of molecules in a gas.                              (5.5)

  1. (a) What is the principle involved in the liquefaction of gases?   (2.5)

(b) Explain Linde’s experimental method of liquefying air.                                                  (5)

  1. (a) Write down the coefficient of cubical expansion and compressibility of a gas in

terms of  partial derivatives.                                                                                    (1.5+ 1.5)

(b) Derive the expressions for coefficient of cubical expansion and compressibility

of an ideal gas.                                                                                                             (2+2.5)

  1. (a) Explain the concept of entropy.     (2.5)

(b)  Deduce the expression for the efficiency of the Carnot’s engine with suitable diagram. (5)

  1. (a) Explain the term phase-space.                                                                                         (3)

(b)     Obtain a relation connecting entropy and thermodynamic probability.                        (4.5)

 

PART – C

Answer any FOUR questions:                                                                        (4× 12.5 = 50 marks)

 

  1. (a) What do you understand by transport phenomena?                               (2)

(b) Derive an expression for the viscosity of a gas in terms of mean free path of its molecules.  Discuss the effect of pressure and temperature on coefficient of viscosity.            (7.5+1.5+1.5)

  1. (a) Describe, with experimental arrangement, Clement and Desormes method of determining γ,

the ratio of heat capacities.                                                                                                  (10.5)

(b) Calculate the values of the molar heat capacities of a gas if γ=1.33 and R = 8.31J/mol-K.     (2)

  1. (a) Derive Clausius –Clapeyron’s latent heat equation. (7)

(b) Establish the Clausius inequality for a cyclic process.                                                            (5.5)

  1. (a) Derive an expression for the Joule- Kelvin coefficient and show that it is zero

for an ideal gas.                                                                                                                       (7+3)

(b) Discuss temperature of inversion.                                                                                            (2.5)

  1. (a) Derive Planck’s law of radiation. (8.5)

(b) Hence deduce Wien’s law and Rayleigh – Jeans law for shorter and longer wavelengths.  (2+2)

 

 

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“Loyola College B.Sc. Chemistry April 2008 Thermodynamics Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

GH 13

 

THIRD SEMESTER – APRIL 2008

CH 3504 – THERMODYNAMICS

 

 

 

Date : 07/05/2008                Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A                              (10 x 2 = 20 marks)

Answer ALL the questions.

  1. Define the term state junction.
  2. What is meant by Joule-Thomson effect?
  3. Define the heat of combustion.
  4. What do you understand by enthalpy change of a system?
  5. What is efficiency of a carnot engine?
  6. How is entropy of a system related to its temperature?
  7. State the Law of mass action.
  8. Why are exothermic reactions generally spontaneous?
  9. What are the properties of equilibrium constant?
  10. State the III law of thermodynamics.

PART – B

                                                                        (8 x 5 = 40 marks)

Answer any EIGHT questions.

  1. The van der waals constants a and b for hydrogen in dm3 atm units, are 0.246 and 2.67 x 10-2 respectively. Calculate the inversion temperature of hydrogen. Define Ti.
  2. Derive Kirchoff’s equation.
  3. State and explain the heat capacity of a system. Show that you one mole of an ideal gas           Cp – Cv = R.
  4. State and explain the term bond energy.  Discuss its application.
  5. Define and explain the term heat of neutralization.
  6. Describe in detail the Carnot reversible cycle.
  7. State and explain the II law of thermodynamics.
  8. Derive the Gibbs – Helmholtz equation. Give its application.
  9. Explain the Le-chatelier Principle with an example.
  10. Derive the vant Hoff’s isotherm.
  11. Explain the various forms of equilibrium constants.
  12. Explain the Nernst heat theorm.

PART – C

                                    (4 x 10 = 40 marks)

Answer any FOUR questions.

  1. Explain the postulates and derive the kinetic theory of gases.
  2. a) One mole of naphthalene was burnt in oxygen gas at constant volume to give carbon dioxide gas and liquid water at 250C. The heat evolved was found to be 5138.8 kJ. Calculate the enthalpy of reaction at constant pressure.
  1. b) Explain the term standard heat of formation.
  1. a) Derive the Maxwell’s equation.
  1. b) Derive the equation for entropy of mixing.
  1. Derive the equations and explain the dissociation of ammonia.
  2. a) Derive the relationship between Kp and Kc.
  1. b) Give any two applications of law of mass action.
  1. Explain how the absolute entropy of a substance is determined with the help of third law of thermodynamics.

 

 

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“Loyola College B.Sc. Chemistry April 2009 Thermodynamics Question Paper PDF Download”

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        LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 12

THIRD SEMESTER – April 2009

CH 3504 – THERMODYNAMICS

 

 

 

Date & Time: 05/05/2009 / 9:00 – 12:00  Dept. No.                                                   Max. : 100 Marks

 

 

 

PART – A

Answer ALL questions:                                                                                  10 x 2 = 20     

 

  1. What is Joule Thomson effect?
  2. What are intensive and extensive properties?
  3. Define bond energy. What does a +ve value of bond energy indicate?
  4. Explain heat of transition with a suitable example.
  5. State second law of thermodynamics in any two ways.
  6. Define thermodynamic efficiency. Explain why the efficiency of a heat engine is always less than unity.
  7. State Le chatelier principle.
  8. At a given temperature, the equilibrium constant Kc for the reaction is 4. If the equilibrium concentration of is 0.5 mol lit-1, what is the equilibrium concentration of ?
  9. How would the equilibrium reaction of dissociation of be affected by
  10. addition of b) decreasing the volume of the container
  11. What are the exceptions to the third law of thermodynamics?

 

PART – B

Answer any EIGHT questions:                                                                      8 x 5 = 40

 

  1. Differentiate between reversible and irreversible processes.
  2. What is an adiabatic process? Show that a constant for the reversible adiabatic expansion of an ideal gas.
  3. What is Joule Thomson coefficient? Deduce the relationship between and .
  4. The heat of combustion of carbon monoxide at constant volume at 27oC is -280 KJ. Calculate its heat of combustion at constant pressure. (R=8.314 x 10-3 KJ).
  5. Derive an expression for the entropy change accompanying isothermal expansion of an ideal gas.
  6. What is Gibb’s free energy? How does it vary with temperature and pressure?
  7. Derive an expression for the efficiency of a carnot’s engine working between two temperatures T1 and T2.
  8. State law of mass action. Find expressions for KP and KC for applying the law of mass action.

 

  1. Show that .
  2. Discuss the effect of change of temperature, pressure and concentration, in the contact process of manufacture of sulphuric acid.
  3. The enthalpy of combustion of benzene, carbon and hydrogen are -3267.7 KJ mol-1, -393.5 KJ mol-1 and -286.2 KJ mol-1 Calculate the enthalpy of formation of benzene.
  4. Explain Nernst heat theorem.

 

PART – C

Answer any FOUR questions:                                                                       4 x 10 = 40

 

  1. a) Discuss the variation of a reaction with temperature.
  2. The heat of reaction was found to be -21.976 KJ at 27o What will be the heat of the reaction at 50oC? ()
  3. Explain Hess law of constant heat summation and discuss its applications.
  4. Derive Gibbs – Helmholtz equation and mention its application.
  5. a) Derive the relationship between KP and KC.
  6. Calculate the ratio of KP to KC at 27oC for the reaction .
  7. Derive Vant Hoff equation showing the variation of equilibrium constant with temperature.
  8. a) State the third law of thermodynamics.
  9. b) How is absolute entropy of a substance determined using third law of thermodynamics?

 

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“Loyola College B.Sc. Chemistry Nov 2010 Thermodynamics Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – NOVEMBER 2010

CH 3504 – THERMODYNAMICS

 

 

 

Date : 08-11-10                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

 

Answer ALL questions.                                                                                               (10 x 2 = 20 marks)

 

  1. Define Joule Thomson effect.
  2. Distinguish between the heat capacities Cp and Cv.
  3. Define heat of transition.
  4. What is meant of enthalpy of neutralization?
  5. Distinguish between spontaneous process and non spontaneous process.
  6. Define efficiency.
  7. What is a reversible process?
  8. How are Kp and Kc related?
  9. State Lechatlier-Braun principle.
  10. State II law of thermodynamics.

 

PART – B

Answer any EIGHT questions.                                                                          (8 x 5 = 40 marks)

 

  1. Prove that dP is an exact differential using ideal gas equation.
  2. Derive the relation between the two heat capacities Cp & Cv of an ideal gas.
  3. Calculate the reversible work done by 3 moles of an ideal gas during the expansion

from 1dm3  to  20 dm3  on surroundings at  310K.   Also calculate DE and DH.

  1. State a) Graham’ law of diffusion. b) Dalton’s law.
  2. Describe how enthalpy of neutralization of acid by a base can be determined.
  3. Derive the expression for the efficiency of a Carnot cyclic heat engine working between

two different temperatures.

  1. Prove that mixing up of equal volumes of two ideal gases is a spontaneous process.
  2. Derive any two Maxwell equations.
  3. The standard concentration equilibrium constant Kco for the formation of NH3 at 673K is

0.5.  Find the value of Kpo  if the reaction is   ½ N2 + 3/2 H2 ® NH3.

  1. Derive Kirchoff’s equation.
  2. Derive the Van’t Hoff isotherm.
  3. Explain the Nernst heat theorem.

PART – C

 

Answer ANY FOUR questions.                                                                                (4 x 10 = 40 marks)

 

  1. a) Derive Vander Waal equation of gas. (6)

 

  1. b) What is Joule Thompson coefficient?                         (4)

 

  1. a) State and explain Hess’s law of constant heat of summation with a

suitable example.                                                                                                                  (5)

 

  1. b) Explain bond energy and bond dissociation energy.                         (5)

 

  1. a) Describe the thermodynamic principle of the working refrigerator. (5)

 

  1. b) Derive Gibbs Helmholtz equation.                                                 (5)

 

  1. a) State the Law of mass action and explain.       (5)

 

  1. b) Derive an expression for Kp for PCl5 <═>   PCl3 + Cl2.                                                  (5)

 

  1. a) Apply Lechatlier Principle to N2 + 3H2 2 NH3.                         (5)

 

  1. b) Calculate the equilibrium constant for a equilibrium reaction at 300K

whose  DGo  value at this temperature is 29.29 kJ mol-1.                                                (5)

 

  1. a) State III law of thermodynamics and explain.             (5)

 

  1.       b) How is absolute entropy of a gas determined?                                                                (5)

 

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“Loyola College B.Sc. Chemistry April 2011 Thermodynamics Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – APRIL 2011

CH 3504 – THERMODYNAMICS

 

 

 

Date : 25-04-2011              Dept. No.                                                  Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

    Answer ALL questions                                                                                  (10 × 2 = 20marks)

 

  1. Among the different states of matter, which state has the maximum entropy? Why?

 

  1. State Le Chatlier-Braun principle

 

  1. Why is Cp greater than Cv?

 

  1. Define Joule – Thomson coefficient.

 

  1. Give the units of entropy and enthalpy.

 

  1. If the equilibrium constant is 1000atm for the forward reaction, what will be its value for the backward reaction?

 

  1. Define standard free energy of formation.

 

  1. What is the ΔH value for a strong acid strong base neutralisation reaction?

 

  1. State the II law of Thermodynamics on the basis of Carnot’s cycle.

 

  1. 5moles of an ideal gas expand reversibly from a volume of 8dm3 to 80 dm3 at a temperature of 27◦ Calculate the change in entropy.

 

PART – B

       Answer any EIGHT questions.                                                                   (8 × 5 = 40 marks)   

 

  1. Prove that Cp – Cv = R. (5)

 

  1. Differentiate extensive property from intensive property. (5)

 

  1. Calculate W and ΔU for the conversion of 1mole of water at 100˚C to steam at 1 atm pressure. The heat of vaporisation of water at 100˚C is 40670J/mol.         (5)

 

  1. State Hess’s law of constant heat of summation and explain its application. (2+3)

 

  1. How is the enthalpy of combustion measured? Explain.       (5)

 

  1. (a)Calculate the maximum efficiency of an engine working between 110˚c and 25˚c.

(2)

 

(b)Calculate the entropy change in the melting of 1Kg of ice at 0˚c. Heat of fusion of ice
is 334.72J/g.                                                                                                                            (3)

 

 

  1. Derive the equation for the entropy of mixing of gases.  (5)

 

  1. Derive the relation between ΔA and Wrev.       (5)

 

  1. Derive the relation between Kp and Kc for a reaction.       (5)

 

  1. Explain the effect of pressure and temperature in the formation of ammonia gas

 

from nitrogen and hydrogen.                                                                                                     (5)

 

  1. Calculate Kp at 25˚c and 325˚c for the reaction NO(g) +1/2 O2NO2(g) if at 25˚c

ΔH = -56.48KJ/mol and ΔG = -34.85KJ/mol.                                                                       (5)

 

  1. 22. Derive Kp for the reaction N2O42NO2 (g).                                                                          (5)

 

PART – C

      Answer any FOUR questions.                                                                  (4×10 = 40 marks)

 

  1.   a) Derive Kirchoff’s equation.

 

  1. b) Derive any one Maxwell equation.               (5+5)

 

  1. 24. (a) Calculate the ∆H for the reaction AgNO3 + NaCl →NaNO3 +AgCl.

Given  Ag+(aq)= -105.9KJ/mol, AgCl(s)= -127.0KJ/mol,

Cl–(aq)= -167.5KJ/mol.

 

(b) Differentiate bond energy from bond dissociation energy.                                     (5+5)

 

  1. a) Derive Gibbs Helmholtz equation.                             (6)

 

  1. b) Explain its application.      (4)

 

  1. Derive Clausius- clapeyron equation and explain its application in Liquid Vapour

equilibrium.                                                                                                                             (5+5)

 

  1. Derive van’t Hoff isotherm equation.

Hence deduce an expression for equilibrium constant.                                                   (5+5)

 

  1. (a) State and explain III law of thermodynamics.         (5)

 

(b) How is standard entropy of oxygen gas evaluated?                                                       (5)

 

 

 

 

“Loyola College B.Sc. Chemistry April 2012 Thermodynamics Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – APRIL 2012

CH 3504/CH 3500 – THERMODYNAMICS

 

 

 

Date : 19-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

Answer ALL the questions:                                                                                 (10 x 2 = 20 marks)

  1. What is work function? How is it related with internal energy?
  2. What is meant by Joule-Thomson effect?
  3. Define heat of transition.
  4. What is integral heat of dilution?
  1. Calculate the maximum efficiency of a Carnot engine operating between 27°C

and 127°C.

  1. What is entropy? What are the units of entropy?
  2. State the law of mass action.
  3. Define the term “equilibrium constant”.
  1. State first law of thermodynamics.
  2. Mention the essential conditions for spontaneity in a chemical reaction.

 

PART – B

Answer any EIGHT of the following:                                                                 (8 x 5 = 40 marks)

 

  1. The enthalpy of reaction (DH) for the formation of ammonia N2 + 3H2 ⇌ 2NH3 at 27°C was found to be -94 KJ. What will be the enthalpy of reaction at 50°C. The molar heat capacities at constant pressure at 27°C for N2, H2 and NH3 are 28.45, 28.32 and 37.07 joules respectively.
  2. What are exact differentials? Explain with conditions and examples.
  3. Bring out the relationship between Cp and Cv.
  4. State and explain Hess’s law.
  5. Deduce an expression for the entropy of mixing of ideal gases.
  6. Explain the need for Second law of Thermodynamics.
  7. Explain the postulates of the kinetic theory of gases.
  8. Derive any two Maxwell relations.
  9. For a water gas reaction at 1000 K the standard Gibb’s energy change is

-8.1 kJmol-1. Calculate the value of equilibrium constant.

 

 

  1. Derive the expressions for Kp for decomposition of PCl5.
  2. Predict whether the reaction CO(g)  + H2O(g)   →  CO2(g)  + H2(g) is spontaneous or

not. The standard free energies of formation of CO(g), H2O(g) and CO2(g) are

-137.27, -228.6 and -394.38 kJ mol-1 respectively.

  1. Explain Nernst heat theorem.

 

PART – C

 

Answer any FOUR of the following:                                                                  (4 x 10=40 marks)

 

  1. a) Compare isothermal and adiabatic reversible expansion of ideal gases.
  2. b) Derive an expression for the variation of enthalpy change of reaction with

temperature.

  1. a) Calculate the bond energy of C – H bond in methane from the following data:
  2. C(s) + 2H2(g)   →  CH4(g)    ∆H = -74.8 kJ
  3. H2(g) →  2H(g)                    ∆H = 435.4 kJ

iii. C(s)   →  C(g)                        ∆H = 718.4 kJ

  1. b) How is enthalpy of combustion measured?
  2. a) Describe in details the carnot cycle for establishing the maximum convertibility

of heat into work.

  1. b) Explain the thermodynamic principle of the working of refrigerator.
  2. a) Derive Gibbs-Helmholtz equation.
  3.  b) Discuss the effect of temperature, pressure and concentration on the reaction

for the formation of ammonia.

  1. a) Derive: (i)   Vant Hoff isothrm

(ii)  Van derwual’s equation.

 

  1.    a) State and explain III law of thermodynamics.
  2.     b) How is the standard entropy of oxygen gas evaluated?

 

 

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“Loyola College B.Sc. Chemistry Nov 2012 Thermodynamics Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – NOVEMBER 2012

CH 3504/3500 – THERMODYNAMICS

 

 

Date : 15/11/2012             Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

 

 

PART – A

 

Answer ALL questions:                                                                                           (10 x 2 = 20 marks)

 

  1. Define isothermal and isobaric processes.
  2. Define the adiabatic process.
  3. What is meant by calorific value?
  4. Define heat of transition.
  5. What is the need for the second law of thermodynamics?
  6. Define the term efficiency of an engine.
  7. State the law of mass action.
  8. What is a homogenous mixture?
  9. Give the Van’t Hoffs isotherm. Explain the terms.
  10. What are the exceptions to third law of thermodynamics?

 

PART – B

 

Answer any EIGHT questions:                                                                               (8 x 5 = 40 marks)

 

  1. Derive Vander Walls equation of state.
  2. Compare Wrev and Wirrev.for an isothermal process.
  3. Derive the Kirchoff’s equation.Give its application.
  4. State Hess’s law of constant heat of summation and explain its application.
  5. For a certain gas Cp = 8.58. J mol-1 Two moles of the gas are expanded adiabatically from an initial

temperature of 20oC to  a final temperature of -45.4oC.   Calculate the work done.

  1. Explain the method for the determination of enthalpy of combustion.
  2. Explain the thermodynamic principle of the working of refrigerator.
  3. Derive the equation for the entropy of mixing of gases at constant temperature.
  4. Derive the relationship between Kp and Kc.
  5. Derive Van’t Hoffs isochore.
  6. Discuss the dissociation of ammonia by applying Le-chatlier principle.
  7. Explain the Nernst heat theorem.

 

 

 

PART – C

 

Answer ANY FOUR questions:                                                                                   (4 x 10 = 40 marks)

 

  1. a) Explain the postulates of the kinetic theory of gases. (5)
  2. b) Discuss Joule Thompson effect.                                                                      (5)

 

  1. a) Discuss the thermodynamics of Carnot cycle.                                                (5)
  2. b) Explain the bond energy.                                                                                (5)

 

  1. a) Derive Gibbs Helmholtz equation. (5)
  2. b) Discuss the criteria for spontaneous process.                                                  (5)

 

  1. a) Explain the properties of equilibrium constant. (5)
  2. b) Calculate the equilibrium constant for a equilibrium reaction at 310K

whose  DGo  value at this temperature is  30 kJ mol-1.                                    (5)

 

  1. a) Apply law of mass action for the formation of HI. (5)
  2. b) Explain the factors which alter the state of equilibrium for the above

reaction.                                                                                                          (5)

 

  1. a) Explain Lewis Randall formulation of third law. (5)
  2. b) How will you determine the absolute entropy of oxygen gas?                      (5)

 

 

 

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