B.Sc. Chemistry Question paper

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

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SIXTH SEMESTER – APRIL 2011

CH 6606/CH 6600 – MOLECULAR DYNAMICS

 

 

 

Date : 05-04-2011              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

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

 

  1. Define the terms orbit and orbitals.
  2. Calculate the energy of the photon associated with light of wavelength 4000 Ao.
  3. Define the term degeneracy of an energy level.
  4. What are operators? Give an example.
  5. Find the value of ln100!
  6. Define thermodynamic probability.
  7. What is internal conversion?
  8. What is quantum yield?
  9. What are thermal reactions? Give an example.
  10. What is Photosensitization?

 

PART – B

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

 

  1. How is photoelectric effect explained by quantum theory.
  2. Explain the energy distribution in Black Body radiation.
  3. Explain Zeeman effect.
  4. State the postulates of quantum mechanics.
  5. Derive on Schrodinger wave equation.
  6. Explain Sackur-Tetrode equation.
  7. Explain the relation between partition function and energy.
  8. Explain the mechanism of photosynthesis.
  9. Explain the primary and secondary processes in a photochemical reaction.
  10. When irradiated with light of 5000 Ao wavelength, 1 x 10-4 mole of a substance is

decomposed.  How many photons are absorbed during the reaction if its quantum

efficiency is 10.00 (Avogadro number N = 6.02 x 1023)

  1. Explain Flash photolysis.
  2. Discuss the kinetics of photochemical reaction between H2 and Cl2.

 

 

 

PART – C

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

 

  1. (i) Derive an expression for energy of an electron using Bohr’s theory.

(ii) State Pauli’s exclusion principle and explain.

 

  1. (i) What is the minimum energy that photons must possess in order to produce

photoelectric effect with platinum metal?  The threshold frequency for platinum

is  1.3 x 1015 sec-1.

 

(ii)   Derive the expressions for eigen value and eigen function for a particle in one

dimensional box.

 

  1. Derive an expression for translation partition function. Mention its significance.                         (7+3)

 

  1. Derive Maxwell-Boltzmann statistics. Give its application.                                                            (7+3)

 

  1. Explain any two of the following:

(i)    Actinometers                                              (ii)    Phosphorescence

(iii)  Chemiluminescence                         (iv)   Radiationless  transition                             (5+5)

 

  1. a) Derive Stern-Volmer equation.

 

  1. b) Explain Jablonski diagram.                                                                                                         (5 +5)

 

 

 

Go To Main Page

 

“Loyola College B.Sc. Chemistry April 2011 Main Group Elements & Solid State Chemistry Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – APRIL 2011

CH 3503/CH 4501 – MAIN GROUP ELEMENTS & SOLID STATE CHEMISTRY

 

 

 

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

Time : 1:00 – 4:00

 

PART –A

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

 

  1. Give the carbonates and bicarbonates of sodium. Mention their uses.
  2. Explain the reaction of alkali metals with water with an example.
  3. Define catenation.
  4. Name any two types of glass. Give an example.
  5. What is superphosphate of lime?
  6. List the oxyacids of nitrogen and phosphorous.
  7. Draw the structure of BrF3.
  8. What are pseudohalogens? Give an example
  9. What are the coordination number of Na and Cl in Sodium Chloride?
  10. What are Miller indices?

 

PART – B

 

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

 

  1. Discuss the biological importance of alkali metals.
  2. How is beryllium extracted from its ore?
  3. Explain the reaction of Boron with oxygen?
  4. Discuss the bonding in diborane.                                              (2 +3)
  5. How are carbides classified?

15 Give the properties and uses of a) Phosphine   b) hydroxylamine.

  1. Discuss the preparation and properties of Caro’s and Marshall’s acid.
  2. Discuss the oxides of nitrogen.
  3. How is available chlorine in bleaching powder determined?
  4. Discuss the strength of oxoacids of halogens.
  5. Explain the Schottky and Frenkel defects of crystals.

21 Explain limiting radius ratio. How is it used to determine the geometry of ionic crystals?

  1. Draw the unit cells of sodium chloride and Zinc blende. Give their salient features.

 

 

PART –C

Answer any FOUR questions                                                                                    (4 x 10 = 40 marks)

 

  1. Give a comparative account of oxides, hydroxides, and hydrides of alkali metals.
  2. What are silicates? How are they classified?
  3. Write a note on acidic, basic, amphoteric and neutral oxides.
  4. a) How is ozone prepared? Discuss it structure and uses.
  5. b) How does aluminum react with dilute HCl and NaOH solutions.
  6. Discuss the structure of a.BrF5 b. ClF3     c. ICl   d. IF3   using VSEPR theory.
  7. How is X-ray diffraction technique used to study the structure of crystals?

 

 

Go To Main Page

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

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SIXTH SEMESTER – APRIL 2011

CH 6611/CH 6605 – INDUSTRIAL CHEMISTRY

 

 

 

Date : 11-04-2011              Dept. No.                                                    Max. : 100 Marks

Time : 1:00 – 4:00

PART – A

 

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

  1. Explain the characteristics of anthracite coal.
  2. How is hydrodesulphurisation carried out?
  3.  What are plant micronutrients?
  4. Give the preparation of Bordeaux mixture.
  1. Define break point chlorination.
  2. Mention the units in which hardness of water expressed.
  3. Where do good ozone and bad ozone occur?
  4. What is the role of Cotrell’s precipitator in controlling air pollution?
  5. What are acid refractories?
  6. Define flash point of a lubricant.

PART – B

 

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

  1. Define the term Octane number. How is it related to the structure of the molecules?
  2. Describe the method of determination of calorific value of a fuel.
  3. How is saccharin synthesised?
  4. Describe the manufacture of 2,4 D.
  5. Explain the principle and method of determination of temporary hardness of water by EDTA method.
  6. How is water softening achieved by ion exchange process?
  7. Describe the process of desalination.
  8. What is enhanced green house effect? Compare the green house effect potentials of

different green house gases.

  1. Explain the biochemical action of cyanide.
  2. Discuss the effect of acid rain on plants and sea organisms.
  3. What are primary and secondary explosives? Give an example for each.
  4. What are abrasives? How is boron carbide prepared?

 

 

PART – C

Answer any FOUR questions                                                       (4 x 10 = 40 marks)

  1. What is meant by cracking? How is fluidised bed catalytic cracking carried out?

24.a. How is Gobar gas produced? Explain. (5)

  1. How is triple superphosphate prepared? (5)
  2. Describe the process of conversion of molasses into ethanol by fermentation.
  3. Explain in detail various steps involved in the treatment of wastewater.
  4. Define biochemical oxygen demand. How is BOD5 of a wastewater sample determined?
  5. a. Mention the purpose of adding plasticizer and stabilizer to plastics. (5)
  6. How is Portland cement manufactured? (5)

Go To Main Page

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

“Loyola College B.Sc. Chemistry April 2011 Hydrocarbons And Stereochemistry Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SECOND SEMESTER – APRIL 2011

CH 2504/CH 2502/CH 2500 – HYDROCARBONS AND STEREOCHEMISTRY

 

 

 

Date : 08-04-2011              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

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

 

  1. Prove that naphthalene is aromatic using Huckel’s rule.
  2. Draw the structure corresponding to the following IUPAC name.

     Hex-3-ene-5-yne.

  1. What happens when ethyl chloride is treated with sodium metal?
  2. How does cyclopropane react with HI.

     Write the product formed.

  1. What is saytzeff’s rule?
  2. Write the products obtained when propyne reacts with NaNH2.
  3. Complete the following reactions.

       

 

  1. Explain why phenol is nitrated more readily than benzene.
  2. Assign E or Z configuration to each of the following compounds.
  3.           ii.

                            

 

  1. What is meant by 1,3 diaxial interaction in methyl cyclohexane?

 

PART – B

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

 

  1. Explain why benzyl carbonium ion is more stable than ethyl carbonium ion.
  2. What is Hybridization?Explain why four covalent bonds in methane are equivalent.
  3. Explain the free radical mechanism of chlorination of methane.
  4. What is meant by Anti Markonikov addition. Give its mechanism.
  5. What is hydroboration?Explain with an example.
  6. How will you synthesize 1,3 butadiene from 1-butene.
  7. Discuss the molecular orbital structure of benzene.
  8. Although chlorine atom is an electron withdrawing group,it is ortho-para directing

     group.  Explain.

 

 

 

  1. Explain Haworth’s synthesis of Naphthalene.
  2. Define geometrical isomerism.Describe any one method of distinguishing between cis and

      trans isomers.

  1. Discuss the relative stabilities of chair and boat conformations of cyclohexane.
  2. Explain Baeyer’s strain theory?Why is it not applicable to cyclohexane.

 

PART – C

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

 

  1. a) Explain resonance with suitable examples.  (4)
  2. b) Describe homolytic and heterolytic fission of a covalent bond.How carbonium ions,

          carbanions and free radicals are obtained.                                                                                 (6)

 

  1. a) How will you synthesize cyclopentane using Dieckmann’s synthesis.       (4)
  2. b) What is refining of petroleum?What different fractions are obtained on refining. (6)
  3. Predict the products of the following reactions.   (10)                                                              

                 

             

 

  1. a) Write a note on “stability of conjugated dienes”. (5)
  2. b) Explain the mechanism of Nitration of benzene.       (5)
  3. a) Explain Diel’s Alder reaction using suitable examples.       (4)
  4. b) Predict the products of the following reactions.                                                                       (6)

 

       

 

  1. Explain the various conformations of n-butane and discuss their stabilities based on the

      energy diagram.                                                                                                                                (10)

 

 

 

Go To Main Page

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

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FOURTH SEMESTER – APRIL 2011

CH 4502 – ELECTROCHEMISTRY

 

 

Date : 07-04-2011              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

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

 

  1. Define electromotive force.
  2. What is a reversible cell.
  3. Write the relationship between ΔG and  EMF.
  4. What are fuel cells? Give its application.
  5. State Faraday’s law of electrolysis.
  6. Define ionic mobility.
  7. What is cell constant?
  8. Define Solubility Product.
  9. What is meant by decomposition potential.
  10. Write down the Ilkovic equation and mention the terms involved in it.

 

PART – B

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

  1. What is meant by single electrode potential? How could you measure the single electrode potential?
  2. Describe the construction and working of Weston cell.
  3. What is the potential of a half-cell consisting of zinc electrode in 0.01M ZnSO4 solution at

25oC, Eored = -0.763 V.

  1. Explain liquid junction potential. How does it affect EMF measurements?
  2. Derive Nernst equation for electrode potentials.
  3. Explain redox potentiometric  titration with an example.
  4. A solution of silver nitrate containing 12.14 g of silver in 50 ml of solution was

electrolysed between platinum electrodes.  After electrolysis, 50 ml of the anode solution was found

to contain 11.55 g of silver, while 1.25 g of metallic silver was deposited on  the cathode.  Calculate

the transport number of Ag+ and NO3¯   ions.

  1. How the Dc of an electrolyte solution can be determined.
  2. How could you determine the solubility of a sparingly soluble salt by conductivity

measurements.

  1. Discuss on the Debye Huckel theory of strong electrolytes.
  2. Describe how the electrolytic separations of metals are carried out.
  3. Explain the principle of polarography.

 

PART – C

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

 

  1. Explain the following :

(i)    Redox electrode              (ii)   Saturated calomel electrode

  1. Explain any four applications of EMF.
  2. How the pH of a solution can be determined using quinhydrone electrode.
  3. What are concentration cells? Derive an expression for the EMF of a concentration cell with

transference.

  1. (i) Discuss Arrhenius theory of electrolytic dissociation. Give its limitations.

(ii)   Explain the variation of specific and equivalent conductance with concentration.

  1. (i) Explain the electrochemical theory of corrosion.

(ii)   Discuss the principle and procedure for conductivity  titration of a weak acid with a strong  base.

 

Go To Main Page


 

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

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SIXTH SEMESTER – APRIL 2011

CH 6607/CH 6601 – COORDINATION CHEMISTRY

 

 

 

Date : 07-04-2011              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART –A

Answer ALL the questions                                                                           (10 x 2=20)

  1. What is the role of catalase in nitrogen fixation?
  2. Calculate CFSE value for Mn2+.
  3. What are noncomplementary electron transfer reactions?
  4. Explain outer sphere mechanism with an example.
  5. What is Trans effect? Give an example.
  6. Give an example of metal phthalocyanin involving metal template synthesis.
  7. State Jahn Teller Theorem.
  8. Draw the structure of Ni(CO)4
  9. Mention the advantages of chelate therapy.
  10. What are coenzymes? Give an example.

PART –B

Answer any EIGHT questions                                                                         (8 x 5 =40)

  1. Describe with a neat diagram crystal field splitting of metal d-orbitals in tetrahedral field.
  2. Explain the polymerization of olefins using Ziegler Natta catalyst.
  3.    Explain photo substitution reactions with a suitable example.
  4. Discuss the mechanism of inner sphere electron transfer reaction with a suitable example.
  5. What is the significance of contrast agents in MRI? Give two examples.
  6. Discuss the theories of Trans effect.
  7. Explain metal template synthesis of Schiff bases with suitable examples.
  8. Describe bonding in Fe3(CO)12
  9. Explain the mechanism of alkene hydrogenation.
  10. Write a note on photoisomerisation reactions.
  11. Discuss the biological role of carboxypeptidase and catalases.
  12. What are the experimental evidences for metal-ligand overlapping?

PART –C

      Answer any FOUR questions                                                              (4 x 10 = 40)

  1. a. Construct MO energy level diagram for [Co (NH3)6]2+
  2. Explain crystal field splitting of metal d-orbitals in octahedral complexes.
  3. a. Discuss the structure and bonding of ferrocene.
  4. Explain dissociative mechanism of ligand substitution reaction in octahedral

complexes.

  1. a. Explain cis effect with two examples.
  2. Describe the metal template synthesis of Schiff bases
  3. a. Write briefly on in vivo and in vitro nitrogen fixation.
  4. Draw the structure of a. Fe(CO)5   b. Mn2(CO)10.
  5. a. Explain 18 –electron rule with any two examples
  6. Construct Metal orbitals and LGO’s suitable for σ and П bonding in octahedral

geometry.

  1. a. Write a note on the following
  2. hydrogenation reaction c. hydroformylation reaction.
  3. photoredox reactions d.  Photoisiomerizations reactions.

 

 

Go To Main Page


 

“Loyola College B.Sc. Chemistry April 2011 Concepts In Inorganic Chemistry Question Paper PDF Download”

by

3LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – APRIL 2011

CH 1503/CH 1500 – CONCEPTS IN INORGANIC CHEMISTRY

 

 

 

Date : 06-04-2011              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

 

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

 

  1. What are the possible values of quantum numbers n, l ,m and s for an electron in 3d orbital?
  2. The metallic character increases in the order As< Sb <Bi. Substantiate.
  3. What would be the effect on lattice energy of increasing the charge on M n+?
  4. What is inert pair effect?
  5. Explain the shape of beryllium chloride, using the concept of hybridization,
  6. He2 + exists while He2 does not. Why?
  7. What are London forces?
  8. Why is sodium in liquor ammonia blue?.
  9. HgO is soluble in HCl but HgS is not. Reason out using HSAB principle.
  10. What are aprotic solvents? Give one example.

PART – B

 

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

 

  1. Describe the method of froth floatation.
  2. How is electronegativity expressed using Mulliken-Jaffé and Allred -Rochow scales? Explain.
  3. What is electrochemical series? Give one application of this series.
  4. State and explain Fajan’s rules.
  5. Using VSEPR theory arrive at the structures of XeF4 and XeF6 .
  6. Explain the factors that affect lattice energy.
  7. State and explain isoelectronic principle.
  8. Construct the qualitative MO energy level diagram of oxygen and account for its paramagnetism.
  9. State and explain Hume – Rothery rules.
  10. What are interstitial solid solutions? Explain.
  11. What are the characteristics of hard and soft acids and bases?
  12. What are leveling and differentiating solvents? Explain with an example for each.

 

 

PART – C

Answer any FOUR questions                                                                                             (4 x 10 = 40 marks)

 

23.What is an Ellingham diagram? With the help of this diagram, fix the criterion for

  1. Reduction of metal oxide by carbon at a given temperature
  2. Reduction of oxide X2O3 by a metal Y and

iii. Reduction of metal oxide by hydrogen.

 

  1. a) Construct and explain, Born-Haber cycle for determination of lattice energy of sodium chloride. (6)

 

  1. b) What is Born – Lande equation.              (4)

 

  1. Using the molecular orbital diagram, explain the magnetic properties and stabilities of CO and N2.

 

  1. Write a comparative account of the VB and MO theories of bonding.

 

  1. Distinguish between conductors, semiconductors and insulators on the

basis of band theory.

 

  1. Describe the following reactions in liquid ammonia giving an example for each:
  2. Acid-base reactions ii. Precipitation reactions  iii. Complex formation reactions and
  3. Ammonolysis.                                                                                                 (10)

 

 

Go To Main Page

“Loyola College B.Sc. Chemistry April 2011 Chemistry Of Natural Products Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SIXTH SEMESTER – APRIL 2011

CH 6610/CH 6604 – CHEMISTRY OF NATURAL PRODUCTS

 

 

 

Date : 09-04-2011              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

 

ANSWER ALL THE QUESTIONS                                                                           (10×2=20 marks)

  1. How is N-methyl group identified in alkaloids?
  2. What happens when piperine is subjected to hydrolysis with NaOH?
  3. Mention the products of ozonolysis of geraniol.
  4. Draw the structure of vitamin-A. How is it structurally related with β-carotene?
  5. What are the uses of anthocyanidin.
  6. What are flavones?
  7. Name the products obtained when uric acid is oxidized with HNO3.
  8. Draw the structures of caffeine and theophylline.
  9. Name the chromophores and auxochromes present in alizarin and methyl orange.
  10. What are phthalein dyes? Give examples.

PART – B

  ANSWER ANY EIGHT QUESTIONS                                                                      (8×5=40 marks)

 

  1. a) What is isoprene rule? b) How are terpenes classified?
  2. Outline the synthesis of piperine.
  3. Establish the structure of coniine and give its synthesis.
  4. Elucidate the structure of menthol.
  5. a) What happens when camphor is i) oxidized and ii) reduced?
  6. b) Show that camphor is bicyclic.    (3+2)
  7. Give any one synthesis of flavones.
  8. a) What are anthocyanins? What are the two components of anthocyanins?
  9. b) What happens when hirsutidin chloride is hydrolyzed with Ba(OH)2 ?    (3+2)
  10. How is uric acid synthesized from urea?
  11. What are purines? Mention their biological importance.
  12. Discuss the structure of caffeine.
  13. Discuss briefly on the relationship between color and constitution of dyes on the basis of

resonance theory.

  1. What are azo dyes? Describe the preparation and applications of any one azo dye.

 

PART – C

ANSWER ANY FOUR QUESTIONS                                                                   (4×10=40 marks)

  1. Establish the structure of nicotine and give its synthesis.
  2. Discuss the structure of citral and its synthesis.
  3. How will you arrive at the structure of quercetin?
  4. Outline the synthesis of oesterone.
  5. Explain the structure and synthesis of cyanidin hydrochloride.
  6. a) Explain the terms i) bathochromic shift ii) hypsochromic shift.
  7. b) How are the following compounds prepared?   i) Alizarin  ii) Indigo                                                                                                                                                                         (4+6)

 

 

 

 

Go To Main Page

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

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SIXTH SEMESTER – APRIL 2011

CH 6608/CH 6602 – CHEMISTRY OF MATERIALS

 

 

 

Date : 09-04-2011              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART –A

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

 

  1. Represent (111) and (110) plane of a simple cubic crystal.
  2. What is CVD?
  3. Give the classification of liquid crystals.
  4. Give an application each for TGA and DTA.
  5. What is SEM analysis?
  6. State Curie –Weiss law.
  7. Predict the coordination number for the following cation and anion Na+( 0.95A0 ) and Cl–(1.81 A0)
  8. What are semiconductors? Give an example.
  9. Distinguish between ferro and ferri magnetic properties.
  10. Identify the following complexes as diamagnetic and paramagnetic.
  1. [NiCl4]2- b. [Fe (CN)6]3-

 

PART –B

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

 

  1. Explain the structure of NaCl.
  2. With a neat diagram explain the wurzite structure.
  3. Give the radius ratio rules. How is it used to determine the coordination number? Explain with an example.
  4. Write a note on Sol gel and hydrothermal method of crystal growth.
  5. Explain photoluminescence with an example.
  6. What are n and p type semiconductors? Explain with suitable example.
  7. Explain the following:
  1. piezoelectric     pyro-electric        c. ferroelctrics

 

  1. MgFe2O4 is a normal spinel whereas NiFe2O4 is an inverse spinel. Explain.
  2. Explain the working of lithium battery.
  3. Discuss Bardeen, Cooper and Schrieffer theory.
  4. Enlist the applications of     i. SEM           ii. organic semiconductors.
  5. Explain the function of photogalvanic cell.

 

PART –C

 

  Answer any FOUR questions                                                                     (4 x 10 = 40 marks)

 

  1. What is magnetic susceptibility? How is it determined?
  2. Write a note on Schottky and Frenkel defects in crystals.
  3. Explain the principle and applications of TGA and   DTA.
  4. Discuss the types and applications of liquid crystals.
  5. Define Bravais lattices. Explain with examples.
  6. Write briefly on the following:
  1. Meissner effect. X-ray diffraction.

 

 

 

 Go To Main Page

“Loyola College B.Sc. Chemistry April 2011 Chemistry For Biologists – II Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FOURTH SEMESTER – APRIL 2011

CH 4204 / 4202  – CHEMISTRY FOR BIOLOGISTS – II

 

 

Date : 05-04-2011              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART-A

      Answer ALL the questions                                                                                            (10 x 2 = 20)

  1. How is glycine synthesized from serine?
  2. What is peptide bond? How is it formed?
  3. Write any two properties of lipids.
  4. What are steroids? Give an example
  5. What are the different types of RNA? Mention their functions.
  6. What is mutation?
  7. What are epimers? Give example.
  8. Write down the biological importance and functions of carbohydrate.
  9. What is ADP? Draw its structure.
  10. What are herbicides? Give an example.

 

PART – B

      Answer any EIGHT questions                                                                         (8 x 5 = 40)

  1. Discuss the primary structure of protein.
  2. How are enzymes classified? Give an example for each.
  3. What are essential and non-essential amino acids? Draw the structures of any three amino acids.
  4. Discuss the following a) Lecithins b) Cephalins      and     c) plasmologens
  5. Discuss the replication of DNA.
  6. Draw and discuss the structure of RNA.
  7. Write a note on a) mutarotation        b) Inversion of cane sugar
  8. Explain the first five steps in the process of conversion of glucose to pyruvic acid.
  9. Draw the Fischer and Haworth structure of D-Fructose.
  10. Draw the structure of sucrose. Discuss its non-reducing property.
  11. What is BHC? Write down its preparation and uses.
  12. Describe the manufacture of superphosphate of lime.

 

 

 

 

PART – C

Answer Any FOUR questions                                                                                 (4 x 10 = 40)

  1. Discuss Edman and Sanger’s methods to determine the N-terminal sequence of amino acid.
  2. a) Write in detail the classification of proteins based on solubility and structure. (8)
  3. b) What is meant by hydrogenation of oil? (2)
  4. Discuss the biosynthesis of cholesterol. (10)
  5. a) Write a brief note on genetic engineering. (5)
  6. b) Write the differences between DNA and RNA. (5)
  7. Explain the complete changes that occur during one complete turn of the citric

acid cycle. (TCA Cycle)  (10)

  1. Discuss the following with structures (10)
  2. Papaverine b) Nicotine        c) Coniine      d) Camphor

 

Go To Main Page

 

 

 

 

 

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

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – APRIL 2011

CH 1502/CH 5501 – ANALYTICAL CHEMISTRY

 

 

 

Date : 19-04-2011              Dept. No.                                                    Max. : 100 Marks

Time : 9:00 – 12:00

 

PART -A

Answer ALL the questions                                                                                          (10 x2 =20 marks)

 

  1. Give the threshold limits of vapor concentration of mercury and formaldehyde.
  2. How is ether handled in the laboratory?
  3. A titration is repeated four times and the titre values are 10.1, 9.9, 10.0 and              10.2 ml. calculate the mean.
  4. How is benzoic acid recrystallised?
  5. What is Rf value?
  6. Calculate the molarity when you dissolve 4.9 g of K2Cr2O7 in 1000 ml of water.
  7. Mention two adsorbents used in Column chromatography.
  8. Mention any two indications used in the titration of a strong acid against a strong base?
  9. What are adsorption indicators? Give an example.
  10. Define co-precipitation.

PART – B

 

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

 

  1. Describe the calibration of a pipette and standard flask.
  2. Analysis of a sample of iron ore gave the following percentage values for the iron content 7.08,7.21.7.12,7.09,7.16, 7.14,7.07,7.14,7.18,7.11.Calculate the mean, standard deviation and coefficient of variation for the values.
  3. Explain, briefly, the various steps involved in fractional distillation.
  4. Discuss the preparation of chromatogram in Thin Layer chromatography.
  5. What are the criteria for a primary standard? Give an example for primary and secondary standard.
  6. Explain the principle of complexiometric titration with a suitable example.
  7. Discuss the factors affecting solubility of precipitates.
  8. Sketch the thermogram of calcium oxalate monohydrate.  Discuss the thermo gravimetric analysis technique.

 

 

  1. Write briefly on ion-exchange chromatography.
  2. What is normal error analysis curve? Give its significance.
  3. Calculate the pH and the [H+] and [OH–] concentrations of a 0.005 M solution of Ba (OH) 2 in water at 250C.
  4. Calculate the molar solubility of Ag2CrO4 in water at 250C at Ksp =9 x 10-12.

 

PART – C

Answer any FOUR questions                                                                                   (4 x 10 =40 marks)      

 

  1. Discuss the principle, experimental technique and instrumentation technique of Gas chromatography.
  2. Explain in detail the types of errors.
  3. Write briefly on a. Sublimation    b. Factors affecting Rf value.
  4. Discuss the theory of acid- base indicators with suitable examples.
  5. How is chloride determined by Volhard’s method?
  6. a. Discuss the factors affecting TG and DTA thermograms.
  1. Mention any three requisites of a good wash liquid in gravimeric analysis.

 

Go To Main Page

 

 

“Loyola College B.Sc. Chemistry April 2012 Transition Elements And Nuclear Chemistry Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – APRIL 2012

CH 5506 – TRANSITION ELEMENTS AND NUCLEAR CHEMISTRY

 

 

 

Date : 27-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

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

 

  1. Explain why the molar volumes of transition elements are much lower than those of

s block elements of the neighbouring  groups.

  1. Give the uses of ferro-vanadium alloy.
  2. What are lanthanides?
  3. Name any two minerals of actinides.
  4. What is co-ordination number? Give an example.
  5. What is chelate effect?
  6. Define radioactivity.
  7. What are pi-mesons and K-mesons?
  8. What are radiopharmaceuticals? Give an example.
  9. Define critical mass.

PART – B

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

 

  1. Explain why most of the transition metals form coloured compounds.
  2. How is titanium extracted from its ores?
  3. What is lanthanide contraction? Explain any one consequence of it.
  4. Explain the isolation of uranium.
  5. Explain spectrochemical series. Mention the significance of the series.
  6. What are ligands? Explain with an example.
  7. Discuss Optical isomerism in coordination complexes with two examples.
  8. A freshly cut piece of wood gives 16100 counts of β-ray emission per minute per kg and an

old wooden bowl gives 13200 counts per minute per kg.   Calculate the age of the wooden

bowl. The half-life period of 14C is 5568 years.

  1. Describe the functioning of scintillation counter.
  2. Explain the significance of ratio with examples.
  3. Explain hydrogen bomb.

 

  1. Discuss ‘neutron activation analysis’.

 

PART – C

 

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

 

  1. (a) Discuss the toxic effects of cadmium.

(b)  Explain the preparation of  K2Cr2O7.

 

  1. (a) Explain the electronic spectra of lanthanide compounds.

(b)  How is neptunium synthesized?   Give its uses.

 

  1. (a) Explain the postulates of VB theory of coordination compounds.

(b)  Discuss the geometrical isomerism exhibited by coordination compounds with two

examples.

 

  1. (a) Discuss any three evidences to support crystal field theory.

(b)  Calculate the CFSE for octahedral high and low spin for d4, d7 configuration.

 

  1. (a) Explain radioactive displacement law.

(b)  Discuss the liquid drop model of the structure of nucleus.

 

  1. (a) Discuss the atomic power projects in India.

(b)  Explain the construction and working of a nuclear reactor.

 

 

 

 

Go To Main page

“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?

 

 

Go To Main page

“Loyola College B.Sc. Chemistry April 2012 Synthetics Organic Chemistry And Spectroscopy Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SIXTH SEMESTER – APRIL 2012

CH 6609/CH 6603 – SYNTHETICS ORGANIC CHEMISTRY AND SPECTROSCOPY

 

 

 

Date : 23-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

Answer all questions:                                                                                                       (10X2=20)

 

  1. What do you mean by umpolung?
  2. What are synthons? Give an example.
  3. Complete the following reactions
  4. Name the reagents used for the following conversion.

 

 

 

 

  1. What is meant by an active methylene group? Give an example.
  2. Give an important condition for a ketone to undergo Aldol condensation.
  3. Calculate the λmax for the following molecule:

 

 

  1. How will you distinguish the following pair of isomers from their IR spectra?

 

 

  1. Define the term chemical shift.
  2. State nitrogen rule in mass spectra.

 

PART – B

Answer any EIGHT questions:                                                                                            (8×5=40)

 

  1. Write a note on convergent synthesis.
  2. Explain the various types of intermediates that are formed in organic reactions.
  3. What are activating groups? Explain their usefulness in organic synthesis.
  4. Write the mechanism of Wolf-Kishner reduction.
  5. What is DIBAL? Explain its preparation and usefulness.
  6. Write the mechanism of Aldol condensation.
  7. Complete the following reactions

 

 

  1. Explain the following with suitable examples:
  2. a) Bathochromic Shift
  3. b) Hyperchromic Shift
  4. How is IR spectroscopy useful in detecting the H-bonding in organic compounds?
  5. Explain the Proton NmR spectrum of ethyl alcohol contaminated with a little HCl.
  6. Write the mechanism of McClafferty rearrangement with reference to mass spectroscopy.
  7. Explain why cyclohexane gives only one peak at room temperature while it gives two peaks

at-100°C.

 

PART – C

Answer any FOUR questions:                                                                                        (4X10=40)

 

  1. a) write a note on retrosynthetic analysis.   (5)
  2. b) What are protecting groups? Explain the usefulness of them in organic synthesis.  (5)

 

  1. Starting from acetoacetic ester, how will you prepare the following?

(i) Acetone (ii) succinic acid (iii) antipyrine   (iv) 4-methyl uracil (v) acetic acid.                  (10)

 

  1. a) How will you distinguish the following pairs of compounds using IR Spectroscopy? (4)

(i) CH3-CH2-OH and CH3-O-CH3

(ii) maleic and fumaric acids

  1. b) An organic compound of molecular formula C9H10O2 showed three peaks in the PMR

spectrum as given below.

δ1.96 (S,3H)

δ5.0 (S,2H)

δ7.2 (S,5H)

Identify the structure of the compound.                                                                                   (6)

 

  1. a) write a note on coupling constants.   (4)
  2. b) A cyclic ketone (C5H8O, A) on reaction with NaOCH3 gives a product B which has the

following NMR signals.

δ 3.6 (S,3H)

δ1.2 (S,9H)

Deduce the structures of A and B.                                                                                           (6)

 

  1. Deduce the structure of the compound C9H8O which exhibited the following spectral data:

UV: λ max(EtOH) : 285 nm (ε 45000)

IR: ۷max (KBr) : 3090,2820,2750,1685,1630,1610,970 cm-1

NMR: δ 6.62(1H, dd) J= 16 and 7 Hz, 7.41 (1H,d), 7.4 (5H, m), 9.66 (1H, d)

MS: m/z 132,131, 103, 91,77 and 51.

 

  1. a) Discuss the instrumentation of IR Spectrometer with the block diagram. (6)
  2. b) How are the following groups protected and deprotected during organic synthesis.  (4)

 

Go To Main page

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

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – APRIL 2012

CH 5402/5400- POLYMER CHEMISTRY

 

 

Date : 27-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

Part – A (Answer ALL questions):                                                                              (10 x 2 = 20 Marks)          

  1. Draw the structures of polyisoprene and polystyrene.
  2. Define: Cohesive energy.
  3. Mention the uses of polyamide and bakelite.
  4. What is Zeigler-Natta catalyst? Mention its use.
  5. Why anionic polymerization is also called living polymerization?
  6. Mention the significance of CMC.
  7. How does benzoyl peroxide initiate polymerization?
  8. Mention the conditions for chain end degradation.
  9. Account for the thermal stability of Teflon.
  10. What are plasticizers? Give an example.

 

Part – B   (Answer any EIGHT only):                                                                            (8 x 5 =40 Marks)

  1. How is the number average molecular weight of a polymer estimated?
  2. Distinguish between homopolymers and copolymers with examples.
  3. Discuss the importance of hydrogen bonding in polymers.
  4. Explain the mechanism of preparation of PVC by cationic polymerization.
  5. Write a note on step growth polymerization with an example.
  6. Explain interfacial polymerization with a suitable example.
  7. Mention any two uses of PTFE, Buna-N and Polyester.
  8. What are known as zipping and unzipping in polymers?
  9. How are (i) Nylon-6,6 and (ii) Neoprene prepared?
  10. Articles made up of polypropylene can be steam sterilized – explain.
  11. Explain the role of polymer additives in polymerization process.
  12. Write a note on injection moulding.

 

 

 

 

Part – C   (Answer any FOUR only):                                                                          (4 x 10 =40 Marks)

  1. Explain the following with suitable examples
  1. a) plastics and elastomers b) natural and synthetic polymers (5+5)
  1. Discuss the mechanism of the preparation of stereo-regular polypropylene using Ziegler-Natta catalyst.
  2. a)  Discuss the mechanism of a free radical polymerization. (6)
  1. b) Explain auto acceleration in bulk polymerization. (4)
  1. Explain the acid and base catalysed mechanism of the formation of phenol-formaldehyde resin.
  2. Explain the conductivity of polypyrrole, polysulphur nitriles and polyphenylene with the factor influencing their conductivity.
  3. Write a note on  the following processing techniques of polymer
  1. a) Calendring b) Die casting (5+5)

 

Go To Main page

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

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

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – APRIL 2012

CH 5402/5400 – POLYMER CHEMISTRY

 

 

Date : 27-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

Part – A (Answer ALL questions)               (10 x 2 = 20 Marks)  

  1. Draw the structures of polyisoprene and polystyrene.
  2. Define: Cohesive energy.
  3. Mention the uses of polyamide and bakelite.
  4. What is Zeigler-Natta catalyst? Mention its use.
  5. Why anionic polymerization is also called living polymerization?
  6. Mention the significance of CMC.
  7. How does benzoyl peroxide initiate polymerization?
  8. Mention the conditions for chain end degradation.
  9. Account for the thermal stability of Teflon.
  10. What are plasticizers? Give an example.

 

Part – B   (Answer any EIGHT only)          (8 x 5 =40 Marks)

  1. How is the number average molecular weight of a polymer estimated?
  2. Distinguish between homopolymers and copolymers with examples.
  3. Discuss the importance of hydrogen bonding in polymers.
  4. Explain the mechanism of preparation of PVC by cationic polymerization.
  5. Write a note on step growth polymerization with an example.
  6. Explain interfacial polymerization with a suitable example.
  7. Mention any two uses of PTFE, Buna-N and Polyester.
  8. What are known as zipping and unzipping in polymers?
  9. How are (i) Nylon-6,6 and (ii) Neoprene prepared?
  10. Articles made up of polypropylene can be steam sterilized – explain.
  11. Explain the role of polymer additives in polymerization process.
  12. Write a note on injection moulding.

Part – C   (Answer any FOUR only)            (4 x 10 =40 Marks)

  1. Explain the following with suitable examples
  1. a) plastics and elastomers b) natural and synthetic polymers (5+5)
  1. Discuss the mechanism of the preparation of stereo-regular polypropylene using Ziegler-Natta catalyst.
  2. a)  Discuss the mechanism of a free radical polymerization. (6)
  1. b) Explain auto acceleration in bulk polymerization. (4)
  1. Explain the acid and base catalysed mechanism of the formation of phenol-formaldehyde resin.
  2. Explain the conductivity of polypyrrole, polysulphur nitriles and polyphenylene with the factor influencing their conductivity.
  3. Write a note on  the following processing techniques of polymer
  1. a) Calendring b) Die casting (5+5)

 

Go To Main page

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

“Loyola College B.Sc. Chemistry April 2012 Physics For Chemistry – II Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – APRIL 2012

PH 3202 – PHYSICS FOR CHEMISTRY – II

 

 

 

Date : 02-05-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

Answer ALL questions:                                                                                                              (10×2=20)

 

  1. Convert the given decimal number into binary number 56.42.
  2. State Demorgan’s theorem.
  3. What is photoelectric effect?
  4. State Pauli’s exclusion principle.
  5. Write any two general properties of nucleus.
  6. What are elementary particles?
  7. Define absorption coefficient of material.
  8. What are the two types of sound waves?
  9. State Heisenberg’s uncertainty principle.
  10. What is box normalization of wave system?

 

PART – B

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

 

  1. Simplify the given Boolean function using K-map F(A,B,C,D)=∑(0,2,5,7,8,10,13,15)
  2. Discuss about different types of photoelectric cells.
  3. Explain nuclear fission reaction by using liquid drop model.
  4. Describe the production of ultrasonic sound waves by Piezo-electric method.
  5. Derive Schrödinger time dependent wave equation from the fundamental wave equation.

 

PART – C

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

 

  1. With a logic circuit and truth table describe the working of a JK flip-flop.
  2. a) State the postulates of Bhor atom model (2.5)
  3. b) Obtain the expression for the radius and electron energy of the nth orbit.    (10)
  4. a) Write the semi-empirical mass formula to calculate the binding energy of the nucleus and explain each term in it. (10)
  5. b) Draw a graph of binding energy per nucleon versus mass number. (2.5)
  6. Derive an expression of reverberation time from Sabine’s law.
  7. a) Find the de-Broglie wave length associated with a 46gm golf ball with velocity 36m/s. (2.5)
  8. b) Describe Davisson and Germer experiment for the study of electron diffraction. (10)

 

Go To Main page

“Loyola College B.Sc. Chemistry April 2012 Physics For Chemistry – I Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SECOND SEMESTER – APRIL 2012

PH 2103/2100 – PHYSICS FOR CHEMISTRY – I

 

 

 

Date : 23-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

 

PART – A

Answer ALL questions:                                                                                                                (10×2=20)

  1. What are generalised coordinates?
  2. Define the term velocity. Write its unit.
  3. Write Newton’s law of gravitation.
  4. Write the principle of equivalence in gravitation.
  5. Write Hook’s law.
  6. Define surface tension of a liquid.
  7. What is a polaroid?
  8. Differentiate between Fresnel and Fraunhofer diffraction.
  9. Define unit cell.
  10. What is the significance of Miller indices?

 

PART – B

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

  1. Explain the significance of velocity- time graph of a moving body.
  2. (i)Two bodies of mass 10kg and 25kg are placed at a distance of 0.2m apart. Find the force between them. G = 6067×10-11 S.I. units. (4.5)

(ii) Define parking orbit.                                                  (3)

  1. Discuss the atomic arrangement in a sodium chloride crystal .
  2. Briefly explain circular and elliptical polarization.
  3. Write in detail, the molecular theory of surface tension.

 

PART – C

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

 

  1. Derive Lagrange’s equation for a simple pendulum.
  2. (i)Write Kepler’s laws of planetary motion

(ii)What is escape velocity? Derive the expression for the escape velocity of a body.

  1. Derive Poiseuille’s formula for the flow of liquid through a capillary tube.
  2. Explain Bragg’s experiment of X-ray diffraction and arrive at Bragg’s law..
  3. Explain in detail, Fraunhofer diffraction at a single slit and arrive at the expression for the secondary maxima.

Go To Main page

“Loyola College B.Sc. Chemistry April 2012 Phase Equilibria And Kinetics Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – APRIL 2012

CH 5507 – PHASE EQUILIBRIA AND KINETICS

 

 

 

Date : 30-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

 

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

 

  1. Define congruent melting point.
  2. State phase rule and mention the terms involved in it.
  3. What are isotonic solutions?
  4. What do you mean by abnormal Colligative properties?
  5. What are zero order reactions? Give an example.
  6. Bring out the differences between order and molecularity of a reaction.
  7. State the steps that are involved in the thermal docomposition of acetaldehyde.
  8. Explain how ionic strength affects the rate of a reaction in solution.
  9. What is heterogenous catalysis?
  10. Define the term Adsorption.

PART – B

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

 

  1. Apply phase rule to water system. Draw the phase diagram of it.
  2. Explain phase rule to lead-silver system and discuss the desilverisation of lead from this

system.

  1. State and explain Raoult’s law.
  2. The molar heat of vaporization of water at 100oC is 40.585 kJ mol-1. At what temperature

will a solution containing 5.60 g of glucose per 1000 g of water boil?

  1. What are azeotropes? Explain.
  2. Derive the expression for the rate constant for the reaction 2A -> products.
  3. Calculate the activation energy of a reaction whose rate constant is tripled by a 10oC rise in

temperature  from the initial temperature of 27oC.

  1. Explain the kinetics of parallel reaction with one example.
  2. Explain the theory of absolute reaction rate and show how it is superior to other theories.
  3. Explain the kinetics of acid catalysed ester hydrolysis.
  4. State and explain the factors that affect the rate of enzyme catalysis.
  5. What are Wilkinson’s catalysts? Explain its catalytic action in reactions.

PART – C

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

 

  1. Draw and explain the phase diagram of FeCl3-H2O system.

 

  1. (a) Derive Clausius-Clapeyron equation and state any one of its applications.

(b) Explain partially miscible binary systems with suitable examples.

 

  1. (a) Derive Nernst distribution law and state its limitations.

(b) Discuss on steam distillation.

 

  1. (a) Explain the differential method of determination of order of a reaction.

(b) Explain the effect of solvent on the rate on SN2 reaction.

 

  1. (a) Explain Lindemann’s steady state principle.

(b) State the postulates of Langmuir’s adsorption equation and derive the equation.

 

  1. Discuss the kinetics of enzyme catalysis with Michaelis – Menton mechanism. How are the

rate constants evaluated?

 

 

 

 Go To Main page

“Loyola College B.Sc. Chemistry April 2012 Organic Functional Groups – II Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – APRIL 2012

CH 5505 – ORGANIC FUNCTIONAL GROUPS – II

 

 

 

Date : 25-04-2012              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

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

 

  1. Why Nitrobenzene is often used as solvent in Friedel Crafts reaction.
  2. How will you prepare nitroethane by vapourisation method?
  3. Assign R and S configuration to the following:

   

                                                

  1. What are enantiomers? Give two properties of enantiomers.
  2. Explain Walden inversion using SN2 reaction.
  3. Explain keto-enol tautomerism exhibited by acetoacetic ester.
  4. What is Cope rearrangement?
  5. Give the products of the following reaction:

      

  1. What is isoprene rule? Indicate the isoprene units in the structure of α-pinene.
  2. Write the structure of Conine.

         

PART – B

Answer any EIGHT questions:                                                                 (8 x5 = 40)

 

  1. Give the products obtained when Nitrobenzene is reduced in
  2. a) Strongly acidic solution
  3.  b) Strongly alkaline solution.
  4. Using Hinsberg test,how will you distinguish between

       N-methylaniline and N,N’ dimethyl aniline.

  1. Explain why pyridine is more basic than pyrrole.
  2. i) What is asymmetric synthesis?
  3. ii) How will you prepare (-) lactic acid from pyruvic acid?
  4. Discuss the optical isomerism exhibited by biphenyl compounds.
  5. How will you synthesize adipic acid from ethyl acetoacetate?
  6. How will you synthesize propionic acid from acetic acid using Arndt – Eistert

      reaction.

  1. Describe Hoffmann rearrangement. Discuss its mechanism.
  2. Describe Fries rearrangement and give its mechanism.
  3. Complete the following reactions.

 

       

  1. How will you synthesize nicotine from nicotinonitrile?
  2. What are the products obtained when Citral is subjected to oxidation with

       alkaline KMnO4  followed by chromic acid?

 

PART – C

 

Answer any FOUR questions:                                                                              (4 x 10 =40)

 

  1. i. How is Nitrobenzene prepared from benzene? Give its mechanism.
  2. How will you prepare o-dinitrobenzene and p-dinitrobenzene from Aniline?

 

  1. i. What is diazotisation? How is benzene diazonium chloride prepared in the

         laboratory?

  1. Explain Gattermann and Sandmeyer reactions using suitable examples.

 

  1. i. Discuss Claisen rearrangement with a specific example . Give its mechanism.
  2. How will you prove that in Claisen rearrangement ,o-isomerisation takes place

         with inversion of position?

 

  1. i. Describe the various methods for the resolution of racemic mixtures.
  2.    Explain the phenomenon of racemisation taking a suitable example.

 

  1. i. How is Quinoline prepared by Skraup’s synthesis?
  2. Electrophilic substitution in pyrrole takes place at 2- position whereas in

          pyridine at 3- position. Why?

 

  1. i. What are Alkaloids? How are they extracted from plants?
  2. How are Terpenes classified?

       iii. What are the structural formula and uses of

  1. Menthol b. α-Pinene  c. Camphor. 

 

 

Go To Main page

© Copyright Entrance India - Engineering and Medical Entrance Exams in India | Website Maintained by Firewall Firm - IT Monteur