B.Sc. Chemistry Question paper

“Loyola College B.Sc. Chemistry April 2009 Bioinformatics – I Question Paper PDF Download”

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     LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY.

VE 06

THIRD SEMESTER – April 2009

PB 3204 – BIOINFORMATICS – I

 

 

 

Date & Time: 16/04/2009 / 1:00 – 4:00         Dept. No.                                                       Max. : 100 Marks

 

 

 

PART A

 

Answer all the questions                                                       (20 marks)

 

  1. Choose the best answer (5X1=5)

 

Answer all the questions

  1. Data model used in bioinformatics application is
  2. a) hierarchial b)relational c)network d)multidimensional
  3. NCBI hosts
  4. a) BLAST b) FASTA c)DDBJ           d)Lalign
  5. Aromatic aminoacids are
  6. a) tyrosine and tryptophan
  7. b) tyrosine and threonine
  8. c) phenylalanine and alanine
  9. d) phenylalanine and leucine
  10. Double helical model of DNA was published by
  11. a) Watson and Crick
  12. b) Linus Pauling and Crick
  13. c) Rosalind Franklin and Crick
  14. d) Corey and Watson
  15. Addition of adenine to mRNA is called
  16. a) 3’ modification
  17. b) 5’ modification
  18. c) Poly A tailing
  19. d) Polymerase Chain reaction

 

  1. State whether the following true or false (5X1=5)

 

  1. Chargaff rule says A=T and G=C.
  2. Removal of introns and reunioin of exons is called Splicing.
  3. RefSeq is a standard database for comparative analyses.
  4. Cn3D is compatible with PDB.

10.NebCutter tool identifies restriction sites.

 

 

 

 

III. Complete the following                                                                          (5X1=5)

 

  1. Proline and glycine are found in _______ of protein secondary structure.
  2. Proof reading function of polymerase is due to________ activity.
  3. PubChem Substance is a _________ database.

 

14._________ are produced by gene duplication within a species but has different functions.

  1. The latest genome sequenced is from an endangered species _______.

 

  1. Answer the following, each not exceeding 50 words. (5X1=5)

 

  1. Compute pI/MW
  2. Expand HSP
  3. What is a Start codon?
  4. Define DotPlot
  5. What is a Rooted Phylogenetic Tree?

 

PART B

                                                                                    (5X8=40)

Answer any five of the following, each not exceeding 350 words.

Draw diagrams and flowcharts wherever necessary.

 

  1. Explain OMIM and its features.
  2. What are the features of PDB?
  3. Discuss about BLAST and its types.
  4. How will you analyze the gene structure in eukaryotes using software tools?
  5. List the databases involved in Protein Domain analyses.
  6. Explain about proteomic tools.
  7. Detail the various molecular visualization tools with emphasis on Homology modeling.
  8. Write about ORF finder of NCBI.

 

PART C

Answer the following, each not exceeding 1500 words                  (2X20=40)

Draw diagrams and flowcharts wherever necessary.

 

29a) Explain Smith Waterman Local Algorithm by aligning the following sequences

ACG TAT CGC GTA TA

GAT GCT CTC GGA AA

Or

  1. b) Elaborate upon Multiple Sequence alignment and its software tools.

 

30 a) Write about the mechanism of translation of protein in detail.

Or

  1. b) How does the process of DNA replication occur inside the cell?

 

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“Loyola College B.Sc. Chemistry April 2009 Chemistry For Biologists – II Question Paper PDF Download”

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     LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

WD 13

B.Sc. DEGREE EXAMINATION – PLANT.BIO&BIOTEC.& ADV.ZOO.&BIO.TECH.

FOURTH SEMESTER – April 2009

CH 4204 / CH 4202 – CHEMISTRY FOR BIOLOGISTS – II

 

 

 

Date & Time: 27/04/2009 / 9:00 – 12:00  Dept. No.                                                   Max. : 100 Marks

 

 

PART A

Answer all the questions.                                                                                   10 x 2 = 20

  1. Who is called as the father of modern enzymology? Why?
  2. Define isoelectric point.
  3. How is glycine prepared by strecker synthesis?
  4. What are coenzymes?
  5. Define rancidity of an oil.
  6. Draw the structure of adenine and guanine.
  7. How is the presence of ketone group in C-2 position confirmed in fructose?
  8. Draw the structures of a) papavarine and b) camphor.
  9. Define saponification value of an oil.
  10. How is urea prepared?

PART B

Answer any eight questions.                                                                                8 x 5 = 40

 

  1. How is N-terminal of an amino acid determined by Sanger’s method?
  2. What are the factors affecting the enzymatic activity?
  3. What are phospholipids? Explain any two types of phospholipids.
  4. Describe the steps involved in the preparatory phase of glycolysis.
  5. What are macro and micronutrients? Discuss with examples.
  6. Explain the classification of alkaloids.
  7. How are the following prepared?
  8. a) Superphosphate of lime                     b) DDT                        c) BHC
  9. Distinguish glucose and fructose by oxidation and reduction reactions.
  10. Explain the isolation of terpenes.
  11. Discuss the different types of soil.
  12. Describe the importance of flavones and flavanoids.
  13. Give any two methods of preparation of an amino acid.

PART C

Answer any four questions.                                                                              4 x 10 = 40

  1. What is enzyme inhibition? Explain the types of inhibition with examples.
  2. a) Explain the double helical structure of DNA.
  3. b) Briefly describe the replication of DNA.        (5+5)
  4. Discuss the various steps involved in TCA cycle with the energy yield.
  5. How is the structure of glucose elucidated?
  6. a) What are coenzymes? Explain the mechanism of coenzyme reaction.
  7. b) What is translation? Explain the process in brief.                     (5+5)
  8. Explain the primary and secondary structure of proteins.

 

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

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 18

FIFTH SEMESTER – April 2009

CH 5501 – ANALYTICAL CHEMISTRY

 

 

 

Date & Time: 17/04/2009 / 9:00 – 12:00 Dept. No.                                                  Max. : 100 Marks

 

 

 

PART – A

 

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

  1. Define relative error.
  2. How is antidote prepared?
  3. Why is vaccum distillation needed for some liquids?
  4. Define elution and eluant in chromatography.
  5. Mention any two characteristics of a primary standard substance.
  6. Define molarity
  7. Differentiate equivalence point from end point.
  8. How is solubility of sparingly soluble salt related to solubility product for AgCl?
  9. State Beer-Lamberts law.
  10. Draw the possible modes of vibrations for water molecule.

PART – B

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

 

  1. Define absolute error. The accepted value for the sets of data 25.40, 25.36, 25.26, 25.34 is 25.28.  Calculate the absolute error.
  2. Write a note on Soxhlet extraction.
  3. What are the steps involved in separation of mixture of components using TLC technique.
  4. Mention principle and the different types of chromatography.
  5. What are the different types of titrimetric analysis? Explain them with examples.
  6. 20ml 0.1M CH COOH is titrated with 0.1 M NaOH calculate the pH at the equivalence point (Ka = 1.8 X 10-5).
  7. What is metal ion indicator? Give examples.
  8. Explain co-precipitation and post precipitation with examples.
  9. What is an adsorption indicator? Explain with an example.
  10. Differentiate chromophore and auxochrome.
  11. How is Beer-Lambert’s law veified? Explain them.
  12. What are the factors affecting the absorption maximum in UV-visible spectroscopy?

 

PART – C

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

 

  1. a) Define Mean, Median and Standard deviation                   (6)
  2. b) Find out the mean and median for following data: 48.32, 48.36, 48.23, 48.11 and 48.38. (4)
  3. a) Compare the following: distillation, fractional distillation and vaccum distillation.  Under

what conditions the above techniques are adopted for purification.                                         (7)

 

  1. b) For a given volume of solvent, multiple extraction is more efficient than single extraction.

Why?                                                                                                                                              (3)

 

  1. a) Explain the separation of a mixture by Gas chromatography.                    (7)
  2. b) Write the different types of ion exchange resin used in ion-exchange chromatography.          (3)

 

  1. a) What is meant by chelating agent? Give examples.                                                                  (2)
  2. b) Explain the different types of EDTA titrations                                                                       (8)

 

  1. a) How is silver ion determined by Volhard method?        (5)
  2. b) Explain the factors affecting the solubility of a sparingly soluble salt.                                      (5)

 

  1. Draw the block diagram of IR spectrometer and explain them. How IR absorption bands useful

in the identification of organic compounds?  Give examples.

 

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“Loyola College B.Sc. Chemistry April 2009 Adv. General Chemistry For Phys.& Maths Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – PHYSICS & MATHEMATICS

WO 08

THIRD SEMESTER – April 2009

CH 3202 / 3200 – ADV. GENERAL CHEMISTRY FOR PHYS.& MATHS

 

 

 

Date & Time: 16/04/2009 / 1:00 – 4:00         Dept. No.                                                       Max. : 100 Marks

 

 

PART-A

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

  • What is meant by intermolecular hydrogen bonding ? Give an example.
  • Write any two consequences of lanthanide contraction?
  • Draw the structure of  Ibruprofen . Give its uses.
  • State the first law of thermodynamics.
  • Mention any two uses of sulphadizine.
  • Give any one preparation of thiophene.
  • How is a dipeptide formed ? Give an equation.
  • What is nuclear fission reaction? Give an example.
  • Write the important function of any three essential nutrients for the plant growth.
  • Define Octane number.

PART-B

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

 

  • Explain the theory involved in hydrogen bonding .
  1. How will you separate o –and p – nitrophenol ?
  • How is the solubility of sparingly soluble salt determined ?
  • Discuss Born– Haber cycle with an example.
  • Define enthalpy of neutralization. Explain why the enthalpy of neutralization of a strong acid vs. strong base is always a constant?
  • Derive Kirchoff’s equation.
  • Derive the relation connecting ∆E and ∆H for a reaction involving an ideal gas.
  • State and explain Kohlrausch’s Law.
  • Discuss the open chain formula of glucose.
  • Explain the preparation of an amino acid by Gabriel synthesis.
  • Describe the classification of enzymes based on IUB system.
  • Explain the uses of radioisotopes in medicines and agriculture.
  • What are mixed fertilizers? Give any four advantages of it.

 

PART-C

Answer any Four questions:                                                   (10 × 4= 40)

 

  • Describe the separation of lanthanides by ion exchange method .(7)
  1. ii) Why do ice float on water? (3)
  • Give a method of preparation and uses of  sulphanilamide ( 5 )
  1. How is naphthalene prepared by Haworth synthesis? (5)
  • Explain conductometric titration of (i) strong acid against a strong base

(ii) weak acid against strong base.

  • Explain the working principle of  primary reference electrode  (7)
  1. What is the electrophile ? Mention the electrophile in sulphonation. ( 3)
  • i . Discuss the various factors affecting the enzyme reaction.(8)

ii . Write the lock and key mechanism of an enzymatic reaction.(2)

  • Write briefly on any two of the following: (5+5)
    1. Bordeaux mixture.
    2. Chromophores
    3. Photosynthesis
    4. Nuclear fusion

 

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“Loyola College B.Sc. Chemistry Nov 2010 Transition Elements And Nuclear Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – NOVEMBER 2010

CH 5506 – TRANSITION ELEMENTS AND NUCLEAR CHEMISTRY

 

 

 

Date : 01-11-10                     Dept. No.                                                    Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

 

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

 

  1. What are molybdates? Give the structure of molybdate ion.
  2. Bring out the biological importance of manganese.
  3. Why do lanthanides show the characteristic +3 oxidation state?
  4. Name the three actinides that are found naturally on Earth.
  5. Write the IVPAC name for each of the following complexes:
  6.   [CrCl3(py)3]X             b. [Pt(H2NCH2CH2NH2)2Cl2]Cl2 .
  7. Draw the fac and mer isomers of [Co(NH3)3Cl3] and [Co(dien)2] 3+ .
  8. What is K-electron capture?
  9. Write the mathematical expression of Geiger-Nuttal’s rule.
  10. What are the limitations of breeder reactors?
  11. Define the term critical mass.

PART – B

 

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

 

  1. Discuss the toxic effects of cadmium.
  2. Write a brief note on organo zinc compounds.
  3. How is neptunium synthesized? What are its uses? Mention its oxidation states.
  4. Describe the method of isolation of uranium from its ores.
  5. Using VB theory explain the geometry and magnetism of [CoF6]3–and [Co(CN)6]3– .
  6. What are chelates? Why are chelated complexes more stable than similar complexes

with monodentate ligands?

  1. Explain the different factors that affect the magnitude of d-orbital splitting values in an

octahedral complex.

  1. Write a note on the applications of radioactive isotopes in agriculture and biology.
  2. Give the salient features of Shell model of the nucleus.
  3. Explain the theory of nuclear fission.
  4. Describe the construction and working of GM counter.
  5. Explain the principle and application of neutron activation analysis.

 

PART – C

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

 

  1. a) Discuss the various oxidations states exhibited by titanium. Which is the most stable

oxidation  state?                                                                                                                       (4)

  1. b) How is chromium extracted from its ores? (6)
  2. What is lanthanide contraction? What are its consequences?
  3. a) Calculate the crystal field stabilization energy in terms of Δo for a d8 system in

octahedral and  tetrahedral complexes. Which is more stable?                                     (5)

  1. b) What are the major drawbacks of VBT.
  2. a) Mention the salient features of crystal field theory. How are d-orbitals split, when a

transition  metal ion is placed in (i) an octahedral field and (ii) a tetrahedral field?    (6)

  1. b) Explain coordination isomerism with an example.                                                           (4)
  2. a) What is n/p#ratio? How is related to stability of nuclei?                                                 (5)
  3. b) What are alpha and beta decay? Give equations.                                                           (5)
  4. Give an account of a nuclear fission reactor.

 

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

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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 Nov 2010 Physics For Chemistry – II Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION –  CHEMISTRY

THIRD SEMESTER – NOVEMBER 2010

PH 3202 – PHYSICS FOR CHEMISTRY – II

 

 

 

Date : 12-11-10                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART-A

Answer all the questions.                                                                                          10×2=20

  1. Subtract the given binary numbers by 2’s complement method, 10001 – 01110
  2. State De-Morgan’s law.
  3. What is photoelectric effect?
  4. State Pauli’s exclusion principle.
  5. What is mass defect?
  6. What is inverse Piezo-electric effect.
  7. What are elementary particles?
  8. A microscope, using photons, is employed to locate an electron in an atom to within a distance of 0.2Ǻ. What is the uncertainty in the momentum of the electron located in this way?
  9. Mention any two factors that affect the acoustics of a building.
  10. What are matter waves?

PART-B

Answer any four questions.                                                                                     4×7.5=30

  1. With a neat circuit diagram and truth table explain full binary adder.
  2. Describe Millikan’s experiment to verify the Einstein’s photo electric equation.
  3. Obtain the Newton’s formula of velocity of sound.
  4. Describe the liquid drop model of the nucleus.
  5. Derive Schrodienger time dependent wave equation from the fundamental wave equation.

PART-C

Answer any four questions                                                                                      4 x12.5=50

  1. a) What is Karnaugh map (K map) method? (2)
  2. b) Simplify the Boolean function F(A,B,C,D) = ∑(0,1,2,4,5,10,11,14,15) using K-map. Design a logic circuit of the simplified equation. (7.5+3)
  3. a) State the postulates of Bohr’s atom model.                   (2.5)
  4. b) Obtain expressions for the radius and electron energy of the nth orbit. (10)
  5. a) State Sabine’s law (2.5)
  6. b) Derive the expression for reverberation time from Sabine’s law (10)
  7. Describe the Davisson and Germer experiment for the study of electron diffraction.
  8. Give a detailed account of the general properties of a nucleus.

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“Loyola College B.Sc. Chemistry Nov 2010 Phase Equilibria And Kinetics Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – NOVEMBER 2010

CH 5507 – PHASE EQUILIBRIA AND KINETICS

 

 

 

Date : 03-11-10                     Dept. No.                                                 Max. : 100 Marks

Time : 9:00 – 12:00

 

PART-A

Answer ALL questions                                                                                            (10 X 2 = 20 marks)

 

  • Write the expression for degree of freedom.
  • Define Eutectic temperature.
  • State Raoult’s law.
  • State Nernst distribution law.
  • Write the chemical equation for the oxidation of iodide by persulphate. What is the

overall order of the reaction.

  • Define specific rate. Comment on its unit.
  • A radio active element undergoes nuclear disintegration. What type of complex

reaction is it?

  • Predict the effect of added KNO3 on the rate of oxidation of iodide by persulphate.
  • Write the general steps involved in a chain reaction.
  • Distinguish between adsorbent and adsorbate.

PART-B

 

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

 

  • Draw the phase diagram of sulphur system and apply phase rule to it.
  • Magnesium and Zinc form a stable compound with the composition of MgZn2 having congruent melting point.  Draw the phase diagram for the system and apply phase rule to it.
  • (a) Define cryoscopic constant and give its significance.                                    (2)

 

(b) 0.001 Kg of a solute  dissolved in 0.1 Kg of solvent having cryoscopic constant 5.0 K Kg

mole-1  gave a depression in freezing point as 0.2 K.  Calculate the molecular mass of

the solute.                                                                                                                                (3)

 

  • What would be the vapour pressure of 0.5molal solution of urea in water at 298 K. (Given

that vapour pressure of pure water at 298 K is 3173Pa).

 

  • Why acid catalysed hydrolysis of ester follows pseudo first order kinetics? Derive the

expression for the rate constant of this reaction.

 

  • Describe Van’t Hoff differential method of determining the order of a reaction.

 

  • (a) What is critical solution temperature? Explain with an example.                                  (2)

(b) How CST of phenol-water system vary with added NaCℓ ?                                              (3)

 

  • In the reaction of hydrogen with bromine under thermal condition, the following observations are made:
  1. The rate of the reaction is having first order dependence on H2 and fractional order dependence on Br2
  2. Product formed, HBr is found to retard the reaction.
  3. Presence of radicals is proved.
  4. Addition of Br2 is found to reduce the inhibiting nature of HBr.
  5. Overall rate expression for the reaction is rate = {k[H2][Br2]1/2}  {k’ + k”[HBr]}

Propose a probable mechanism for the reaction to explain the above observations.

 

  • List any five factors that affect the rate of a chemical reaction.
  • Explain Lindemann hypothesis of unimolecular reactions.
  • Explain the steps involved in a heterogeneous catalysed reaction.
  • Discuss the kinetics of enzyme catalysed reactions.

PART-C

 

Answer any FOUR questions                                                                                  (4 X 10 = 40 marks

 

  • Ferric Chloride when added to water, forms four different types of hydrates having definite congruent melting points. Draw a phase diagram depicting the observed phenomenon and apply phase rule to the system.
  • (a) Explain the principle of Pattinsons process.                                      (5)

(b) Explain the principle of fractional distillation.                                                                                    (5)

  • When 1 liltre of an aqueous solution containing 5g of a solute is shaken with 50 mL of ether, it is found that 0.84 g of solute passes into ether. How much of solute will be left unextracted if same aqueous solution is shaken with second installment of 50 mL ether.  What would be left behind if there was only one extraction with 100 mL of ether.
  • (a) Derive the expression for the rate constant of of a second order reaction

2 A products                                                                                                                             (5)

(b) Define half life of a reaction.  How half life measurements can be used to determine the

order of the reaction.                                                                                                                  (5)

27) Give the postulates of collision theory and deduce the expression for the rate constant of

a bimolecular reaction.                                                                                                          (4+6)

28) Derive Langmuir adsorption isotherm equation and explain.                                                     (5+5)

 

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“Loyola College B.Sc. Chemistry Nov 2010 Organic Functional Groups – II Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – NOVEMBER 2010

CH 5505 – ORGANIC FUNCTIONAL GROUPS – II

 

 

 

Date : 29-10-10                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

 

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

 

  1. Explain why nitration of nitrobenzene is more difficult than that of benzene.
  2. Account for the fact that Nitromethane is acidic.
  3. Give the IUPAC name of
  4. CH3-NH-C2H5  ii.CH3-N(CH3) –CH3.
  5. What are diastereomers?Explain with an example.
  6. Explain Walden inversion using SN2 reaction.
  7. Show how will you prepare 3-methylpentanoic acid from diethyl malonate.
  8. What is Cope rearrangement.
  9. Give the products of the following reaction

    

    ii.

       

 

  1. What is isoprene rule?
  2. Write the structure of piperic acid.

 

PART – B

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

 

  1. Give the products obtained when Nitrobenzene is reduced electrolytically in
  2. Strongly acidic solution.
  3.   Strongly alkaline solution.
  4. Arrange the following in decreasing order of basicity giving suitable reasons.

       Aniline, p-Nitroaniline , m-Nitroaniline and  Diphenylamine.

  1. What is coupling reaction?Give the products obtained when benzene diazonium

      chloride reacts with i. phenol  ii. N, N-dimethylaniline.

  1. i. What is asymmetric synthesis?
  2. How will you prepare (-) lactic acid from pyruvic acid?
  3. Discuss the optical isomerism exhibited by biphenyl compounds.
  4. How will you synthesize n-butyric acid from ethyl acetoacetate?
  5. How will you synthesize propionic acid from acetic acid using Arndt – Eistert

      reaction.

  1. Describe Pinacole –Pinacolone rearrangement.Discuss its mechanism.
  2. Describe Curtius rearrangement and give its mechanism.
  3. Give the mechanism and orientation of electrophilic substitution in pyridine.
  4. How will you synthesize nicotine from nicotinonitrile.
  5. 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 marks)

 

  1. i. How is Nitrobenzene prepared from benzene? Give its mechanism.             (5)
  2. How will you prepare o-Nitroaniline and p-Nitroaniline from Aniline      .                                   (5)

 

  1. i. How is benzene diazonium chloride prepared in the laboratory. (4)
  2. Explain Gattermann and Sandmeyer reactions using suitable examples.                         (4)

      iii. How will you prepare Phenol from benzene diazonium chloride.                                                 (2)

 

25.i. Discuss Claisen  rearrangement with a specific example . Give its mechanism.                  (5)

  1. How will you prove that in Claisen rearrangement ,o-isomerisation takes place

         with inversion of position.                                                                                                                   (5)

 

  1. i. Describe any one method for the resolution of racemic mixtures.             (4)
  2. Explain by giving an example the phenomenon of racemisation.                                       (3)
  • Assign R and S configuration to the following Fischer projection.                  (3)

 

  1.                                                         iii.

                        

 

  1. i. How is Quinoline prepared by Friedlander synthesis using o-Amino benzaldehyde. (5)

      ii.Complete the following reactions.                                                                                                       (2)

        a.

           

 

        b.

           

       

      iii.Explain why pyridine is more basic than pyrrole?                                                                          (3)

28.i.What are Alkaloids? How are they extracted from plants.                                                                (5)

     ii.What are the structural formula and uses of

  1. Menthol b. α-Pinene  c. Camphor.                                                                                              (5)

 

 

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“Loyola College B.Sc. Chemistry Nov 2010 Organic Functional Groups – I Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – NOVEMBER 2010

CH 3502 – ORGANIC FUNCTIONAL GROUPS – I

 

 

 

Date : 30-10-10                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

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

 

  1. Arrange the following compounds in increasing order of reactivity towards SN2

          reaction. Give reasons.

          t-butyl chloride, n-propyl chloride.

 

  1. How is benzyl chloride prepared from benzaldehyde.

 

  1. Why does phenol have higher boiling point than toluene.

 

  1. Complete the reaction

 

           

 

  1. Give the IUPAC name of the following compounds

 

 

  1. How will you prepare phenyl methyl ether from phenol using Williamson’s synthesis?

 

  1. What happens when calcium acetate is heated? Give its equation.

 

  1. What is Norrish type –I reaction.

 

  1. What is trans esterification.

 

  1. Arrange the following in terms of increasing acid strength and give reasons.

           Propionic acid , 2chloropropionic acid , 2 fluoropropionic acid.

 

PART – B

Answer any EIGHT questions                                                                  (8 x 5 = 40)

  1. Give a mechanism for the reaction of tert.butyl bromide with aqueous NaOH to

  form tert.butyl alcohol.

  1. Explain Saytzeff rule and Hofmann rule with an example.
  2. How is phenol prepared from Cumene.
  3.    Although both phenol and alcohols contain hydroxyl group, Phenol is acidic    

            whereas aliphatic alcohols are not acidic – Explain.

  1. How will you prepare primary,secondary and teritiary alcohols from Grignard

            reagent.

  1. How is ethyl methyl ether prepared by Williamson’s synthesis.What  type of

            mechanism is followed.

  1. Write a short note on cleavage of ethers by acids.
  2. Discuss the mechanism of Cannizaro reaction.
  3. Explain crossed aldol condensation with an example.
  4. What is Wittig reaction ? Explain its mechanism.
  5. Discuss the geometric isomerism of unsaturated dicarboxylic acids.
  6. Explain the mechanism of alkaline hydrolysis of esters.

 

                                                        PART – C

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

 

  1. a) Explain the fact that allyl chloride undergoes substitution reaction by SN1 

                mechanism whereas n-propyl chloride reacts by SN2 mechanism.

  1.   b) Discuss the Mechanism of E1 and E2 reactions of alkyl halides.

                     

  1. a) Give the mechanism of Reimer Tiemann reaction and Kolbe’s reaction.
  2. b) How is phenolphthalein prepared from phenol?

 

  1. i. How is acetic acid converted to ethyl acetoacetate.
  2.          How would you prepare the following compounds from acrylic acid.
  3. Propionic acid.
  4. Glyceric acid.
  5. 2- bromo propionic acid.

 

  1. a) How is ethylene oxide prepared?
  2.     b) How does diethyl ether react with

                 i.O2/long contact    ii.PCl5

  1.  c) How does ethylene oxide react with the following reagents:
  2.        H2O/H+   ii. HBr   iii.CH3CH2OH  iv.NH3.

 

  1.   i. How will you prepare the following compounds
  2.               a) 2-propanol from CH3CHO
  3.             b) Lactic acid from CH3COCH3
  4.           Discuss the mechanism of Reformatsky reaction.         

 

  1. a) Write notes on Clemmensen reduction and Wolff-Kishner reduction.
  2. b) How will you synthesize cinnamic acid using Perkin’s and Knoevenagel

                reactions.

 

 

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“Loyola College B.Sc. Chemistry Nov 2010 Main Group Elements & Solid State Chemistry Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – NOVEMBER 2010

CH 3503 – MAIN GROUP ELEMENTS & SOLID STATE CHEMISTRY

 

 

 

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

Time : 9:00 – 12:00

PART – A

 

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

 

  1. Why does the basic strength of hydroxides of alkali metals increase on moving down the group?
  2. Beryllium and magnesium do not impart any colour to the flame. Why?
  3. What is meant by catenation?
  4. How does aluminium react with dilute mineral acids and strong alkali solutions?
  5. How is carbon suboxide prepared?
  6. Write the structure of caro’s acid.
  7. Give the preparation of perchloric acid.
  8. What are pseudohalogens? Give one example.
  9. Represent (110) plane of cubic structure.
  10. Calculate the relative sizes of the anions and cations required for a perfect fit of the cation into

the octahedral sites in a close packed anion array.

 

PART – B

 

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

 

  1. Explain the role of Na+ and K+ ions in biological system.
  2. Write briefly on anomalous behavior of lithium.
  3. What is Borax? How is it prepared?
  4. What are interstitial carbides? Explain with an example.
  5. Write a note on sulphides of phosphorus.
  6. Explain the preparation and structures of oxides of nitrogen.
  7. How is orthophosphoric acid prepared? Write its structure.
  8. How is available chlorine in bleaching powder estimated?
  9. How are dichlorine monoxide and iodine pentoxide prepared?
  10. Derive Bragg’s equation for X-ray diffraction.
  11. Explain the crystal structure of fluorite.
  12. How are seven solid systems, classified into Bravais lattices?

 

PART – C

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

 

  1. a) How is beryllium extracted from beryl? (6)
  2.  b) Give an account of  hydroxides and halides of s block elements                                            (4)
  3. Discuss the structures and properties of chain and sheet silicates.
  4. a) Give the preparation and uses of hydrazoic acid. (5)
  5.  b) How are superphosphate and triple superphosphate prepared?
  6. a) How are oxides classified? Give an example for each type. (5)
  7. b) Explain the structure of diborane. (5)
  8. What are interhalogen compounds? How are they classified? Explain the structures of
    ClF3 and IF5.
  9. a) Discuss (i) Frenkel defect and (ii) Schottky defect. (6)
  10. b) What are Miller indices. (4)

 

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“Loyola College B.Sc. Chemistry Nov 2010 Fundamentals Of Spectrascopy Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – NOVEMBER 2010

CH 5508 – FUNDAMENTALS OF SPECTRASCOPY

 

 

 

Date : 09-11-10                     Dept. No.                                                    Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

 

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

 

  1. Which electromagnetic radiation has wave length 1 m? Give the frequency of that

electromagnetic radiation.

  1. Explain signal-noise ratio.
  2. State Beer-Lambert’s Law.
  3. What are chromophores and auxochromes?
  4. Why water cannot be used as a solvent in IR spectral analysis?
  5. How will you distinguish intramolecular hydrogen bonding from intermolecular hydrogen

bonding by IR spectroscopy?

  1. Define coupling constant.
  2. Why is KMnO4(ag) coloured?
  3. What is the difference between base peak and molecular ion peak?
  4. If the m/e value of the molecular ion [M] is 173 and there is an [M+2] peak with equal

relative abundance, what are your inferences?

 

PART – B

 

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

 

  1. Distinguish between the following:
  2. Absorption spectra-emission spectra.
  3. Electronic energy levels-rotational energy levels.
  4. Write the principle of ASS and explain its instrumentation.
  5. Write the Boltzmann distribution formula and explain.
  6. ‘Isotopic peaks have a rich source of information’ – Justify.
  7. Enlist the factors that affect chemical shift values.
  8. Explain the different types of electronic transitions.
  9. Describe the various IR bands for ethyl benzoate.
  10. Using NMR spectroscopy, how will you differentiate between
  • 1-propanol and 2-propanol.
  • Acetone and acetaldehyde.
  1. Discuss mutual exclusion principle.
  2. Write a note on sample handling in IR spectroscopy.
  3. Can you distinguish CH3 CH2 OCH3 from (CH3)2 CHOH by PMR Spectroscopy?
  4. Explain the fragmentation pattern of n-butanol.

PART – C

 

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

 

  1. Draw the block diagram of double beam IR spectrometer and explain its components.
  2. List out the difference between (i) IR and Raman spectroscopy (ii) Stoke’s and antistoke’s

lines.

  1. a) What are the merits of TMS?
  2. b) Discuss the basic instrumentation in NMR.
  3. a) How will you determine the structure of a compound whose m/e value are 86 (molecular

ion), 57 (base peak), 29?

  1. b) What are the factors that affect absorption maximum and intensity in UV-visible

spectroscopy?

  1. Discuss the principle and applications of flame photometry.
  2. Explain a) MCLafferty rearrangement b) high resolution NMR Spectrum of ethanol.

 

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“Loyola College B.Sc. Chemistry Nov 2010 Concepts In Inorganic Chemistry Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – NOVEMBER 2010

CH 1503 – CONCEPTS IN INORGANIC CHEMISTRY

 

 

 

Date : 12-11-10                     Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

 

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

 

  1. Size of Cl– ion is greater than that of Chlorine atom – Explain.
  2. Define Ionisation energy.
  3. What is Aufbau principle?
  4. What is inert pair effect?
  5. Define bond order.
  6. What is Lewis concept of acids and bases?
  7. What are interstitial compounds?
  8. Explain why O2 is paramagnetic whereas O22– is diamagnetic.
  9. Which is more soluble in water MgSO4 or BaSO4? Why?
  10. Find the oxidation number of
  • Mn in KMnO4 2) S in  H2S2O8.

PART – B

 

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

 

  1. Explain the following processes
  2. Smelting  b) Froth floatation.                                                                                              (2+3)
  3. Define Electron affinity. Explain its trend across the period and down the group of periodic table.
  4. Describe the factors favouring the formation of covalent bond in reference to Fajan’s rule.
  5. Explain ‘Ellingham diagrams’.
  6. Lithium shows greater resemblance with magnesium than with other alkali metals.
  7. What are the postulates and limitations of Valence bond theory?
  8. Draw the M.O diagram for NO molecule and explain its magnetic behavior.
  9. What do you mean by inter and intra molecular hydrogen bonding?Discuss the effect of H-bonding on melting point and boiling point of substances.
  10. What are bonding and antibonding molecular orbitals?

 

  1. Write a note on clathrates.
  2. Explain Pearsons’s concept of hard and soft acids. Give examples.
  3. Balance the following chemical reaction by ion- electron method

MnO4– + C2O42– à Mn2+ + CO2   (in acidic medium).

 

PART – C

 

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

 

  1. What is electronegativity? How do you calculate electronegativity on the basis of
  2. Pauling’s approach        b) Mulliken’s approach                                                        (2+4+4)

 

  1. Define lattice energy and solvation energy. Describe how lattice energy of ionic solids is evaluated by Born-Haber cycle.

 

  1. Define Hybridisation. On the basis of hybridization discuss the geometry of the following molecules.
  • SF6        2) PCl5            3) NH3            4) XeF4                                                                   (2+8)

 

  1. a) Explain the postulates of VSEPR theory.                                                                                  (6)

 

  1. b) Differentiate between a σ bond and a π bond. With an example.             (4)

 

  1. a) Distinguish between cubic close packing and hexagonal close packing of spheres. (6)

 

  1. b) Give reasons for the following:

1) H2S is a gas H2O is a liquid

 

2) Diamond is a hard substance while graphite is soft.                                                       (4)

 

  1. Describe the following reactions in liquid ammonia giving suitable examples.

 

  1. a) Acid-base reactions
  2.    b) Precipitation reactions
  3.    c) Complex formation reactions
  4. d) Ammonolysis

 

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

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIRST SEMESTER – NOVEMBER 2010

CH 1502 – ANALYTICAL CHEMISTRY

 

 

 

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

Time : 1:00 – 4:00

 

PART – A

 

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

 

  1. What first aid will you do if a student spills phenol in his hands?
  2. Write answers on the basis of significant figures for the following:
  3. a) 7  +  0.08  +  2.9
  4. b) 20  X  127/10.8
  5. Name the types of adsorbents used in chromatography.
  6. Define Rf.
  7. Can we use phenolphthalein as indicator for the titration of Na2CO3 against HCl?
  8. Define the term normality.
  9. Mention the factors that influence precipitation.
  10. What are complexometric titrations? Give one example.
  11. Mention any two applications of TGA.
  12. What do you understand by the term ‘reaction interval’ in thermal analysis?

 

PART – B

 

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

 

  1. List out the differences between accuracy and precision.
  2. What are the advantages of a single pan balance over a double pan balance?
  3. When is distillation done under reduced pressure? Draw a sketch of a distillation set.
  4. Describe ‘hot filtration’ and give its significance.
  5. Write a note on gas chromatography.
  6. What are the conditions for a good primary standard?
  7. Find out the solubility product of silver chloride. Its solubility in water is

9.6 X 10-9 mol dm-3.

  1. Calculate the pH of a buffer solution containing 0.2M of acetic acid and 0.02 M of

sodium acetate. (Ka of acetic acid = 1.8 X 10-5 at 25oC)

  1. Discuss one theory of acid-base indicators.
  2. Explain adsorption indicators. Give examples.
  3. Explain homogenous precipitation with an example.
  4. Explain the thermal analysis of Ca(COO)2.H2O.

 

PART – C

 

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

 

  1. a) Write a detailed outline about the types of errors.                         (5)

 

  1. b) Find out the (i) mean (ii) median and  (iii) standard deviation for the

following data :  20.2, 19.3, 19.9, 21.5, 20.7.                                                                     (5)

 

  1. a) Explain the Principle and applications of column chromatography.             (5)

 

  1. b) Write briefly on ion exchange chromatography. (5)

 

  1. a) When is Soxhlet extraction resorted to? Explain its principle with a diagram. (5)

 

  1. b) Derive Henderson  equation for an acid buffer and mention its applications.                       (5)

 

  1. a) How is Chloride ion in a solution estimated? (any one method)                         (5)

 

  1.       b) Explain post precipitation.                                                                                                   (5)

 

  1. a) Explain Von Weiman ratio.                         (5)

 

  1.       b) What are the characteristics of metal-ion indicator?  Give an example.                      (5)

 

  1. a) Discuss on the various components for the instrumentation of DTGA. (5)

 

  1.       b)  Explain the factors that influence a thermogram.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

“Loyola College B.Sc. Chemistry April 2011 Transition Elements And Nuclear Chemistry Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – APRIL 2011

CH 5506 – TRANSITION ELEMENTS AND NUCLEAR CHEMISTRY

 

 

 

Date : 18-04-2011              Dept. No.                                                    Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

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

 

  1. Explain why most of the transition metals form coloured compounds.
  2. What are interstitial compounds? Give any two examples.
  3. What are actinides? Why are they so called?
  4. Name any two minerals of lanthanides.
  5. What is co-ordination number? Give an example.
  6. What are ligands? Explain with an example.
  7. Define radioactivity.
  8. What are pi-mesons and K-mesons?
  9. What are moderators? Give an example.
  10. Explain orbital electron capture.

 

PART – B

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

 

  1. Discuss the toxic effects of lead and mercury.
  2. How is titanium extracted from its ores?
  3. Explain the electronic spectra of lanthanide compounds.
  4. Explain the metallurgy of uranium.
  5. Explain spectrochemical series.
  6. What is chelate effect? Explain.
  7. Discuss Cis-trans isomerism in four coordinate square planar complexes.
  8. Calculate packing fraction, mass defect and energy released in the formation of argon atom 40Ar.   Isotopic mass of Ar = 39.96238 a.m.u.

18

  1. Discuss the shell model of nucleus on the basis of closed shells of magic number.
  2. Describe the working of G.M.counter.
  3. Differentiate between atom bomb and hydrogen bomb.
  4. Discuss the atomic power projects in India.

 

PART – C

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

 

  1. (a) Explain the preparation of            (i) TiCl3           (ii)  K2Cr2O7

(b)  Explain the biological importance of any two transition  elements.

 

  1. (a) Describe how lanthanides are separated  by ion-exchange chromatography.

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

 

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

(b)  Give possible isomers of  [CO(NH3)2(H2O)2Cl2]+.

 

  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)  Describe the functioning of scintillation counter.

 

  1. Explain the construction, working and applications of a nuclear reactor.

 

 

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

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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 2011 Sythetics Organic Chemistry And Spectroscopy Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS) CHENNAI – 600 034

B.Sc., DEGREE EXAMINATION – CHEMISTRY

SIXTH SEMESTER – APRIL 2011

CH 6609/6603 – SYTHETICS ORGANIC CHEMISTRY AND SPECTROSCOPY

DATE:11-04-2011                                                                                                                              MAX:100 MARKS

TIME:1:00 – 4.00

 

PART A

Answer ALL Questions                                                                                                                                  (10 x 2 = 20)

  1. What are activating groups? Give
  2. Suggest any two criteria for choosing protective groups?
  3. Complete the following reactions

O

  1.                                          H2

Pd / C

 

  1.   COOH

Na

Liq. NH3

  1. Mention the role of DMSO in oxidation reactions
  2. What is the structure of aldol product from propanal?
  3. What is the significance of active methylene group?
  4. Calculate the lmax for the following

 

 

O

  1. C – CH3

 

  1. The lmax of benzene is 256nm whereas aniline is 280nm – Give reason.
  2. Predict the structural formula for the compound with the following molecular formula showing only one NMR signal a) C2H6O b) C5H12
  3. Define nitrogen rule. Give an example.

 

 

 

 

PART B

Answer any EIGHT Questions                                                                                                                    (8 x 5 = 40)

  1. Explain Retrosynthetic analysis.
  2. What do you understand by linear and convergent synthesis? Explain.
  3. Discuss synthon approach in construction reactions.
  4. Discuss the mechanism of Clemmenson reduction and mention its significance.
  5. Explain hydroboration reaction and mention the utility of the rection.
  6. Explain Diels Alder reaction. Give any two examples.
  7. Complete the following reaction

O

+ C6H5CHO                NaOH

 

CHO

 

 

  1. NaBH4

 

OCH3                                    CH3OH

                                                           

  1. B2H6
  2. CH3 – (CH2)7 – CH = CH2
  3. H2O2
  4. What are chromophores and auxochrome? Give examples.
  5. Discuss the factors which affect the IR absorption frequency of a functional group.
  6. Define chemical shift. Why is TMS a good reference standard in NMR spectroscopy.
  7. How will you distinguish 2-pentanone and 3-pentanone using mass spectroscopy.
  8. Explain shielding and deshielding mechanism.

 

PART C

Answer any FOUR Questions                                                                                                                     (4 x 10 = 40)

  1. a) Explain umpolung synthesis.                                                 (5)
  2. b) Using umpolung synthesis convert the following reaction.                                 (5)

O                                                                  O

nC5H11 – C – H                                               C5H11 – C – CH2 – R

  1. a) How will you distinguish the following pairs using IR spectroscopy.                                 (6)
  2. CH3 – CO – CH3 and CH3 – CH = CH – CH2OH
  3. O-hydroxy benzaldehyde and m- hydroxy benzaldehyde
  4. b) Draw the structure of each of the following compounds which meets the given requirements in the NMR spectrum.                                 (4)
  5. C3H3Cl5 (one doublet and one triplet) ii. C3H7Cl (one doublet and one septet)
  6. a) Explain spin-spin spliting with a suitable example.                                 (6)
  7. b) A compound with molecular formula C8H8O gives the following NMR spectrum – multiplet
    d28 (5H), Doublet d 2.88 (2H), Triplet d 9.87 (1H). Determine its structure (4)
  8. Using malonic ester how will you synthesis the following.
  9. Succinic acid           Adipic acid
  10. Cinnamaldehyde             n-Valeric acid.
  • Barbituric acid.
  1. a) An organic compound with molecular weight 72 absorbs at 274 nm.

In IR the bands are formed at 1715 cm-1 (s), 2941 – 2857 cm-1(m) and 1460 cm-1 (m).

In NMR the signals  formed are 2.48 d quartet (2H), 2.12 d singlet (3H), 1.07 d triplet (3H). Determine the structure of the compound.

b)Define the following terms and mention its significance                                                            (4)

  1. Base Peak ii. Metastable peak
  2. a) Discuss the instrumentation of UV –Visible spectrophotometer with the block diagram.(6)
  3. b) How are the following groups protected and deprotected during organic synthesis (4)                        – NH2                 ii.             C = O                     iii.  – OH                iv.  –  COOH

 

 

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

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – APRIL 2011

CH 5402/5400 – POLYMER CHEMISTRY

 

 

Date : 12-04-2011              Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

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

  1. How are polymers classified on the basis of their origin?
  2. What are reinforced plastics? Give an example.
  3. Distinguish between organic and inorganic polymers.
  4. How is polystyrene prepared?
  5. What is coordination polymerization? Give an example.
  6. What are the causes of chain end degradation?
  7. What is ion-pair precipitation?
  8. Account for the thermal stability of PTFE.
  9. What are addition and condensation polymerizations?
  10. Mention the significance of organosols.

 

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

  1. Explain Natta’s bimetallic mechanism of polymerization.
  2. Discuss the different types of polycondensation.
  3. Explain copolymerization and homopolymerisation with examples.
  4. What are zipping and unzipping? Give examples.
  5. Explain interfacial condensation polymerization with an example.
  6. Give the preparations and applications of LDPE and HDPE?
  7. How are linear and cross-linked phenol-formaldehyde resins obtained?
  8. Explain inter and intra molecular chain transfer.
  9. How will you remove the defects in polypropylene polymer?
  10. Describe polyaddition polymerization with an example.
  11. Discuss the mechanism of anionic polymerization.
  12. How are isotactic and syndiotactic polymers obtained?

 

 

 

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

  1. a) Discuss the primary and secondary bond forces present in polymer   (6)
  1. b) Chain polymerization is also called vinyl polymerization – explain. (4)
  1.  Why is the molecular weight of a polymer expressed as an average? Describe the   weight average molecular weight determination of a polymer.
  2. a) Explain the various possible modes of addition in the propagation step of free radical polymerization.                                                                             (6)
  1. b) Why are inhibitors called short stops? Mention their uses. (4)
  1.  a) Explain i) Blow moulding  ii) Injection moulding                              (6)
  1. b) Write a note on compounding. (4)
  1. a) Discuss the role of metering and feed zones in extrusion moulding.   (5)
  1. b) Writ a note on elastomeric materials and fibre forming polymers. (5)
  1. Discuss the mechanisms of conduction exhibited by polyphenylene and polyacetylene polymers.

 

 

 

 

 

“Loyola College B.Sc. Chemistry April 2011 Phase Equilibria And Kinetics Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – APRIL 2011

CH 5507 – PHASE EQUILIBRIA AND KINETICS

 

 

 

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

Time : 1:00 – 4:00

 

SECTION –A

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

  1. The fusion curve of ice in the phase diagram of water is inclined towards the pressure axis. Account for this phenomena.
  2. State phase rule and mention the terms involved in it.
  3. Define zero order reaction. Give an example.
  4. Bring out the differences between order and molecularity of a reaction.
  5. “Addition of a non-volatile solute lowers the vapour pressure of a solution” – Offer a theoretical explanation for this statement.
  6. What do you mean by abnormal Colligative properties?
  7. State the steps that are involved in the thermal decomposition of acetaldehyde.
  8. Explain how ionic strength affects the rate of a reaction.
  9. What is a pseudo order reaction?
  10. Define the term ‘Adsorption’.

SECTION –B

Answer ANY EIGHT questions                                                                                (8 x5 = 40 MARKS)

  1. Apply phase rule to sulphur system.
  2. Explain phase rule to lead-silver system and discuss the desilverisation of lead from this system.
  3. Define osmotic pressure. Derive a relationship between osmotic pressure and lowering of vapour-pressure.
  4. If a solution containing 6g of triphenyl methane(mol.wt=244) in 1000g of benzene is cooled to 22°C below the freezing point of benzene, how much solvent will crystallize out ?

( Kf = 5.1 K kg mol-1)

  1. Derive the expression for the rate constant for the reaction 2A → products.
  2. Why do the rates of reactions in general have a large temperature co-efficient?
  3. The specific reaction rate of a reaction is 1 x 10-3 min-1 at 27°C and 2×10-3 min-1 at 37°C. Calculate the energy of activation of this reaction and its specific reaction rate at 47°C.
  4. Explain i) consecutive reaction ii) parallel reaction with one example for each.
  5. Explain the theory of absolute reaction rate and show how it is superior to other theories.

 

 

  1. Derive Nernst distribution law and state its limitations.
  2. State and explain the factors that affect the rate of enzyme catalysis.
  3. What are Wilkinson’s catalysts? Explain its catalytic action in reactions.

 

SECTION –C

Answer any FOUR the questions                                                                               (4 x 10 = 40 MARKS)

  1. Draw and explain the phase diagram of FeCl3-H2O system.
  2. (a) How are volumetry, monometry, useful in studying the reaction kinetics. Give one example for each.

(b) Explain the mechanism of SN1 reaction.

  1. Explain Lindemann’s steady state principle. Show that the reaction is first order at high concentration and second order at low concentration. Derive the relevant expression.
  2. (a) State Raoult’s law. Explain the different types of deviation from this law.

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

  1. Explain with a suitable diagram that lowering of vapor pressure is the cause for change in boiling point and freezing poing of a solution.
  2. State the postulates of Langmuir’s adsorption equation and discuss the effects at very low and high pressures.  Derive the equation.

 

 

 

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“Loyola College B.Sc. Chemistry April 2011 Organic Functional Groups – I Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – APRIL 2011

CH 3502/CH 4500 – ORGANIC FUNCTIONAL GROUPS – I

 

 

 

Date : 12-04-2011              Dept. No.                                                    Max. : 100 Marks

Time : 1:00 – 4:00

 

SECTION-A

ANSWER ALL QUESTIONS                                                                   (10×2=20)

  1. What is Saytzeff’s rule? Give an example.
  2. What is Sandmeyer reaction?
  3. What is Clemmensen reduction?
  4. What happens when acetone is treated with I2 and NaOH?
  5. Name the products obtained when anisole is treated with HI.
  6. Explain why anisole cannot be prepared by the reaction of phenyl iodide and

sodium methoxide.

  1. What is crossed Cannizzaro reaction?
  2. How do you convert benzaldehyde  into cinnamaldehyde?
  3. What is transesterification?
  4. How is succinic acid prepared? Name the product obtained  when it is

heated.

 

SECTION-B

  ANSWER ANY EIGHT QUESTIONS                          (8×5=40)

  1. Compare SN1 and SN2 reaction mechanisms.
  2. Write notes on Wurtz-Fittig reaction.
  3. How are alcohols prepared by hydroboration? Give  an example.
  4. Why o-nitrophenol has a lower boiling  point  than p-nitrophenol?
  5. How do you convert phenol into
  6. a) picric acid b) salicylaldehyde

 

  1. Discuss the mechanism of cleavage of ethers by HI.
  2. Explain Williamson’s synthesis of ethers.
  3. Discuss Norrish type-I reaction.
  4. Discuss the mechanism of Wittig reaction and its uses in organic synthesis.
  5. Explain Wolf-Kishner reduction with its mechanism.
  6. Give any two methods of preparation of adipic acid.
  7. Discuss the mechanism of acid catalysed hydrolysis of esters.

 

SECTION-C

       ANSWER ANY FOUR QUESTIONS                             (4×10=40)

 

  1. Discuss the E1 mechanism for elimination reactions of alkyl halides.
  2. a) Why p-nitrophenol is more acidic than phenol whereas p-cresol is less

acidic than phenol?                                                                                     (6)

  1. b) What will be the product obtained when  p-cresol is treated with

CH3COCl  and AlCl3. Give reason.                                                          (4)

  1. a) Explain why epoxides are more reactive than ethers. (4)
  2. b) Name the products obtained when ethylene oxide is treated with

i)H2O/H+          ii)C2H5OH/H+                iii)NH3                                              (6)

  1. Discuss the following reactions.
  2. a) Benzoin condensation b) Reformatsky reaction (5+5)
  3. How will you bring about the following conversions?
  4. i) Salicylic acid into aspirin ii) Malonic acid into carbon suboxide

iii) Phthalic acid into phthalimide    iv) lactic acid into pyruvic acid

(v) acrylic acid into acrylamide.

  1. a) Explain Norrish type-II reaction with an example.
  2. b) How do maleic and fumaric acids differ in their properties?                     (5+5)

 

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