B.Sc. Chemistry Question paper

“Loyola College B.Sc. Chemistry April 2008 Adv. General Chemistry For Phys.& Maths Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

GH 9

 

B.Sc. DEGREE EXAMINATION – MATHEMATICS & PHYSICS

THIRD SEMESTER – APRIL 2008

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

 

 

 

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

Time : 1:00 – 4:00

PART A

Answer all the questions                                                                                      10 x 2 = 20

  1. Why the molecular weight of acetic acid in benzene is 120?
  2. ‘Ethanol is soluble in water but not thiol’. Why?
  3. Draw the resonance structures of thiophene.
  4. How is aspirin prepared? Give the equation.
  5. Define enthalpy of combustion with an example.
  6. Define equivalent conductance.
  7. How is the presence of –OH groups in fructose determined?
  8. Give an example for the optical specificity of an enzyme.
  9. What is the role of humus in agricultural chemistry?
  10. How is DDT prepared?

PART B

Answer any eight questions                                                                                  8 x 5 = 40

  1. What are the types of hydrogen bonding? Explain with examples.
  2. How is lanthanides extracted by ion exchange method?
  3. Write a note on the following.
  4. a) Vat dyes b) direct dyes.
  5. How is naphthalene prepared by Haworth synthesis?
  6. State Hess’s law and explain how the law is used to calculate the enthalpy of a reaction.
  7. How is malachite green prepared?
  8. Draw and explain saturated calomel electrode.
  9. How is conductometric titration helpful for the precipitation titrations?
  10. How is N-terminal of an amino acid determined by Sanger’s method?
  11. What is competitive inhibition? Explain with an example.
  12. Explain the different types of soil.
  13. Discuss the principle involved in the nuclear fission reaction.

PART C

Answer any four questions                                                                                4 x 10 = 40

 

  1. a) Explain the lanthanide contraction.
  2. b) Explain the mechanism of bromination of naphthalene.               (4+6)
  3. What are chemotherapeutic drugs? Explain with examples.
  4.       Define lattice energy. How is it determined?
  5. a) Derive Kirchoff’s equation.
  6. b) The molar conductance of sodium acetate, hydrochloric acid and sodium chloride at infinite dilution are 91.0´10-4, 426.16´10-4 and 126.45´10-4 Sm2mol-1 respectively at 25° Calculate the molar conductance at infinite dilution for acetic acid.                                  (6+4)
  7. a) Describe the secondary structure of proteins.
  8. b) What are the factors affecting the enzymatic activity? Explain.                (6+4)
  9. Explain the role of macro and micro nutrients in agricultural chemistry.

 

 

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“Loyola College B.Sc. Chemistry Nov 2008 Transition Elements And Nuclear Chemistry Question Paper PDF Download”

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DB 11

 

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FIFTH SEMESTER – November 2008

CH 5506 – TRANSITION ELEMENTS AND NUCLEAR CHEMISTRY

 

 

 

Date : 05-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

 

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

 

  1. Explain Goldschmidt thermite process.
  2. List out two uses of vanadium
  3. Orbital contributions to magnetic moments of lanthanide ions are significant. Why?
  4. The +3 oxidation state is the characteristic oxidation state of lanthanides. Account for.
  5. Write the IUPAC names of i.[Co(NH3)5CO3]Cl ii.Na[B(NO3)4].
  6. [Zn(NH3)4 ] 2+ cannot be a square planar complex. Why?
  7. What is K-electron capture?
  8. Write down the mathematical expression of Geiger-Nuttal’s rule.
  9. Bring out the relationship between the efficiency of a nuclear reaction and nuclear cross section.
  10. Why is technetium 99 m is used for diagnostic purposes ?

 

 

PART – B

 

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

 

  1. How is potassium dichromate prepared?
  2. Give an account of toxicity of mercury.
  3. Describe the methods of separation of lanthanides.
  4. Write briefly on the oxidation states exhibited by actinides. Why do they have greater tendency to

form complexes compared to lanthanides?

  1. Explain EAN rule and predict the formula of chromium carbonyl assuming that it obeys EAN rule.
  2. Sketch the possible geometric isomers for [Cr(NH3)2Cl4 ]– .Which of these will exhibit optical

isomerism?

  1. For the complex ion, [Cr(H2O)6]2+, the pairing energy is found to be 23500 cm-1. The value of Δo is

13900 cm-1. Calculate the crystal field stabilization energy for the complex in weak field and strong

field states.

  1. Write a note on the applications of radioactive isotopes in agriculture and biology.
  2. Describe the functioning of scintillation counter.
  3. What is binding energy? Explain with an example.
  4. Describe the process of spallation.
  5. What is isotopic dilution analysis? How is it carried out?

 

 

PART – C

 

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

 

  1. Explain how titanium is extracted from its ores. Mention two used of titanium. (10)
  2. What is lanthanide contraction? What are its consequences? (10)

 

  1. a. What are the postulates of valence bond theory, as applied to coordination compounds? Bring out

its defects.                                                                                                                                    (6)

  1. Draw VB diagram and indicate the type of hybridization in [Ni(CN)4]2-                                   (4)
  2. a. How are d-orbitals split, when a transition metal ion is placed in i. an octahedral field and
  3. a tetrahedral field?    (5)
  4. With the help of crystal field theory explain the given values of magnetic moments of the

following complexes:  i. K3[Fe F6 ]  5.9 μ (B.M)    ii. [Ni(H2O)6]Cl2  2.8 μ (B.M.)                   (5)

  1. Discuss the nuclear shell model and mention the defects of such a model.
  2. Write notes on : i. Nuclear fusion and ii. Theory of β decay.  (5+5)

 

 

 

“Loyola College B.Sc. Chemistry Nov 2008 Polymer Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

 

DB 15

 

FIFTH SEMESTER – November 2008

CH 5402/CH 5400 – POLYMER CHEMISTRY

 

 

 

Date : 12-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART-A                                       

 

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

 

  1. What are natural polymers and how do they differ from synthetic ones?
  2. Define inorganic polymers.
  3. What are polycondensation polymers? Give only the names of the monomers used for the synthesis of polyamide .
  4. Write any four characteristic features of anionic polymerization.
  5. What is bulk polymerization? Mention any two drawbacks of bulk polymerization.
  6. Why is the thermal stability of Teflon high?
  7. How are the following serve as initiators?

(a) benzoyl peroxide           (b) azobisisobutyronitrile.

  1. How is polystyrene prepared?
  2. What are antioxidants? Give any two examples.
  3. How does the reinforcement affect the properties of rubbers and plastics?

 

PART-B

 

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

 

  1. Define the following with example for each (a) Oligomers     (b) Elastomers
  2. Suggest ways to help make the synthetic polymers eco-friendly.
  3. Distinguish addition polymerization and condensation polymerization reactions.
  4. Describe the kinetics of chain polymerization by free radicals.
  5. Write short notes on gas phase polymerization.
  6. Explain the factors influencing the stability of polymers.
  7. Write short notes on (a) ring opening polymerization (b) living polymers.
  8. Mention the steps involved in the formation of bakelite and explain.
  9. How are the following polymers synthesized?

(a) HDPE       (b) Neoprene

  1. Explain the role of the following with example:

(a) Plasticizers  (b) Fire retardants

  1. Explain the process of calendaring.
  2. Discuss the stages involved in and importance of blow moulding.

 

 

PART-C                                                 

 

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

 

  1. Discuss the importance of secondary bond forces in polymers with suitable example

for each case.

  1. Write mechanism of Ziegler Natta polymerization. How is the growing chain

terminated?  Why are stereo-regular polymers obtained from it?                                       (6+2+2)

  1. Explain the mechanism of emulsion polymerization.
  2. Discuss the different types of polymer degradation and explain any one methods of

prevention for each type.

  1. What are conducting polymers? What are their characteristics of conducting

polymers?  Explain with the conductance value for polysulphurnitriles, polyphenylene,

poly pyrrole and polyacetylene.                                                                                          (2+4+4)

  1. Explain three major techniques of FRP and mention their applications?

 

 

 

 

 

 

 

 

 

 

“Loyola College B.Sc. Chemistry Nov 2008 Physical Chemistry – II Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

DB 17

 

FIFTH SEMESTER – November 2008

CH 5500 – PHYSICAL CHEMISTRY – II

 

 

 

Date : 03-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

 

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

 

  1. What is a reference electrode? Give an example.

 

  1. Define EMF.

 

  1. What is meant by Hydrogen over voltage?

 

  1. Calculate the ionic strength of 0.1M KCl.

 

  1. Define order of a reaction.

 

  1. What is a Psuedo-unimolecular reaction? Give an example.

 

  1. Mention any two factors affecting the enzyme catalysis?

 

  1. What is adsorption? Give an example.

 

  1. Define quantum yield.

 

  1. What is chemiluminesence?

 

PART – B

 

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

 

  1. Explain the experimental method of determining the standard reduction potential

of Zn electrode.

 

  1. Explain the working of Weston cell.

 

  1. Calculate the EMF of the following electrochemical cell at 25oC.

 

Cu, Cu2+ (a = 0.1 M)  ||  H+ (a = 0.01M),  H2(0.95 atm); Pt Eoxd cu2+| cu 0.34 volt

 

  1. Discuss briefly the principle of polarography.

 

  1. Explain the term decomposition potential. Discuss its application.

 

  1. How is order of a reaction determined experimentally using half life method?

 

  1. Explain the kinetics of unimolecular reaction using Luidemann theory.

 

  1. Calculate the activation energy of a reaction whose rate constant is tripled by a 10oC rise in temperature in the vicinity of 27oC.

 

  1. Derive Langmuir adsorption isotherm.

 

  1. Discuss the general characteristics of catalytic reaction.

 

  1. Derive an expression for rate constant of a second order reaction with equal concentration of

reactants.

 

  1. Explain the basic concepts of photosensitized reactions.

 

PART – C

 

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

 

  1. a) Derive the Nernst equation for a cell reaction.                       (5)

 

  1. Derive the emf of a concentration cell with transference. (5)

 

  1. a) Explain the determination of pH using quinhydrone electrode.  (5)

 

  1. b) How will you prove electrochemically that mercurous ion exists as Hg22+   (5)

 

  1. Explain Debye Huckel Theory of strong electrolytes.

 

  1. Explain the collision theory of bimolecular reactions. What are its limitations.

 

  1. a) Explain the influence of ionic strength on the rates of ionic reactions.  (5)

 

  1. b) Discuss on Absolute reaction rate theory.                                               (5)

 

  1. Derive Michaelis – Menton equation for a single substrate enzymatic reaction and explain.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

“Loyola College B.Sc. Chemistry Nov 2008 Physical Chemistry – I Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION – CHEMISTRY

DB 06

 

THIRD SEMESTER – November 2008

CH 3500 – PHYSICAL CHEMISTRY – I

 

 

 

Date : 06-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

PART – A

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

 

  1. State the first law of thermodynamics.

 

  1. Write Van der Waals equation for ‘n’ moles if a gas.

 

  1. Distinguish between state function and path function.

 

  1. Explain the term Eutectic point with an example.

 

  1. Define the congruent melting point.

 

  1. Explain the term degrees of freedom.

 

  1. What are azeotropes? Give an example.

 

  1. State Raoult’s law.

 

  1. Find the molal elevation constant of water which evaporates at 100oC with the absorption of 40669.2 J per mole (R = 8.134 J K-1 mol-1).

 

  1. 0.1 M aq. solution of KNO3 shows an osmotic pressure of 4.5 atm at 300K, while the calculated one is 2.5 atm. What is the Van’t Hoff factor ‘i’ for the solution.

 

PART – B

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

 

  1. State the postulate of the Kinetic theory of gases.

 

  1. Define Cp and Cv. Derive the relationship between them for an ideal gas.

 

  1. Prove that TVγ-1 = constant for an adiabatic expansion of an ideal gas.

 

  1. Calculate the entropy of mixing of one mole of oxygen gas and two moles of hydrogen gas, assuming that no chemical reaction occurs and the gas mixture behaves ideally.

 

  1. Derive Clausius-Calpeyron equation.

 

  1. Draw and explain the phase diagram of water system.

 

  1. Give the general account of three components system.

 

  1. Derive thermodynamically the Gibb’s phase rule.

 

  1. Discuss the principle and application of Fractional distillation.

 

  1. Explain the effect of adding NaCl to the CST of phenol water system.

 

  1. Discuss the Van’t Hoff’s theory of dilute solutions.

 

  1. The molar heat of vaporisation of water at 1000 C is 40.585 kJ mol-1. At what temperature will a solution containing 5.60 g of glucose per 1000 g of water boil?

 

PART – C

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

 

  1. a) Derive Kirchoff’s equation.                            (5)

 

  1. b) Explain Joule-Thomson effect.                       (5)

 

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

 

  1. b) Derive Gibb’s Helmholtz equation.                            (5)

 

  1. a) Explain the phase diagram of Pb-Ag system.             (4)

 

  1. b) The vapour pressure of water at 100oC is 760 mm. What will be the vapour pressure at 95oC?  The heat of vaporisation of water in this temperature range is 41.27 kJ per mole.

(6)

  1. Discuss the phase diagram of formation of compound with congruent melting point.

 

  1. a) State and explain the Henry’s law.   How is it related to Raoult’s law?                    (5)

 

  1. Write notes on steam distillation. (5)

 

  1. a) Derive thermodynamically nernst distribution law.                                                    (6)
  2. b) Explain one of its applications.                                                                                   (4)

 

 

 

“Loyola College B.Sc. Chemistry Nov 2008 Phase Equilibria And Kinetics Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

   B.Sc. DEGREE EXAMINATION – CHEMISTRY

DB 12

 

FIFTH SEMESTER – November 2008

CH 5507 – PHASE EQUILIBRIA AND KINETICS

 

 

 

Date : 07-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART A

Answer ALL the questions                                                                        10X2=20

 

  1. What is condensed phase rule equation.
  2. Find out the number of components in           (i) CaCO3(s) CaO(s)+ CO2(g)

(ii)NH4Cl(s)  NH3(g)  + HCl(g)

  1. Define vapour pressure of a liquid?
  2. Give two limitations of Nernst distribution law.
  3. Distinguish between order and molecularity.
  4. Give an example each for first order and zero order reactions
  5. How does ionic strength affect the rate of a reaction?
  6. What is adsorption?
  7. Cite an example for homogeneous and heterogeneous catalysis.
  8. Mention the characteristic features of enzyme catalysis.

 

PART B

Answer any EIGHT questions                                                                     8X5=40

 

  1. The melting point of ice is higher than that of ice mixed with salt. Why?
  2. Discuss the salient features of the phase diagram of Pb-Ag system
  3. How will you obtain absolute alcohol from rectified spirit?
  4. 1.1 g of a protein were dissolved in 100 mL of solution. The osmotic pressure at 25˚C was measured as 1150 Nm-2. What is the molar mass of the protein?
  5. Describe any one method of determination of order of a reaction.
  6. Obtain the integrated rate equation for a second order reaction 2Aproducts.
  7. Compare and contrast absolute reaction rate theory and collision theory.
  8. A first order reaction has a half life of 30 minutes at 27˚C. Its rate constant at 47˚C is 1.15X10-3 sec-1. Calculate the energy of activation.
  9. Derive Langmuir’s adsorption isotherm equation.
  10. Explain kinetics of bimolecular surface reactions with one example.
  11. Discuss the significance of     (i) Raoult’s law

(ii) Henry’s law

  1. Enumerate the steps involved in thermal dissociation of acetaldehyde.

 

 

PART C

Answer any FOUR questions                                           4X10=40

 

  1. Derive Michaelis Menten equation for the kinetics of enzyme catalysis.
  2. Explain Lindemann hypothesis with reference to the kinetics of unimolecular reactions.
  3. (a) At 27°C in the presence of a catalyst, the activation energy of a reaction is lowered by 2 k cal. Calculate by how many times the rate of the reaction increases by the presence of this catalyst.            (5)

(b) Differentiate physisorption from Chemisorption.                        (5)

  1. (a) Draw the phase diagram of water system and explain.                 (5)

(b) Derive Nernst distribution law                                                      (5)

  1. (a) Discuss the principle and experimental method involved in fractional

Distillation of a binary liquid mixture.

(b) Derive phase rule equation                                                            (5)

  1. Derive thermodynamically the relation between elevation in boiling point and morality.

 

 

 

“Loyola College B.Sc. Chemistry Nov 2008 Organic Functional Groups – I Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

DB 07

 

   B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – November 2008

CH 3502 / CH 4500 – ORGANIC FUNCTIONAL GROUPS – I

 

 

 

Date : 06-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

 

PART – A

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

 

  1. How is 1-bromo-2-methylpropane prepared from 2-methylpropene?
  2. Write one example each for a)SN1 and b)SNAr reactions.
  3. How are the following distinguished using a characteristic chemical test?

a)benzyl alcohol & ethanol     b)phenol & benzyl alcohol

  1. How is benzene converted into p-nitrophenol?
  2. Write the IUPAC name for a)anisole b)methyl isopropyl ether.
  3. How is methyl isopropyl ether prepared using Williamson’s method?
  4. Write one example each for a)Norish type-I reaction and b)Wolf-Kishner reduction.
  5. Write equations to explain the preparation of a)propan-1-ol using ethanal.
  6. Write IUPAC names for a)oxalic acid and b)cinnamic acid.
  7. What is trans-esterification? Write one example.

 

 

PART – B

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

 

  1. Explain the difference in stereochemistry between n-butyl iodide and t-butyl iodide during nucleophilic substitution reaction, by writing suitable mechanisms.
  2. What happens when ethyl iodide is reacted with: a)alc KOH b)alc AgCN c)sodium phenoxide  d)moist silver oxide  e)sodium acetate?
  3. Write a suitable mechanism for hydroboration – oxidation reaction. (3)

Explain how 2-phenylethanol prepared by this method.                                (2)

  1. a)Arrange the following in the increasing order of acidity: ethanol, methanol, benzyl alcohol and phenol.             (2)

b)Explain why sodium phenoxide is a weaker base than sodium ethoxide.   (3)

  1. How is phenol converted into a) salicylaldehyde b) benzene c)aspirin         (2+1+2)
  2. Predict the major product when propene oxide is reacted with a)NaNH2 / NH3

b)H3O+                                                                                                           (5)

  1. Write a suitable mechanism for Williamson’s synthesis                                  (5)
  2. How are the following converted? a)CH3CH2OH à CH3CH=CHCHO

b)CH3COOH à CH3COCH3  c)C6H5CHO à C6H5CH=CH2                     (2+1+2)

  1. How would you distinguish the following? a)methanol & ethanol b)methanal & benzaldehyde  c)acetophenone & benzaldehyde                                                                    (1+2+2)

 

  1. Write a suitable mechanism for Cannizaro reaction. Identify the rate determining step.

(4+1)

  1. How is benzaldehyde converted into benzoin? Write equation. (3)

In which case the α-hydrogen is more acidic between ethanal and propanone.  Why? (2)

  1. How are the following compounds prepared? a)acetic acid into malonic acid b)phthalic acid from naphthalene  c)propanoic acid into acrylic acid.                                 (2+1+2)

 

 

PART – C

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

 

  1. A)Point out the differences between SN1 & SN2 reactions with respect to

a)effect of using a polar solvent  b)kinetics  c)reactivity of alkyl halides.             (6)

B)How is n-propyl bromide prepared from a)propene b)ethyl bromide         (1.5 + 2.5)

  1. A)How are the following compounds prepared from ethanol? a)CHI3 b)ethanoic acid  c)phenyl ethanoate  d)ethyne  e)methanal                                                              (5 x 2 =10)
  2. A)How is ethane oxide prepared? (4)

B)Write a suitable mechanism for the reaction:

CH3CHO + CH3CH2CHO à CH3CHOHCH(CH3)CHO                 (6)

  1. A)Write a note on a)Jablonskii diagram b)use of a cyanohydrin (3+3)

B)Predict the product when alkaline KMnO4 is reacted with maleic acid and fumaric acid.

(2+2)

  1. A)Arrange the following in the increasing order of pKa values:

benzoic acid, o-nitrobenzoic acid, m-nitrobenzoic acid and p-nitrobenzoic acid. (4)

B)How are the following prepared from acetyl chloride?  a)ethanal  b)acetophenone

c)acetic anhydride                                                                                                   (6)

  1. A)What happens to the acid strength along the homologous series of carboxylic acids?

Explain.                                                                                                           (1+3)

B)Write note on the following: a)Knoevenagel reaction  b)action of heat on α, β and γ-hydroxy acids  c)Use of Zn-Hg / HCl in organic synthesis.                                      (3×2=6)

 

 

 

 

“Loyola College B.Sc. Chemistry Nov 2008 Mathematics For Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

 

AB 04

 

THIRD SEMESTER – November 2008

MT 3103/MT 3101 – MATHEMATICS FOR CHEMISTRY

 

 

 

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

Time : 9:00 – 12:00

Section A

Answer ALL questions:                                                                             (10 x 2 = 20)

  1. If, find.
  2. Find the slope of at (2, 4).
  3. Integrate with respect to x.
  4. Solve
  5. Prove that
  6. If  , show that
  7. Simplify.
  8. Expand tan 6θ in terms of tanθ.
  9. Find the arithmetic mean of the following frequency distribution:

x:         1          2          3          4          5          6          7

f:          6          10        11        15        11        12        10

  1. Define the probability mass function of binomial distribution.

 

Section B

Answer any FIVE questions:                                                                    (5 x 8 = 40)

  1. Determine the maxima and minima of.
  2. Find the equation of the tangent and normal to the curve at.
  3. Evaluate (a); (b).
  4. Show that

 

  1. Find the sum to infinity the series.
  2. Expand in terms.
  3. Two unbiased dice are thrown. Find the probability that:
  • Both the dice show the same number,
  • The first die shows 6,
  • The total of the numbers on the dice is 8.
  • The total of the numbers on the dice is greater than 8.
  1. A car hire firm has two cars, which it hires out day by day. The number of demands for a car on each day is distributed as a Poisson distribution with mean 1.5. Calculate (i) the proportion of days on which neither car is used, and (ii) the proportion of days on which some demand is refused.

 

Section C

Answer any TWO questions:                                                                   (2 x 20 = 40)

 

  1. (a) Find the angle of intersection of the cardioids  and                                         .

(b) If, prove that.                  (12 + 8)

  1. (a) Evaluate .

(b) Integrate  with respect to x using Bernoulli’s formula.

(c) Solve .                                                                     (8 + 4 + 8)

  1. (a) Sum to infinity the series .

(b) Find the characteristic roots and the characteristic vectors of the matrix

 (8 + 12)

  1. (a) Prove that.

(b) If  in  show that.                   (10 + 10)

 

 

“Loyola College B.Sc. Chemistry Nov 2008 Main Group Elements & Solid State Chemistry Question Paper PDF Download”

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DB 08

 

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

THIRD SEMESTER – November 2008

CH 3503 – MAIN GROUP ELEMENTS & SOLID STATE CHEMISTRY

 

 

 

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

Time : 9:00 – 12:00

 

PART – A

 

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

 

  1. Lithium forms normal oxide while sodium forms peroxide. Account for.
  2. When sodium is shaken with naphthalene in nonaqueous solution it turns paramagnetic. Why?
  3. What is meant by catenation?
  4. What are interstitial carbides?
  5. Give the preparation of metaphosphoric acid.
  6. How is hydroxylamine prepared?
  7. Give the preparation of perchloric acid.
  8. Iodine pentoxide is used to determine carbon monoxide. Why?
  9. Distinguish between amorphous and crystalline solid.
  10. What are Miller indices? Sketch the plane in a cube having Miller indices 110.

 

PART – B

 

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

 

  1. Explain the role of Na+ and K+ ions in biological system.
  2. How does Beryllium differ from other elements of Group 2? Discuss the main points of difference.
  3. How does tetraborane undergo symmetric and unsymmetrical cleavage? Give its structure.
  4. What is Borax? How is it prepared?
  5. How is nitric oxide prepared? How does it react with acidified potassium permanganate?
  6. How is orthophosphoric acid prepared? Write its structure.
  7. Give the preparation and two uses of thionyl chloride.
  8. How is available chlorine in bleaching powder determined?
  9. Explain the structures of ClF3­ and BrF5 using VSEPR theory.
  10. Explain the structures of i. CsCl and ii. zinc blende.

21.Write the salient features of Schottky and Frenkel defects.

  1. Derive the Bragg equation for the diffraction of X-rays by crystals.

 

PART – C

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

 

23.a. How is beryllium extracted from beryl?                                                (6)

  1. Give an account of hydroxides and halides of s block elements          (4)
  2. Write a note on sheet silicates and three dimensional silicates.
  3. a. How is ozone prepared? Establish its structure. (5)
  4. Give the preparation and uses of hydrazoic acid. (5)
  5. Write a note on acidic, basic amphoteric and neutral oxides.
  6. a. What are pseudohalogens? (5)
  7. Compare the reactivity of halogens. (5)

28.a. Describe the three types of cubic unit cells among the Bravais lattices. Calculate the number of atoms per unit cell in each case.                                                                      (6)

  1. Explain the structure of sodium chloride. (4)

 

 

 

 

 

“Loyola College B.Sc. Chemistry Nov 2008 Inorganic Chemistry – I Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

DB 01

 

FIRST SEMESTER – November 2008

CH 1500 – INORGANIC CHEMISTRY – I

 

 

 

Date : 12-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART – A

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

 

  1. How does Ionisation potential vary across a period?
  2. Arrange the following in the increasing order of ionic character: .
  3. Why an anion is always bigger and a cation is always smaller than the parent atom?
  4. Calculate the bond order of N2.
  5. Why H2S is a gas whereas H2O is a liquid at 298k.
  6. What are London forces? Give its origin?
  7. Arrange the following acids according to their increasing acid strength with relevant explanation:
  8. Give an example each for protic and aprotic solvents.
  9. How Caro’s acid can be prepared.
  10. Complete the reactions:

 

 

PART – B

Answer any Eight                                                                           (8 x 5 = 40 marks)

 

  1. What is Lattice energy? How is it determined for the formation of NaCl using Born Haber cycle.
  2. Calculate the electornegativity of Si following allred-rochow procedure. Covalent radius of Si=1.75 Ǎ.
  3. Like compounds dissolve in like solvents – comment.
  4. Discuss the hybridization and structure of SF6 and BeF2.
  5. Give the importance of LCAO method.
  6. What are clathrates? Explain with an example.
  7. What is difference between Valence Band and Conduction band.
  8. What is conjugate acid-base pair? Give two examples.
  9. Complete the reaction

 

 

 

  1. Compare the stability of NH3 and PH3.
  2. How Hydrazine is prepared? Give any three of its reactions.
  3. Write notes on the various allotropic forms of sulphur.

 

 

 

PART – C

Answer any four                                                                             (4 x 10 = 40 marks)

 

  1. (a) Discuss Fajan’s rule with suitable examples.

(b) Calculate the lattice energy of sodium chloride using Born-Haber cycle.

Heat of sublimation of sodium (S) = 108.5kJ/ Mol

Dissociation energy of Cl2(D) = 243.0kJ/ Mol

Ionization energy of sodium (I.E) = 495.2 kJ/Mol

Electron affinity of Chlorine (EA) = -348.3 kJ/ Mol

Enthalpy of formation of NaCl(ΔHf)=-381.8 kJ/Mol

  1. Arrange the following species in the order of increasing order of bond strength and explain:

O2+, O2–, O2 ,O2 2+, O22-

  1. (a). Based on VB theory predict the magnetic property of Oxygen molecule.

(b). Give the preparation, properties and uses of Hydrazine.

  1. How does band theory of metals explain the conduction property of metals.
  2. Explain HSAB theory. Mention any four applications.
  3. Write in detail the properties and structures of various oxides of sulphur.

 

 

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“Loyola College B.Sc. Chemistry Nov 2008 General Microbiology Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

ED 03

 

   B.Sc. DEGREE EXAMINATION – CHEMISTRY & ZOOLOGY

THIRD SEMESTER – November 2008

PB 3200 – GENERAL MICROBIOLOGY

 

 

 

Date : 13-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART A

       Answer all questions                                                                              (20 Marks)                                

       Choose the correct answer                                                                (5×1 =5 Marks)

 

  1. Which of the following is seen in all algae?
  2. Chlorophyll a         b. Chlorophyll c  c.Chlorophyll b                d. fucoxanthin
  3. Cryopreservation involves storage
  4. at low temperature             b.  at optimum temperature
  5. for long periods                  d. at very low temperature using liquid nitrogen
  6. Lac operon in E.coli is an example of ________operon.
  7. inducible                             b. positively regulated
  8. repressible d. negative inducible
  9. Okazaki fragments are used to elongate
  10. the leading strand towards the replication fork
  11. the lagging strand towards the replication fork
  12. the leading strand away from the replication fork
  13. the lagging strand away from the replication fork
  14. Which bacterium is dominant in Trickling filters?
  15. Pseudomonas                         b. Aeromonas
  16. c. E. coli Zoogloea

 

II State whether the following statements are true or False                  (5×1= 5 Marks)

 

  1. The conidiospores are sexual spores.
  2. The generation time of a bacterial population is the time it takes for a bacterial population to double.
  3. Competence is related towards transformation.
  4. Xanthomonas citri is a rod shaped, monotrichous and anaerobic bacterium.
  5. Water can be purified by exposure to UV.

 

 

 

 

 

 

III Complete the following                                                                           (5×1 = 5 Marks)

  1. The cell wall of diatoms are made of ___________.
  2. The bacteria which grow in the presence of minimum quantities of free oxygen are

known as __________.

  1. During replication of DNA, the enzyme known as __________ attaches nucleotides

together to form the new DNA strand.

  1. __________ is a heteroecious fungus with macrocyclic life cycle.
  2. Desulfovibrio is involved in ______________.
  3. Answer all, each in about 50 words   (5x 1 = 5 Marks)
  4. Write short notes on enveloped viruses.
  5. Distinguish between flagella and fimbriae.
  6. Define transcription.
  7. What is dikaryotisation?
  8. What are vaccines?

PART B

Answer any five, each within 350 words only.  Draw diagrams and flowcharts wherever necessary.                                                                                                                 (5x 8= 40 Marks)

  1. List out the salient features of algae.
  2. What is a microbial colony? How can the numbers of bacteria be measured in a bacterial

population?

  1. Explain the different methods of reproduction in bacteria.
  2. Describe the structure and functioning of lac operon in E.coli.
  3. Briefly write about Little leaf of brinjal.
  4. Give a brief account of the Tobacco Mosaic disease.
  5. Write short notes on microbial enzymes.
  6. Discuss briefly about sulfur cycle.

PART C

Answer the following, each within 1500 words only.  Draw diagrams and flowcharts wherever necessary.                                                                                                      (2×20= 40 Marks)

 

29 a. Write detailed notes on the characteristic features and classification of viruses.

                                                      OR

  1. Explain the following:
  2. i) Cheese production ii) Beer production

 

30 a. Describe the ultrastructure of a bacterial cell.

OR

  1. Explain the following:
  2. i) Bacterial conjugation ii) Transduction

 

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“Loyola College B.Sc. Chemistry Nov 2008 Concepts In Inorganic Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

 

DB 03

 

FIRST SEMESTER – November 2008

CH 1503 – CONCEPTS IN INORGANIC CHEMISTRY

 

 

 

Date : 12-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

PART- A

 

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

 

  1. Why orbitals like 1 p and 3 f are not possible?
  2. Define inert pair effect. Give an example.
  3. State Hume Rothery’s ratio rule.
  4. HF is a liquid whereas HCl, HBr and HI are gases at 298k.
  5. Define oxidation and reduction in terms of electronic concept.
  6. Classify the following as Lewis acids or bases.
  7. BF3 ii) NH3 iii) Cl– iv) Zn2+
  8. Of the following species which has the shortest bond length? NO or NO+
  9. Give Born – Lande equation for lattice energy.
  10. Electron affinities of halogens are high. Give reason.
  11. What are bonding and anti bonding orbitals?

 

PART – B

 

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

 

  1. Discuss Mulliken Jaffee concept of electronegativity.
  2. Differentiate between Zone refining and electrolytic refining
  3. What is ( n+l ) rule? Why is 4s orbital is lesser in energy than 3d orbital?                                  (2+3)
  4. Discuss the structure of XeF4 on the basis of VSEPR theory.
  5. Draw the molecular orbital energy diagram for CO molecule.
  6. Nitrogen molecule is diamagnetic while oxygen molecule is paramagnetic. Explain on the basis of Molecular Orbital diagram.
  7. What are clathrates? Give any three applications.                                                                  (2+3)
  8. Explain the nature of conductors, insulators and semi conductors using band theory.
  9. Explain the terms polarization, polarizing power and polarizability.
  10. State giving reasons which cation will have greater polarizing power.
  1. Na+ or Mg2+             ii) Cu2+ or Ca2+                        iii) Pb2+ of Pb4+
  1. What are hard and soft acids and bases? Give examples.
  2. Discuss the crystal structure of CsCl.

PART C

 

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

 

  1. Define the following and explain their trends in a period and in a group.                             (3 + 7)
  1. Electron affinity ii) Ionization energy                ii) Atomic radius
  1. Mention the hybridization and bond angle for the following geometries.
  1. Octahedral ii) Trigonal planar        ii) Trigonal bipyramidal           iv) Tetrahedral
  2. v) Pentagonal bipyramidal
  1. Differentiate the following                                                                                                     (2 x 5)
  1. Inter and Intramolecular hydrogen bonding with a suitable example.
  2. Cubic close packing and hexagonal close packing.
  1.  a) What is lattice energy? Discuss the factors affecting lattice energy.                                   (2 + 4)
  1. b) State and explain Fajan’s rule.                       (4)

 

  1. a) How does inductive effect and resonance effect contribute to the strength of Lewis acids?    (6)
  2. b) Discuss the following reactions in liquid ammonia as solvent.
  3. i) Acid – Base reaction            ii) Precipitation reaction                                                      (4)

 

  1. a)  Explain the hybridization and geometry of SF4.                                                                        (5)

 

  1. b) How are the molecular shapes predicted by Sidgwick – Powell theory?                                 (5)

 

 

 

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“Loyola College B.Sc. Chemistry Nov 2008 Chemistry For Biologists – I Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

DB 04

 

B.Sc. DEGREE EXAMINATION – ADV.ZOOLOGY&PLANT BIO & BIOTECH

THIRD SEMESTER – November 2008

CH 3104/CH 3102 – CHEMISTRY FOR BIOLOGISTS – I

 

 

 

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

Time : 9:00 – 12:00

PART – A

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

  1. Define ionization energy.
  2. What is dipole-induced dipole interaction?
  3. Why do ionic compounds usually have high melting points?
  4. Calculate the pH of a solution whose H+ ion concentration is 0.5 mol/litre.
  5. What is hybridization? Give an example.
  6. Differentiate between order and molecularity.
  7. What is peptisation?
  8. Why is chloroacetic acid stronger than acetic acid?
  9. What is chiral carbon? Give an example.
  10. Arrange the following in the increasing order of basicity:
  1. a) NH­3 b) CH3NH2 c) (CH3)2NH             d) (CH3)3N

PART – B

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

  1. What are the factors influencing the formation of ionic bond?
  2. Discuss the optical isomerism in octahedral complexes with examples?
  3. What are hydrogen bonds? How are they classified? Cite an example for each type.
  4. Write briefly about homogeneous and heterogeneous catalysis with examples.
  5. Derive the dissociation constant for weak acid.
  6. Explain the characteristics of a primary standard substance.
  7. Explain the kinetic and optical properties of colloids.
  8. What is resonance? Discuss the resonance structure of the following:
  1. a) phenol b) nitrobenzene
  1. Discuss the application of colloids.
  2. Explain the structure of BF3 and NH3
  3. What are enantiomers and diasteriomers? Give an example.
  4. a) Define normality.
  1. b) What is the normality of solution containing 5.3g of NaOH in 250 mL.

 

PART – C

Answer any four questions                                                                                    (4 × 10 = 40 marks)

 

  1. Discuss the postulates of Werner’s theory.
  2. Write short notes on a) Electrophoresis b) Electro osmosis
  3. Derive the rate expression for a second order reaction 2A® products.
  4. How are the following polymers manufactured?

(a) Nylon-6,6            (b) Teflon               (c) PVC          (d) Buna-S

  1. Explain any two methods of separation of racemic mixture.
  2. Explain postulates of VSEPR Theory. Predict the geometries of IF7, CH4 and PCl5

using VSEPR theory.

 

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“Loyola College B.Sc. Chemistry Nov 2008 Bioinformatics – I Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

       B.Sc. DEGREE EXAMINATION –MATHS & PHYSICS, CHEMISTRY

ED 04

 

THIRD SEMESTER – November 2008

PB 3204/PB 3202 – BIOINFORMATICS – I

 

 

 

Date : 13-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART A

 

Answer ALLl the questions                                                                                                             (20 marks)

 

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

 

  1. The database for retrieving information on genetic disorders in man is
  2. a) OMIM b) OMIA c) Medline Plus           d) Pubmed
  3. Basic proteins of chromosomes are
  4. a) histones b)histidine c)globin           d)globulin

3.7-Methyl guanosine is added to the nucleotide sequence in

a)5’ end           b) 3’ end          c)intron            d) exon

  1. ORF finder translates the sequence in
  2. a) 6 frames b) 5 frames c) 64 frames    d) 20 frames
  3. A software for identifying restriction site is
  4. a) Neb Cutter b)Rasmol c)Cn3D           d)GRAIL

 

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

 

  1. Rough endoplasmic reticulum is the region of protein synthesis.
  2. RefSeq serves as a standard for genomic analyses.
  3. Entrez is a SRS of NCBI.
  4. Rosalind Franklin provided X-ray crystallographic data of DNA to Watson and Crick for elucidating double helical model.
  5. One letter code of Tryptophan is G.

 

III. Complete the following                                                                                                              (5X1=5)

 

  1. Pubchem substance is a ___________ database.
  2. KEGG is a________ database.

13.__________ is compatible with Rasmol.

  1. Lalign is a ________ alignment tool.
  2. Shannon’s Noise in replication refers to _________.

 

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

 

  1. Mention any two differences between prokaryote and eukaryote.
  2. Differentiate BLAST and FASTA.
  3. What is a Protein Motif.?
  4. What is MapViewer?
  5. Write about Composite Databases.

 

 

 

 

 

PART  B

                                                                                                                       

Answer any five of the following, each not exceeding 350 words.                                                (5X8=40)

 

Draw diagrams and flowcharts wherever necessary.

 

  1. Explain the primary databases in detail.
  2. What is PDB and what are its features?
  3. Discuss about Human Genome Project and the genesis of bioinformatics tools.
  4. Write about enzyme databases and its features.
  5. How is the GenBank flatfile organized and write about header and features table?
  6. Briefly discuss about DNA replication.
  7. Write about proteomic tools including Compute pI/MW and Signal P.
  8. How is the protein secondary structure organized into Alpha helix and Beta strands?

 

PART C

 

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

Draw diagrams and flowcharts wherever necessary.

 

  1. a) Elaborate upon BLAST, its parameters, types and applications

 

(OR)

 

  1. b) Align the following sequences using Needleman Wunsch algorithm

Seq 1: ACTCG

Seq 2: ACAGTAG

 

  1. a) Discuss about protein signature prediction by defining Motif, Domain, Family and Signature .List the

databases from which the details can be retrieved.

 

(OR)

 

  1. b) Explain the structure visualization tools including Homology Modeling.

 

 

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“Loyola College B.Sc. Chemistry Nov 2008 Bio Chemistry Question Paper PDF Download”

by

LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

DB 16

 

FIFTH SEMESTER – November 2008

CH 5404/CH 5401 – BIO CHEMISTRY

 

 

 

Date : 14-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART A

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

 

  1. What are the functions of cytoplasm of the cell?
  2. How is the presence of aldehyde group confirmed in glucose?
  3. What are essential fatty acids? Give an example.
  4. Define iodine number of an oil.
  5. Write down the differences between amylose and glycogen.
  6. What is glycosidic bond? Give an example.
  7. What is respiration? What are the two phases of respiration?
  8. Define oxidative phosphorylation.
  9. Draw the structure of adenylic acid.
  10. What are coenzymes?

PART B

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

 

  1. Write down the differences between Prokaryotic and Eukaryotic cells.
  2. Discuss the β-Oxidation theory of fatty acids.
  3. What are phospholipids? Explain the types of phospholipids.
  4. Mention any five differences between animal and plant fats.
  5. Discuss any five characteristic features of biological oxidation.
  6. Explain the classification of carbohydrates with examples.
  7. Discuss briefly the phase II of the glycolysis process.
  8. Discuss the mechanism of electron transport system.
  9. Explain the replication of DNA.
  10. Draw and explain the double helical structure of DNA.
  11. Explain the steps involved in the translation process of protein synthesis.
  12. How is the cyclic structure of glucose elucidated?

 

PART C

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

 

  1. Discuss any two methods to determine the N-terminal of an amino acid.
  2. Explain the types of reversible enzyme inhibition.
  3. Explain the series of reactions involved in TCA cycle with the enzymes involved and energy yield.
  4. Discuss the biosynthesis of cholesterol.
  5. a) Draw and explain the structure of t-RNA.
  6. b) Explain the importance of primary structure of proteins.                                                                   (5+5)
  7. a) Explain the chemistry of hemoglobin in blood.
  8.  b) What is genetic code? Mention any five important characteristics of genetic                           (5+5)

 

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“Loyola College B.Sc. Chemistry Nov 2008 Adv. General Chemistry For Phys.& Maths Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

DB 05

 

   B.Sc. DEGREE EXAMINATION – MATHS & PHYSICS

THIRD SEMESTER – November 2008

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

 

 

 

Date : 13-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART-A

Answer all the questions                                                                           (10×2= 20)

 

  1. Mention any two methods involved in the detection of hydrogen bonding?
  2. H2O has a higher boiling point than H2S. Justify.
  1. Define lattice energy.
  2. Give a method of preparation of pyrrole.
  3. Define Internal energy.
  4. What is solubility product?
  5. How is energy transformed in photosynthesis reaction?
  6. What are transferases? Give an example.
  7. Differentiate renewable sources from non renewable sources of energy.
  8. Mention two advantages of mixed fertilizers.

PART-B

Answer any eight questions                                                                      (8×5= 40)

  1. Discuss lanthanide contraction giving causes and its consequences.
  2. How are the following prepared? Give equations. a) Congo red b) Malachite green.
  3. Give a synthetic method of preparation and uses of asprin.
  4. Write any one method of preparation of furan and explain the nitration of furan with example.
  5. Discuss the classification of dyes based on their structure.
  6. How is (a) pyridine converted to 2- nitro pyridine and (b) pyrrole to pyrrole-2-aldehyde
  7. What are broad spectrum antibiotics? Give two examples with uses.
  8. What are carbohydrates? How are they classified?
  9. Describe Sanger’s method for the sequential determination of amino acid.
  10. What are enzymes? Give any four properties of enzymes.
  11. Write short notes on thermal cracking and catalytic cracking of liquid fuels.
  12. Mention any four functions each for macro and micro nutrients in plants growth.

PART-C

Answer any four questions                                                                      (4×10= 40)

  1. i) Define hydrogen bonding. Explain the two types of hydrogen bonding with example. (7)
  2. ii) Why do ice float on water? (3)
  3. i)Explain the working principle of secondary reference electrode.(5)
  4. ii) How is naphthalene prepared by Haworth synthesis? (5)
  5. i) What are the factors affecting lattice energy? (5)
  6. ii) Derive the variation of enthalpy of reaction with temperature.(5)
  7. i) Draw and explain the working principle of calomel electrode. (6)
  8. ii) Explain Hess’s law. (4)
  9. i) Establish the open chain formula of fructose. (7)
  10. ii) Discuss the secondary structure of protein in detail. (3)
  11. Explain any two of the following. (5+5)
  12. a) Nuclear fusion b)  Herbicides   c) Phosphatic fertilizers  d) Fungicides

 

 

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“Loyola College B.Sc. Chemistry Nov 2008 Analytical Chemistry Question Paper PDF Download”

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

DB 18

 

FIFTH SEMESTER – November 2008

CH 5501 – ANALYTICAL CHEMISTRY

 

 

 

Date : 05-11-08                     Dept. No.                                        Max. : 100 Marks

Time : 9:00 – 12:00

PART – A

 

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

 

  1. What will you do as first when phenol spilts on the hands.
  2. How many significant figures are there in a) 0.10000 b) 6.023X1023.
  3. When is distillation under pressure carried out?  Give an example.
  4. Write down two applications of Rf values.
  5. Distinguish between formality and normality.
  6. Can we use methyl orange indicator in the titration of NaOH against HCl?  Justify.
  7. What are adsorption indicators?  Write an experiment where it is used.
  8. Calculate the energy of an electromagnetic radiation of wave length 663 pm.
  9. Sketch the vibrational modes of H2O and label each as IR active or inactive.
  10. Enlist the factors affecting solubility.

 

PART – B

 

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

 

  1. Draw the block diagram of single pan balance and label the components.
  2. Give the differences between precision and accuracy.
  3. Write a note on Soxhelet extraction.
  4. What are the types of resins used in ion exchange chromatography.  Give examples and applications.
  5. Calculate the pH of a buffer solution containing 0.1 M of acetic acid and 0.01 M of sodium acetate.  (Ka of acetic acid = 1.8X10-5 at 25oC).
  6. Write a note on theories of indicators.
  7. Distinguish between co-precipitation and post-precipitation.
  8. Discuss the principle of titration using EDTA.
  9. How would you prepare 100 mL of N HCl from i) concentrated HCl (11N)
  1. ii) a solution of 2 N HCl
  1. What are chromophores and auxochromes?  Cite examples.
  2. Write Beer Lambert’s law.  What are its limitations?
  3. How will you distinguish different types of hydrogen bonding by IR spectroscopy?

 

 

 

 

PART – C

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

 

  1. a) Name the various types of errors in chemical analysis.                                                       (4)
  1. b) Find out the (i) mean (ii) median and (iii) mean deviation for the following data: 0.1010,

0.1020, 0.1005, 0.1030, 0.1015.                                                                                         (6)

 

 

  1. a) Write about (i) Bathochromic shift; (ii) hypsochromicshift; (iii) hyperchromic shift
  2. b) What are the types of electronic transitions?                                                                       (6+4)

 

  1. a) List out the requirements of a primary standard?
  2. b) Describe Volhard’s method of chloride estimation. (5+5)

 

  1. a) What are the tests of purity?
  2. b) Compare thin layer chromatography with column chromatography. (5+5)

 

  1. Discuss different types of titrations with an example for each type.

 

  1. Distinguish between             a) end point and equivalence point            b) stationary phase and mobile phase
  2. c) Symmetric stretching and asymmetric stretching                         (3+3+4)

 

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“Loyola College B.Sc. Chemistry April 2009 Transition Elements And Nuclear Chemistry Question Paper PDF Download”

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    LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 25

FIFTH SEMESTER – April 2009

CH 5506 – TRANSITION ELEMENTS AND NUCLEAR 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) 

  1. Most of the transition metals form coloured compounds. Explain.
  2. Explain the terms Calcination and Roasting giving suitable examples.
  3. What is meant by Half-life period of a radio active element?
  4. Name the important mineral and its composition of lanthanides which occur in India.
  5. Fill in the blanks.
  1. 7N14 + 2He4 → ……. + 1H1
  2. 4Be9 + …… → 6C12 + 0 n1 +  5 MeV.
  1. Complete the following.
  1. 92U238 + 7N14 →  …….+ 4 ( 0 n 1 )
  2. ……. + 8O16 → 100Fm250 + 4 ( 0 n 1)
  1. Explain the co-ordination position isomerism with suitable example.
  2. What is Spectrochemical series? Why is it so called?
  3. Write down the general electronic configuration of actinides?
  4. Define Binding energy of nucleus.

PART-B

 Answer any eight questions                                                                    ( 8 X 5 = 40)

  1. Explain the extraction of Titanium from its chief ore.
  2. Give an account of the various types of furnaces used in the extraction of metals.
  3. What is Lanthanide contraction? What are the consequences of lanthanide contraction?
  4. Give an account of magnetic and spectral properties of actinides.
  5. Sketch all possible isomers of [Co( NH3)2(H2O)2Cl2]+.
  6. Discuss the application of Valence Bond theory to [Fe(CN)6]8- complex.
  7. Discuss the cis-trans isomerism in 4 co-ordinate square planar complexes.
  8. How will the n / p ratio influence the stability of the given nucleus?
  9. Describe the application of neutron activation analysis in trace metal analysis with suitable example.
  10. Describe the principle, working and uses of G.M. Counter.
  11. Explain the salient feature of Shell model.
  12. Discuss the Atomic Power Projects in India.

 

PART-C

 Answer any four questions                                                                (4 X 10 = 40)

  1. Discuss the preparation and applications of any four compounds of transition

elements, which act as industrial catalyst.

24.a) What are inner transition elements? Comment on their position in the periodic table.

  1. b) Describe how lanthanides were successfully separated by ion-exchange
  2. a)What is a Chelate? What are the factors which affect the stability of chelates.
  3. b) How are chelate formation useful in i) Volumetric analysis and ii) Gravimetric analysis.
  1. a)Discuss the splitting of “d” orbitals of metal in square planar complexes with diagram.

b)What are the merits and demerits of Crystal Field Theory?

  1. Write short notes on a) Atomic bomb b) Hydrogen bomb
  2. Describe the Principle, construction, working and applications of a nuclear reactor.

 

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

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        LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

B.Sc. DEGREE EXAMINATION – CHEMISTRY

WD 12

THIRD SEMESTER – April 2009

CH 3504 – THERMODYNAMICS

 

 

 

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

 

 

 

PART – A

Answer ALL questions:                                                                                  10 x 2 = 20     

 

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

 

PART – B

Answer any EIGHT questions:                                                                      8 x 5 = 40

 

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

 

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

 

PART – C

Answer any FOUR questions:                                                                       4 x 10 = 40

 

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

 

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“Loyola College B.Sc. Chemistry April 2009 Synthetics Organic Chemistry And Spectroscopy Question Paper PDF Download”

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    LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

WD 22

B.Sc. DEGREE EXAMINATION – CHEMISTRY

SIXTH SEMESTER – April 2009

       CH 6609 / 6603- SYNTHETICS ORGANIC CHEMISTRY AND SPECTROSCOPY

 

 

 

Date & Time: 25/04/2009 / 9:00 – 12:00     Dept. No.                                                       Max. : 100 Marks

 

 

PART – A

Answer ALL questions:                                                                               (10 x 2 = 20)

  1. What is retrosynthetic analysis in Organic chemistry.
  2. What is disconnection approach.
  3. Write the mechanism of C-alkylation of acetoacetic ester.
  4. Write the product of aldol condensation of Acetaldehyde.
  5. Predict the product of Diel’s – Alder reaction.

(i)                                                                            (ii)

 

 

  1. Write the structure of the product

(i)                                                            (ii)

 

 

  1. Calculate the max value for the following compounds using Woodward Fieser rule?

(i)                                                            (ii)

 

 

  1. Concentrated solution of ethanol and 1, 2- glycol in CCl4 exhibit broad O-H stretch near 3350 cm-1 in their IR spectra. On dilution with CCl4 the spectrum of 1, 2 – glycol does not change but that of ethanol exhibits a sharp band at 3600 cm-1 in addition to the broad band at 3350 cm-1. Explain the observation.
  2. C13 is NMR active while C12 is not explain.
  3. How will you account for the appearance of prominent peaks at m/z 31, 42 and 70 in the mass spectrum of n- pentanol.

PART – B

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

  1. Explain Umpolung synthesis.
  2. What is the difference between conversion and synthesis.
  3. Predict the product of Birch reduction of
  • Benzoic acid (ii) Anisole.
  1. Explain the product and mechanism of hydroboration of propene.
  2. Write the mechanism and stereochemistry of Diel’s Alder reaction of

 

  1. Discuss the method of protecting aldehyde and keto group?
  2. Explain the importance of molecular in peak in mass spectra.
  3. Write note on i) bathochromic shift      ii) coupling constants
  4. How many different set of equivalent protons do each of the following compounds have? How many signals would each compound give in its lH NMR spectram
  5. CH3-CH3 ii) CH3-O-CH3      iii) CH3-CH2–      -CH2-CH3                                iv) CH3 –     -O CH3
  6. Give a brief account on Refrence standards used in ‘H NMR spectral technique.
  7. The IR spectrum of methyl salicylate shows the following peaks at 3300 cm-1 1700 cm-1 3050 cm-1, 1540 cm-1, 1590 cm-1 and 2950 cm-1. Attribute these peaks to the following features of the molecule.
  8. What is meant by shielding and Deshielding of protons in NMR spectoscopy.

PART – C

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

  1. What are the application of Electrophilic Synthon and Synthetic equivalent in Retro Synthetic analysis.
  2. i) How does IR spectroscopy useful to distinguish between  a) O-nitro phenol and p-

nitrophenol.

  1. A compound having the molecular formula C10H14 exhibits following HlNMR signals. d28(5H singlet) 0.880 (9 H S). Assign the structural formula of the compound.
  2. i) How are the following groups protected and de protected during the synthesis of organic compound.
  3. –NH2 b) –OH group
  4. An organic compound A (molecular formula C9H10O2) exhibits the following spectral data

IR: 1745 cm-1,             1225 cm-1             749 cm-1               697 cm-1

UV: lmax 268, 264

|HNMR=d1.96(3H, S)              5.00(2H, S)          7.22(5H, S)

  1. i) How will you synthesis i) Acetylacetone               ii) Crotonic acid from ethylacetoacetate.
  • “Diels-Alder reaction is highly stereo specific”. Explain.
  1. Using Umpolung reaction how will you synthesis
  2. C6H5-CH2– -CH3               ii)
  3. Explain any two of the following (5+5)
  4. Clemmenson reduction and its mechanism
  5. Working principle of UV=Visible spectrophotometer with a block diagram.
  6. Oxidation by peracids.

 

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