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School Living Certificate Examination (Grade 10)
Group B Chemistry only
Attempt 3 questions from this group. Q No. 6 is compulsory
6.
(a). What is meant by a solution ? In most solutions the solute is a solid and the solvent is liquid. This is not always true. Give four different examples of solutions where this is not true. (No description is required.) 1+(1/2)x4=3 (b). Give the meaning of solubility curve. The solubility of common salt at 30oC is 200. What amount of water is required to prepare a saturated solution for 1 Kg of the salt ? 1+2=3 (c). What are the causes of temporary hardness in water ? Write one method with chemical reactions to remove such hardness 1+1+1=37. Ammonia gas can be prepared in the laboratory by heating two solid substances together :
i. Name two solid substances with formula which could be used in it. 1+1=2 ii. Write a balanced equation for this chemical reaction. 1+1=2 iii. Draw a neat and well labelled diagram of the apparatus for the preparation of ammonia gas in the laboratory 1+1=2 iv. Mention two uses of this gas. 1+1+28.
(a). Explain the special properties of highly reactive non-metal on the basis of electronic configuration of atoms and write one example of such highly reactive non-metal. 3+1=4 (b). What do you mean by molecular formula ? What is its importance ? Write the molecular formulae of sodium bicarbonate and sodium sulphate. 1+1+1+1=49.
Explain the meaning of the term - Indicator. Give full forms (words) of P.V.C., D.D.T., and B.H.C. And write one use of each of them (No description). 2+(1+1)x3=8
(First Year)
Time : 3 hrs.
Full Marks : 100
Candidates are required to give their answers in their own words as far as practicable
The figures in the margin indicate full marks.
Attempt EIGHT questions, selecting at least ONE each from Group A and B and TWO from Group C.
Group A
1. Illustrate with example any four different types of chemical reactions. (6) The solubility of a salt is 25 at 25oC. What amount of salt will be present in 75 g of its saturated solution at that temperature ? (4) 2. State Charles' law and show how it leads to the relationship. V T when P is constant (4) If 40 l of nitrogen are collected at 22oC over water at a pressure of 0.957 atm, what is the volume of dry nitrogen at STP, given aqueous tension at 22oC = 19.76 mm ? (6) 3. Write a short note on Bronsted - Lowry's definition of acid-base behaviour and show how it differs from the Arrhenius difinition (5+2(1/2)) Write electron dot formula of ammonia and show hot it can function as a lewis base. (2(1/2))4. How is copper extracted from copper pyrites and refined ? Write a short note on its action with HNO3. Use only balanced equations for reactions involved. (5+2(1/2)+2(1/2)) 5. What are the alkali metals ? Write a short not on their characteristics. (5) Write down the principles involved in the extraction of sodium metal from sodium chloride (Downs' process). Also give a labelled diagram for the same. (5) 6. Describe and explain what happens when (a) silver nitrate is strongly heated (b) water is lowly added to a piece of quicklime (c) gypsum is heated (d) ammonia solution is added to the solution of blue vitriol drop by drop to excess (e) ammonia gas is reacted with heated CuO. Give only balanced equations for reactions shown. (2x5)Group C
7. Describe giving balanced chemical equations how and under what conditions water reacts with iron, zinc, calcium and carbon. (1(1/2)x4) What is nascent hydrogen ? Show by using KMnO4 solution why it is a more powerful reducing agent than ordinary hydrogen. Give balanced chemical equations. (1(1/2)+1(1/2)) What is hydrogenation ? 8. Under what conditions do hydrogen and nitrogen combine to form ammonia ? (2+5) Explain giving balanced equations how ammonia is oxidised into nitric acid. (3) Show how nitric acid reacts with I2. 9. Describe giving a neat, self-explanatory sketch how sulphuric acid is manufactured by the contact process. Give one balanced chemical equation to show that sulphuric acid is (a) an oxidising agent and (b) a dehydrating agent. (3+5+2x1) 10. What do you mean when you say that graphite and diamond are really one and the same element ? Compare their properties. What is activated charcoal ? (2+3+1) Under what conditions and with what effect does CO react with (a) nickel (b) NaOH ? (2+2) 11. Write balanced chemical equations for reactions that occur when (a) conc. HC1 and K2Cr2O7 (b) SO2 and H2S. (c) KI and conc. H2SO4 (d) Br2 and KOH (e) P4 and NaOH (f) H2O2 and acidified KMnO4, react with each other under appropriate conditions. (Do any five only). (2x5) 12. Describe a technical method for the production of Iodine. (6) Explain why HBR and HI can not be prepared by the method used for the laboratory preparation of HCl. (4)
(Second year)
Time : 3 hrs.
Full Marks : 80
Candidates are required to give their answers in their own words as far as practicable.
The figures in the margin indicate full marks.
Attempt EIGHT questions, slecting at least ONE from Group A and Group B and TWO from Group C.
Group A.
1. State Avagardro's hypothesis and show how it leads to the relationship, molecular weight=twice the vapour density. (1+4) 2g. of a substance on vapourisation gave 3 litres of vapour at 27oC and 780 mm pressure. What is the molecular weight of the substance ? (5) 2. Explain clearly what you understand when it is said that a solution of sodium carbonate is decinormal and also state giving reason whether the solution can be used as a standard solution. (4) 18 ml of N/2 NCl solution, 10.3 ml of 2N HCl solution and 16.4 ml of N/10 HCl solution are mixed together. Calculate the strength of the mixture in terms of normality and grams per litre. (6) 3. State and explain any two of the following : (5X5)a. Faraday's second law of electrolysis b. Le-Chatelier's principle c. Dulong and Petit's law4. How is mercury extracted from its chief ore and purified ? Describe giving balanced chemical equations the reactions between corrosive sublimate and (a) potassium iodide (b) stannous chloride. (6+2+2) 5. What is steel ? How is it manufactured by the Open Hearth process ? What are the advantages of this process over the Bessemer process ? (1+6+3) 6. Describe and explain giving balanced chemical equations what happens when (a) zinc oxide is reacted separately with dilute sulphuric acid and caustic potash, (b) caustic soda solution is added drop by drop to excess to a solution of white vitriol, (c) hydrogen sulphide is passed separately through a neutral and an acidic solution of white vitriol, (d) zinc is reacted with dilute nitric acid, and (e) zinc is heated with concentrated suphuric acid. (2x5)Group C
7. Explain giving examples what is meant by the term, 'homologous series'. Write down the structures, common names and IUPAC names of the isomers of pentane. (4+6) 8. Give with a neat diagram the mothod of preparing ethene in the laboratory. Under what conditions and with what effects does it react with (a) halogens, (b) sulphuric acid, (c) ozone, and (d) hydrogen. (6x4) 9. What are alcohols ? How are they classified ? How are they distinguished from one another ? (2+3+5) 10. Describe how aniline is prepared in the lab. Starting with aniline how will you prepare (a) acetanilide, (b) benzene diazonium chloride, (c) phenyl isocyanide, (d) p-sulphanilic acid, and (e) phenol. (5+5) 11. How may (a) methyl alcohol be converted to ethyl alcohol, (b) acetaldehyde to formaldehyde, (c) formic acid to acetic acid, (d) benzene to aniline, and (e) phenol to aniline ? (5x2) 12. Describe with a neat sketch how a sample of pure diethyl ether is prepared in the lab. What happens when ether is reacted with (a) H2 SO4, (b) HI (c) PCI5 (d) air ? (6+4)
Chemistry I Paper
Full Marks : 100
Time : 3 hrs.
Candidates are required to give their answers in their own words as far as practicable.
The figures in the margin indicate full marks.
Attempt any TWO questions from Group A and andy FOUR from Group B.
Group A
1. Discuss the deviation of real gases from ideal gas behaviour. How are they accounted for in Van der Waal's equation ? Calculate the temperature at which 2 moles of nitrogen will occupy a volume of 10 litres at a pressure of 15 atm. (Vander Waal's constants for N2: a = 1.39 lit. atm. mol-1; b=0.039 lit-atm. mol-1. Also R = 0.082 lit. atm/deg./mol.) (6+4+6) 2. State and derive Raoult's law for lowering of vapour pressure. Explain its limitations. (7+3+6) Dissolution of 18.2 of urea in 100 g of water at 50oC produced a lowering of vapour pressure by 5 mm Hg. Calculate the molecular weight of urea if the vapour pressure of pure water at 50oC is 92 mm Hg. 3. Write notes on any two of the following : (8+8)a. Kohlrausch's law b. Order & molecularity of a reaction c. Pauti exclusion principle d. Le-chatlier's principle4. What do you mean by hybridisation ? Explain any four types of hybridisation with suitable examples. (4+3x4) 5. Write a short note on any tow of the following (8+8)a. Electronegativity b. Variation of Ionization potential in the periodic table c. Nitrogen fixation6. (a) Discuss the position of manganese in periodic table (8) (b) Write the preparation and properties of potassium dichromate. (8) 7. Write the chemistry of the following compounds : (any two) (8+8)(a) Diborane (b) Marshall's acid (c) Hydrogen peroxide (d) Hydroxyl amine8. What are complex compound ? Discuss the Werner's theory for co-ordination compound. Use any theory of your choice to account for the nature of bonding in complex compound. (2+6+8) 9. Describe the extraction of aluminium. Mention some of the alloys of aluminium and give their uses. (10+3+3)
Bachelor Level / II Year/ Science
Chemistry II Paper
Full Marks : 100
Time : 3 hrs.
Candidates are required to give their answers in their own words as far as practicable.
The figures in the margin indicate full marks. 4 marks for general impression.
Attempt SIX questions, any TWO from Group A and any FOUR from Group B.
1. Deduce Kirchoff's equation and explain its significance. When 1 mole of liquid benzene is completely burnt in oxygen to form liquid water and carbon dioxide gas, the heat evolved is 781 kcal at 25oC and constant pressure, Calculate the beat of the reaction at constant volume at the same temperature. 8+8 2. What do you understand by single electrode potential ? Explain the use of the calomel electrode for determination of single electrode potential. Comment on the function of the salt bridge used. 6+8+2 3. What are colloids ? Distinguish between lyophobic and lyophilic colloids. Describe Bredig's method of preparing lyophobic colloids and the use of ultrafiltration in its purification. 3+5+5+3 4. Write short notes on any two (a) Adsorption theory of hetereogeneous catalysis. (b) Theory of strong electrolytes, (c) Beer-Lambert's law and (d) Criteria of catalysis. 8x25. Discuss the stability of the cycloalkanes. 16 6. Explain how mechanisms of organic reactions may be determined. 16 7. What are elimination reactions and how do they proceed ? Give examples to illustrate your answer. 6+10 8. What is hybridisation ? Discuss hybridisation of carbon atom in methane, ethylene and acetylene. 4+4x3 9. What are (a) enantiomers (b) diastereoisomers ? Write a note on specifying absolute configuration on an assymetric system by R, S system 4+4+8 10. Explain why pyridine shows basic character. Discuss electrophilic and nucleophilic substitution in pyridine. Explain its structure. 4+4+4+4 11. How is stability of benzene accounted for by the resonance theory ? Give the mechanism of (a) Nitration (b) Friedel-Crafts alkylation of benzene. 12. Convert an aldohexose into an depentose and vice versa. Discuss the effect of halogen on electrophilic aromatic substitution. 5x2+6
Science (Organic Chemistry)
Full Marks : 100
Time : 4 hours
Candidates are required to give their answers in their own words as far as practicable. The questions are of equal value.
Attempt any SIX questions, selecting at least ONE from each group.
Group A
1. Define aromatic, homoaromatic, non-aromatic and anti-aromatic compounds with examples. Also explain which of the following are aromatic or non-aromatic or anti-aromatic.(a) Cyclobutadiene (b) Cyclopropenyl anion (c) Tropolones (d) Fulvenes (e) Sydnone (f) Ferrocene.2. Answer any four of the following :(a) Explain why the carbon-chlorine bond distance decreases in the series: Ethylchloride, vinylchloride and chloroacetylene. (b) Explain the face that it is impossible to remove a proton (H+) from ethane while a very strong base will remove a proton from acetylene according to the equation,._ HC = CH + B --> HC = C+BH.(c) Explain why is it easier to generate a carbonium ion bonded to benzene ring than it is to make methyl carbonium ion. (d) Ethoxide ion is a much stronger base than acetate ion. Explain (e) The more substituted a free radical, the more stable it is and faster it is formed. Explain.3. Write short notes on any three of the following :(a) Homoconjugation (b) Benzyne and nitrene intermediates (c) C13-NMR (d) Kinetic method of determining reaction mechanism.OR Discuss the 1H-NMR spectrum of ethylacetate. 4. Discuss fully and establish the structure of Oxytoxin. Also describe a method of polypeptide synthesis. 5. What are Ureids and Purines ? Starting from uric acid show how can you obtain purin, adenine, guanine, xanthene, hypoxanthene, caffeine, theophylline and theobromine. OR An organic compound A(C5H4O3N4) gives four different monomethyl derivaties. On HNO3 oxidation compound A gives in equimolecular proportions urea (NH2 CO NH2) and a compound B (C4H2O4N2) having no free anion or carboxyl groups. B on KOH hydrolysis gives one molecule of urea and one molecule of meso oxalic acid (HOOC-CO-COOH). On oxidation with PbO2 or KMnO4 A gives carbon dioxide and a compound C (C4H6O3N4) which on KOH hydrolysis gives one molecule of flyoxalic acid (HCO-COOH) and two molecules of urea. Compound C on HNO4 oxidation gives in equimolecular proportions urea and a compound D (C3H2O3N2) which on hydrolysis gives again urea and oxalic acid. What are A,B,C and D. Give a synthesis of A. 6. Write short notes on the following (any three):(a) DNA (b) Coenzyme (c) Photosynthesis (d) Carbohydrate conformation.7. Answer the following :(a) Draw potential energy diagram for different conformers of ethane and explain their stability. (b) Explain with example the differences between enantiomers and diastereomers.8. Write notes on any four of the following :(a) Asymmetry (b) Dissymmetry (c) Dihedral angle (d) Reflection symmetry (e) Epimers.9. Answer the following :(a) What is a photosensitizer ? Explain the mechanism of the photochemical reaction. hµ OH OH 2(C6H5)2CO+2RH -----> (C6H5)2 --C---C--(C6H5)2+R--R. An important side product is (C6H5)2 C(OH)R. (b) Describe HMO (Huckel Molecular Orbital) Calculation for butadiene.10. Suggest mechanism for the following reactions (any three):(a) Drazen's glycidic ester condensation (b) Mannich reaction. (c) Wolf-Kishner reduction (d) Wagner-Meerwein rearrangement.11. Describe the synthetic uses of any four of the following reagents giving mechanism of the reaction which involves the following reagent.(a) (CH3)3COK (b) NBS (c) Pb(OAc)4 (d) C6H5-CO3H (e) NaBH4.12. Suggest mechanism for the following (any three)
Chemistry I Paper (Physical Chemistry)
Full Marks : 100
Time : 4 hours.
Candidates are required to give their answers in their own words as far as practicable.
The questions are of equal value.
Attempt any SIX questions selecting at least ONE question from each group.
Group A
1. What are the main assumptions of Debye-Huckel theory of strong electrolyte ? Explain how this theory accounts for the variation of equivalent conductance with dilution of strong electrolytes. Calculate the ionic strength of 0.3 M aluminium sulphate. 2. What are concentration cells ? Derive an expression for the emf of an electrolyte concentration cell with transference. Calculate the emf of the following cell,Ag/AgNO3(0.1M)/AgNO3(0.001M)/AgActivity coefficient of 0.1 M and 0.001 M AgNO3 are 0.62 and 0.99 respectively and transference number of cation is 0.465.Group B
3. What is Gibb's free energy function ? Discuss criterion of spontaneity for a physicochemical change using this function. Calculate Æ G and equilibrium constant for the following reaction at 25oC.C(graphite) + 2H2(g) ' CH4(g)having given, C(graphite) 2H2(g) CH4(g) ____________________________ Æ Hfo KJ mol-1 9.0 0.0 -74.83 So J K-1 mol-1 5.68 130.6 188.2 4. Write brief account on any two.(a) Entropy change for expansion of an ideal gas. (b) Third law of thermodynamics. (c) Pressure and temperature dependence of free energy.5. Explain parallel reaction with suitable examples. The reactions,k1 (a) A ------> D+E fast E+B ------> C and k2 (b) A+B ------> C+Doccur side by side (parallel reactions). k1 is a first order rate constant and k2 a second order rate constant. Derive a rate equation for these parallel reactions. Suggest a method for the evaluation of the individual values of k1 and k2. 6. Discuss the effects of temperature on the rates of chemical reactions. Derive Arrehenius equation relating rate constants with temperature. In the following gaseous decomposition,CH3COOCH3 (g) --> C2H4(g) + H2(g) + CO2(g)the initial pressure was 0.42 atmosphere. The pressure was increased to 0.54 atmosphere after 6.5 mins. Fine the rate constant of this decomposition if the reaction follows first order kinetics. What will be the pressure after 10 mins ? 7. Write notes on (any two)(a) Laws of Photochemistry (b) Photochemical reaction between hydrogen and chlorine. (c) Effects of light absorbed by molecules.Group D
8. What are Miller indices ? Draw neat diagrams to indicate Miller indices of the important plane systems in simple cubic crystal. Obtain a relation between interplanar spacing and cube edge. 9. What is a surface active agent ? Discuss the quantitative aspects of the equation which is used to measure the excess of the solute concentration at the surface of the solution. 10. Write notes on (any two)(a) Phase rule equation. (b) Symmetry operations. (c) Origin of charge on colloidal particles.
Chemistry II Paper (Inorganic Chemistry)
Full Marks : 100
Time : 4 hours.
Candidates are required to give their answers in their own words as far as practicable.
The questions are of equal value.
Attempt any SIX questions.
1. Derive the wave function and energy for the particle in a one dimensional box. 2. (a) What are three important types of hybrid orbitals that can be formed by an atom with onlys and p orbitals in the valence shell ? Describe the molecular geometry which each of these produces. (b) Using both the MO approach and the resonance energy explain why the NO bond in NO3- have a bond order of 1x. 3. Write short notes on any two : (a) Nuclear fission (b) Radioactive distintegration series (c) Binding energy 4. Attempt any two of the following : (a) The complex [NiCN)]4-2 is diamagnetic but [NiCl4]-2 is paramagnetic. Explain it by using simple Crystal Foeld Theory. (b) Diamagnetic complexes of cobalt (III) such as [Co(NH3)6]+3 [Co(en)3]+3 are orange yellow. In contrast the paramagnetic complexes [CoF6]-3 and [Co(H2O)3F3] are blue. Explain qualitatively this difference in colour. (c) Show that John Tellor distortion is expected for d9 configuration (octahedral environment) 5. Write notes on any two of the following :(a) Linkage isomerism (b) Orgel diagram (c) Nephelauxetic series (d) Term Symbols.6. What are mixed metal oxides ? How are the mixed metal oxides of Ti and Zr have variable oxidation states ? Give their known oxidation states and stereo chemistry. OR Give a group discussion of Gr VI A (Mo. W) 7. Discuss the electronic configuration and oxidation states of Lanthanides. Why is that it is difficult to separate the Lanthanides. Discuss at least one method which can be used for the separation of Lanthanides. 8. Write a note on any one(a) The use of Organic reagents in Inorganic analysis (b) Use of liquid SO2 as a non-aqueous solvent.9. Attempt any two(a) What are two-electron three centred bonds ? Illustrate with an example. (b) The 1st ionization potential of B.AI, Ga, In and TI is 8.30, 5.98, 6.00, 5.79 and 6.11 ev. How do you account for this non unformity ? (c) The melting point of o-nitrophenol. m-nitorphenol and p-nitrophenol are as follow 45o, 96o, 114o C. How do you account for it ?10. Write a notes on (a) Crystal structure of TiO2 (b) Bonding in Xenon complexes
Proficient Certificate Examination :
1. Experiment involving bending, rounding off glass tubes and fitting up of a wash bottle.
2. Experiment involving solution, distillation, sublimation, precipitation, , crystallization and separation of mixture.
3. Fitting up of apparatus for the preparation of H2, CO2, NH3, HCl, H2S and SO2 and study of their properties.
4. Study of different types of chemical reactions and preparation of salts by neutralizing acids and bases.
5. Study of the reactions by wet and dry methods of CO3--,, SO3--,, NO2-, NO3-, Cl-, Br-, I-, and SO4--,
6. Dry tests for Basis redicals (NH4+, Na+, K+, Cu2+, Zn2+, Pb2+, Ni2+ Co2+, Mn2+, Ca2+, Ba2+, Al3+, Fe3+, Fe2+, Mg2+
7. Wet tests for basic redicals of simple salts.
8. Complete analysis of simple salts.
1. Recovery and preparation of simple salts from mixtures.
2. Determination of eq.wt. of Zn., Mg. Al, by H2 displacement method and of Cu by Oxide method.
3. Letermination of % of water os crystallization.
4. Expts. involving preparation of standard solution and determination of strength of approximately decinormal solutions of acids and bases.
5. Determination of the strength of fairly concentracted solution of acids, uses and determination of eq. wts. of metals and %
6. Standardization of KMnO4 solution against Oxalic acid solution.
7. Detection of elements of organic compounds (N.S, halogens).
8. Identification of formate, oxalate, acetate, glycerine, acetone, alcohol in solution.
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