final dtp1
TRANSCRIPT
R. BALAJI M.Sc., M.Phil., B.Ed.
Ph. 9962001120
P.G. Asst in Chemistry.
SUCCESS TUTION CENTRE
INORGANIC CHEMISTRY
1. ATOMIC STRUCTURE
1. State Heinsberg’s uncertainity principle.
2. What is the significance of negative electronic energy?
3. Why He2 is not formed?
4. What is bond order?
5. What are the difference between particle and wave?
6. What is bohr’s quantum condition?
7. Define hybridization.
8. What are the condition for effective hydrogen bonding?
9. What do you understand by dyal character of matter?
10. Define node or nodal surface.
11. Write difference between bonding M.O and anti-bonding M.O.
12. How Hydrogen molecule if formed?
13. Write strength of hydrogen bonding.
2. PERIODIC CLASSIFICATION – II
1. Why electron affinity of fluorine is less than that of chlorine?
2. Mention the disadvantages of pauling and mulliken scale?
3. Define electronegativity.
4. Define ionization energy.
5. What are the factors affecting ionization energy?
6. Define electron affinity.
7. Electron of noble gases are zero. Why?
3. P – BLOCK ELEMENTS
1. Write a note on plumbosolvency.
2. H3PO3 is diprotic. Why?
3. H3PO4 is triprotic. Why?
4. Prove that P2O5 is a powerful dehydrating agent.
5. Draw the Structure of PCl5 and H3PO3.
6. Discuss the oxidizing power of fluorine.
7. Write the uses of Neon.
8. What is inert pair effect?
9. What is the action of water on PCl5?
10. How is phosphene prepared in laboratory?
11. Write a short note on Holme’s signal.
12. Mention the uses of Helium.
13.How to prepare Potash Aluminum?
14. What is burnt aluminum?
15. Why HF is not stored in Silica (or) glass bottles?
16. Write note on Etchiny on glass.
17. What is inter halogen compound?
18. How Xenon fluoride compounds are prepared?
4. d – BLOCK ELEMENTS
1. Why d – Block Elements exhibit variable oxidation states?
2. Why transition elements form complexes?
3. Write a short note on aluminothermic process?
4. What happens when KI solution is added to an aqueous solution of
CuSO4?
5. What is the action of heat on copper sulphate crystals?
6. Why Zn+2 are colourless while Ni2+ salt are coloured?
7. Why most of the transition metal ions are coloured?
8. Most of the transition meta;s and their compounds have catalytic
activity. Why?
9. Why do transition elements form alloys?
10. Explain the action of heat on copper?
11. Write two alloys of copper and their uses?
12. Write short note on chrome plating.
13. What is philosopher’s wool?
14. What is spitting of silver?
15. How is gold reacts with aquaregia?
16. K2Cr2O7 is a powerful oxidizing agent. Explain?
17. What is Bordeaux mixture? Mention its uses?
18. What is the action of heat on calamine?
19. Write a note on purple of cassius.
20. What is transition elements?
21. Explain Chromyl Chloride test?
22. How Copper Sulphate is prepared?
23. Explain action in silver nitrate?
24. Mention the uses of Lunar Caustic?
7. NUCLEAR CHEMISTRY
1. What is a Q-value of nuclear reaction?
2. What is half life period of nuclear reaction?
3. What is binding energy of nucleus?
4. Explain the principle behind hydrogen bomb?
5. State theory of radioactive disintegration.
6. Write short note on nuclear reaction taking place in sun.
7. What are 4 types of decay serives?
8. SOLID STATE-II
1. Sketch a)Simple cubic b)Face centred cubic c)Body centred cubic.
2. What is vitreous state?
3. State Bragg’s law.
4. What are super conductors? Mention its application.
5. Define unit cell?
6. Write short note on metallic crystal.
7. Write short note on molecular crystals.
8. How are glasses formed?
9. What is imperfection in solids?
10. Explain types of ionic crystal?
11. Define point defeets.
12. Define “TC”.
13. How glass are formed?
9. THERMODYMANICS-II
1. What in Entropy? What are the units of entropy?
2. Mention the essential conditions for spontaneity ina chemical reaction?
3. State first law of thermodynamics?
4. What are the limitations of First law of thermodynamics?
5. State Trouton’s rule.
6. What are the substances that deviate from trouton’s rule?
7. When does entropy increase in a process?
8. How? G is related ?H and ?S? What is meaning of ? G=0?
10. CHEMICAL EQUILIBRIUM
1. Why do equilibrium reactions referred to as dynamic equilibrium?
2. What is equilibrium constant?
3. State Lechatelier’s principle?
4. Dissociation of PCl5 decrease in presence of increase in Cl2 Why?
5. Define reaction quotient?
6. Define Dissociation constant?
PHYSICAL CHEMISTRY
11. CHEMICAL KINEMATICS-II
1. What is activation energy?
2. Write the Arrehenius equation and Explain the term?
3. Give three examples of First order reaction.
4. Give three examples of Opposing reactions.
5. Define half life period of a reaction.
6. What are pseudo first order reaction? Give example.
7. What are parallel reaction? Give example.
8. What are Opposing reaction?
9. Define order of true reaction?
10. Mention the characteristics of first order reaction?
11. What is threshold energy?
12. SURFACE CHEMISTRY
1. What are active centers?
2. Why colloidal system in gas does not exist?
3. What are emulsions? Give examples.
4. What is Tyndall effect?
5. What is Brownian movement?
6. What is Auto Catalyst? Give example.
7. Define adsorption.
8. What are promoters? Give examples.
9. What is catalytic poison? Give examples.
10. What is peptisation?
11. Mention the medicinal application of colloids?
12. What is negative catalyst? Give examples.
13. What is Helmholtz double layer?
14. Why colloids are purified?
15. Define positive catalyst.
16. Define homogenous and heterogenous catalysts.
17. Define Induced catalyst.
13. ELECTRO CHEMISTRY-I
1. State Faraday’s First law.
2. State Faraday’s Second law.
3. What is electro chemical equivalent?
4. Define specific resistance.
5. Define specific conductance.
6. Define Equivalent conductance.
7. Define molar conductance.
8. What is cell constant?
9. State Kohlraush’s law.
10. What is common ion effect? Give example.
11. What is buffer solution?
12. State Ostwald’s dilution law.
13. What are indicators? Give example.
14. What is titration curve?
15. What is Henderson equation?
16. Why Methyl Orange is not a suitable indicator in the titration of
Strong base against weak acid?
17. Why Phenolphthalein is not a suitable indicator in the titration of
against weak base?
18. Mention the importance of first law of electrolysis.
15. ISOMERISM IN ORGANIC CHEMISTRY
1. Distinguish racemicform from mesoform?
2. Distinguish Enantiomers from diastriomer.
3. What are the conditions for optical activity?
4. What is racemic mixture? Give example.
5. What are cis and Trans isomer? Give example.
6. Transisomer are more stable than cis isomer?
7. Explain trans isomer in 1,3 butadienc?
ORGANIC CHEMISTRY
16. HYDROXY DERIVATIVES
1. How is terylene is prepared from glycol?
2. Write the conversion of ethylene glycol to 1,4-dioxan.
3. How does glycerol react with KHSO4?
4. Explain Dow’s process?
5. Alcohol cannot be used as solvent for a Grignard reagent. Why?
6. How can you identify alcohol consumed person?
7. What is saponification?
8. How will you convert Benzene diazonum chloride into phenol?
9. What happens when an alcohol react with alumina at 620k?
10. Write test for phenol.
11. Write Schotten-Baumann reaction.
12. Write coupling reaction.
13. Write Riemer tiemann reaction.
14. Write Lederer-Manasse reaction.
15. Write phthalin fusion.
16. How alocohol difference from inorganic hydroxides?
17. Lower alcohol are soluble in water but higher members are not. Why?
18. Explain Lucas test?
17. ETHERS
1. Ethers should not be heated to dryness. Why?
2. Ethers are the best solvent for Grignard reagent. Account for this.
3. Write Williamson Synthesis.
4. Mention the uses of diethyl ether.
5. How will you convert phenol in to anisole?
18. CARBONYL COMPOUNDS
1. What is Rosen mud’s Reduction? What is the purpose of adding BaSO4
in it?
2. What is Urotropine? Give its uses.
3.What happens when calcium acetate is dry distilled?
4. What is Formalin? Write its uses.
5. Write a note on haloform reaction.
6. How will you convert acetophenone to phenacyl bromide?
7. Give two tests for aldehydes.
8. Write Stephen’s reaction.
9. Write Clemmension reduction .
10. Write WolfKishner Reduction.
11. Write Pott’s rule.
12. How are the following conversion carried out
a) formaldehyde to para formaldehyde
b) acetaldehyde to paraldehyde
13. Write Claisen Schmidt reaction.
14. Write Benzoin Condensation.
15. How will you convert acetone into phorone?
16. Distinguish formaldehyde from acetaldehyde.
19. CARBOXYLIC ACID
1. What is Estirification? Give example.
2. Write three test for carboxylic acid.
3. Mention the uses of oxalic acid.
4. How will you convert lactic acid into lactide?
5. Formic acid cannot be prepared by Grignard reagent. Why?
6. Why Carboxylic acid having high boiling point?
7. Write HVZ reaction?
8. Write Kolbes electrolytic reaction.
9. How is Benzoic acid is prepared by Grignard reagent?
10. Write test for Salicyclic acid.
11. Acetamide exist as dimer. Why?
12. Mention the uses of lactic acid.,
13. What is the action of heat on Oxalic acid and succinic acid?
14. What is the action of ammonia on oxalic acid and succinic acid?
15. How will you convert Benzoic acid to Benzene?
16. How is Salicyclic acid prepared for phenol?
17. Mention the uses of benzoic acid.
18. Write Freidyl craft Acetylation.
19. What is Trans esterification? Give example.
20. ORGANIC NITROGEN COMPOUNDS
1. Write about the functional isomerism of nitro methane?
2. What is Gabrielphthalamide synthesis?
3. How is benzene diazonium chloride prepared?
4. Write a note on sand mayer reaction.
5. What happens when aniline is treated with phosgene?
6. Write carbylamines reaction?
7. Write mustard oil reaction.
8. Write diazotitation reaction.
9. How will you distinguish between aniline and ethylamine?
10. Write Gattermann’s reaction.
11. Write Gomberg Bachmann reaction.
12. What is chloro picrin? How it is prepared? Mention its uses.
22. CHEMISTY IN ACTION
1. Define chemotherapy.
2. What are anesthetics? Give example.
3. What are antibiotics? Give example.
4. In what way antacids are important?
5. Give the characteristics of dye.
6. What are analgesics? Give example.
7. What are antiseptic? Give example.
8. Write note nylon 66.
9. What are artificial sweetening agents? Give example.
10. What are antipyretics? Give example.
R. BALAJI M.Sc., M.Phil., B.Ed.
Ph. 9962001120
P.G. Asst in Chemistry.
SUCCESS TUTION CENTRE
CHEMISTRY
PART III
52. Atomic Structure
1. Explain the formation of oxygen molecule by molecular orbital theory.
2. Derive De-Broglie equation.
3. Discuss Davission and Germer’s experiment.
4. Explain the formation of N2 molecule by molecular orbital theory.
5. Discuss the shapes of S and P orbitals.
6. Briefly explain Molecular Orbital theory.
7. What are the salient features regarding hybridization?
8. Problem (Related to debroglie equ (or) Heisenberg’s principle).
9. Explain various types of Hydrogen bonds with examples.
10. Write significance of de-broglie waves.
11. Discuss the shapes of d-orbital.
12. Write importance of Hydrogen bonding.
53. d-Block elements
1. How is zinc extracted from it chief ore?
2. Explain the extraction of silver from it chief ore (Argenite).
3. How is gold extracted from it ore?
4. Explain how potassium dichromate is extracted from chromite ore.
5. Explain briefly the extraction of silver from silver coin.
6. How is Cr2O3 reduced to chromium by Almino Thermic process.
7. Explain extraction of copper.
54. f-Block elements
1. Compare the points of similarities and difference between lanthanides
and acitinides.
2. Explain the consequences of lanthanide contraction.
3. Describe the extraction of lanthanide from monazite sand.
4. What is lanthanide contraction? Discuss it causes and any two
Consequences.
5. Mention the uses of Lanthanides and Acitinides.
6. Explain the consequences of acitinides contraction.
55. Co-ordination and bio co-ordination compounds
1. Explain the postulates of Werner’s theory.
2. Using VB theory explain why [Ni(CN)4]2- is diamagnetic where as
[Ni(NH)3)4]2+ is paramagnetic.
3. For the complex K4[Fe(CN)6] mention a) IUPAC name
a) central metalion b) Geometry of the complex
c) Ligand d) Co-ordination number
4. Mention the types of hybridization and magnetic property of the following
Complexes using VB theory a) [FeF6]4 b) [Fe(CN)6]4
5. Explain co-ordination and ionization isomerism with suitable examples.
6. Mention the function of haemoglobin in natural process.
7. How chlorophyll is all important in environmental chemistry? Mention its
function.
8. In what ways differs [FeF6]4- differs from [Fe(CN)6]4-.
9. [CU(NH3)4]2+ is square planar, where as [NiCl4]2- is tetrachedral explain.
10. Explain i) Hydrate
ii) Linkage
iii) Ligand isomerism
11. Explain VB theory.
12. Define the following wards
1. Central metal ion.
2. Ligand.
3. Co-ordination n umber.
4. Co-ordination spere.
5. Chelafes.
13. Explain briefly Geometrical isomers of co-ordination compounds.
SECTION - B
56. Thermodynamics II
1. Write the various statements of second law of thermodynamics.
2. Write the characteristics of free energy.
3. Write the characteristics of Entropy.
4. What are spontaneous reactions? What are the condition for the
spontaneity of a process?
5. Problems.
57. Chemical Equilibrium II
1. Derive the relation Kp=Kc(RT) for a general chemical equilibrium.
2. Apply Lechatlier principle to Haber’s process of manufacture of
ammonia.
3. The dissociation equilibrium constant of HI is 2.06X10-2 at 458oC. At
Equilibrium concentration of HI and I2 are 0.36M and 0.15M respectively.
What is the equilibrium concentration of H2 at 458oC?
4. Derive the expressions for Kc and Kp for the dissociation of PCI5.
5. Discuss the conditions which favour the formation of SO3 in contact
process.
58. Chemical kinetics II
1. State the Characteristics of order of a reaction.
2. Explain the experimental determination of rate constant for the
Decomposition of hydrogen peroxide in aqueous solution.
3. Discuss the characteristics of first order reaction.
4. Explain the experimental determination of rate constant of acid
Hydrolysis of methyl acetate.
5. Derive the expression for the rate constant of first order reaction.
6. Write note on (i) Consecutive reactions ii) Parallel Reactions
(iii) Opposing reactions.
7. Write an account of the Arrhenius equation for rates of chemical
reactions
8. What are the differences between simple and complex reactions?
59. Electro Chemistry II
1. Calculate the emf of the cell having the cell reaction 2Ag++Zn 2Ag+Zn2+
Eocell =1.56v at 25oC When concentration of Zn2+=0.1M and Ag+=10M in
the solution
2. Derive Nernst equation.
3. The emf of the half cell Cu2+(aq) / cu(s) containing 0.01M cu2+solution is
+0.301v. calculate the standard emf of half cell.
4. Calculate the standard emf of the cell: Cd/Cd2+//Cu2+/Cu and determine
the cell reaction. The standard reduction potentials of Cu2+/Cu and
Cd2+ /Cd are 0.34v and -0.40v respectively. Predict the feasibility of the
Cell reaction.
5. Determine the standard emf of the cell and standard free energy change
Of the cell reaction. Zn, Zn2+//Ni2+, Ni. The standard reduction
Potentials (Eo) of Zn2+/Zn and Ni2+/Ni half cells are -0.76v and -0.25v
Respectively.
6. How emf of a half cell is determined?
7. Write notes on IUPAC convention of representation of a cell.
8. Explain Relation between EMF and Free Energy.
9. Write the differences between electrolytic and Electro chemical cells.
10. Problems (Related to Nernst Equ)
11. Explain lamiel cell.
12. Explain construction of SHE.
SECTION – C
60. Ethers.
1. How do ethers react with HI? Give 3 significance of the reaction?
2. Distinguish between anisole and diethylether.
3. How does diethyI ether react with the following reagents?
a) O2/long contact b) dil. H2SO4 c) PCI5
4. Write all possible isomers with the MF C4H10O and name them.
5. Give any three methods of preparing diethyl ether.
6. Mention the methods of preparation of anisole.
7. Illustrate electrophilic substitution reaction of anisole.
61. Carbonyl compounds.
1. Explain the mechanism of Cannizaro reaction
2. Write the mechanism of crossed aldol condensation of acetone
3. Explain the mechanism of aldol condensation of acetaldehyde.
4. Give the mechanism for claisen or claisen-schmidt reaction.
5. How is acetone converted to:
a) mesitylene b) mesityul Oxide c) Phorone
6. Write a note on a) Perkins reaction
b) Knoevenagal reaction
7. Distinguish between Acetaldehyde & Acetone (Acetaldehyde & Ketones)
8. Explain popott’s rule
9. Distinguish between HCHO and CH3CHO
10. Distinguish between CH3CHO and C6H5CHO
62. Carboxylic acids
1. How is lactic acid manufactured in large scale?
How can it be converted into cyclicdiester?
2. Account for reducing property of formic acid.
3. How is benzoic acid obtained from
a) CH2CH3 b) Phenyl cyanide c) Carbon di oxide
4. Distinguish between formic acid and acetic acid.
5. Explain the isomerism exhibited by carboxylic acids.
6. How is oxalic acid manufactured from sodium formate?
7. Give the mechanism involved in the esterification of a Carboxylic
Acid with Alcohol.
8. How are the following conversions carried out?
a. Salicylic acid aspirin
b. Salicylic acid Methyl salicylate
c. Lactic acid lactide
9. What happen when lactic acid is
a. treated with dil.H2SO4
b. Heated alone
c. Oxidised with alkaline KMnO4
10. Give any two methods of preparation of Lactic acid.
11. Explain the acetic strength of Carboxylic acids.
12. Write any three methods of preparation of Benzoic acid.
13. Explain the mechanism of Bromination of Salicylic acid.
14. Explain the mechanism of Kolbes reaction.
63. Chemistry in action.
1. Explain briefly the characteristics of rocket propellants.
2. Write a note on anesthetics’.
3. Write briefly on Buna rubbers.
4. Explain briefly on colour and structure of dye.
5. How is hylon 66 is prepared.
CHEMISTRY
PART – IV
64. a) Periodic classification II
1. Explain pauling method to determine ionic radii.
2. Explain the various factors that affect electron affinity.
3. How do electronegativity values help to find out the nature of
Bonding between atoms.
4. Explain pauling scale to determine Electro negativity.
5. How is atomic radii calculated from covalent bond length.
6. Explain the variation of IE along the group and period.
7. Explain mulliken scale? Determine electro negativity.
b) P-block Elements:
1. What are silicones? How are they prepared?
2. Give an account of manufacture of Lead.
3. How are the following compounds prepared from
phosphorous?
4. Mention the use of Fluorine.
5. What are inter halogen compounds? How they are prepared?
6. How are Noble gases isolated by Ramsay – Raleigh’s method?
7. How are Noble gases separated by Dewar’s method?
8. How is fluorine isolated from their fluorides by Dennis
Method?
9. Mention the uses of silicones.
10. Discuss anomalous properties of fluorine.
11. Discuss the structure of inter halogen compounds of AX and
AX5, type.
65. a) Co-ordination compounds and Bio co-ordination compounds
Refer Question No. 55.
b) Nuclear Chemistry
1. How are radioactive isotopes useful in medicine?
2. Write notes on radio carbon dating.
3. Explain the principle underlying the function of hydrogen bomb.
4. What is nuclear fission reaction? Write notes on nuclear power
Generator?
5. Differentiate chemical reactions from Nuclear Reactions.
6. Explain the nuclear reaction taking place in sun.
7. Explain the uses of Radio-active isotopes in reaction mechanism.
66. a) Solid state II
1. Explain schottky aand frenkel defects.
2. Explain Bragg’s spectrometer method.
3. Explain the nature of glass.
4. What are super conductors? Give their uses.
5. What is Bragg’s equation? Give its significance.
6. Write the properties of ionic crystals.
7. Explain AB and AB2 type ionic crystals with one example for
each.
8. Explain types of crystal b surface chemical.
9. What is ultrafiltration? Explain.
10. Write technical application of colloids.
b) Surface Chemistry
1. Write briefly about the adsorption theory of catalysis.
2. Write any three methods for the preparation of colloids by
dispersion method.
3. Write chemical methods for the preparation of colloids.
4. Write briefly on intermediate compound formation theory of
catalysis with an example.
5. Distinguish between physical adsorption and chemical
adsorption.
6. What is electro-osmosis? Explain?
7. Explain the factors affecting adsorption.
8. What are the characteristic of catalytic reactions?
9. Explain Adsorption theory of catalysis.
10. Write the application of Catalysis.
11. Explain electrophoresis.
12. What are Emulsion? Explain.
67. a) Electro Chemistry I
1. Explain Ostwald’s dilution law.
2. Explain Ostwald’s theory of indicators.
3. Derive Henderson equation.
4. Write a note on Quinonoid theory of indicators.
5. Write an account of the Arrhenius theory of electrolytic
dissociation.
6. Explain buffer action with example.
7. State and explain Kohlrausch’s law.
8. What are the differences between Electronic conduction and
Electrolytic conduction?
9. Write the evidences of Arrhenius theory of electrolyti
dissociation.
10. Explain the Faraday Law of Electrolysis.
b) Electro Chemistry II
1. Refer Question No.59
68. a) Isomerism in Organic Chemistry
1. Distinguish enantiomers from disenetiomers. Give an example
each.
2. Discuss the optical isomerism in tartaric acid.
3. Distinguish racemic form from mesoform with suitable
example.
4. Describe the confirmations of cyclochexanol. Comment on their
stability.
5. What is cis-trans isomerism? Give an example.
6. Klhat is a Racemic mixture? Explain with example.
7. Mesotartiaric is an optically inactive compounds with chiral
carbon atoms Justify.
8. Describe the D.L – System of designation of Configurations.
9. Discuss optical isomerism compounds.
b) Carboxylic acids
Refer Question No. 62
69. a) Organic Nitrogen Compounds.
1. Distinguish between primary, secondary and tertiary amines.
2. How are following conversions carried out.
i) nitrobenzene to phenylhydroxylamine
ii) Aniline tp phenyl isocynide
iii) Benzene diazonium chloride to biphenyl.
3. Write a note on the reduction of nitrobenzene under different
conditions.
4. Explain the Mechanism of Nitration of benzene.
5. Write the Mechanism of Hoffmann’s bromaamides reaction.
6. How do primary, secondary and tertiary amines reacts with
Nitrous acid?
7. Write a note on
a. Carbylamine reaction.
b. Mustard oil reaction.
8. Comment on the basic nature of amiline.
9. How are the following compounds obtained from benzene
diazonium chloride?
a) Phenol b) P – hydrozy azobenzene c) Biphenyl
b) Biomolecules
1. Discuss the structure if fructose in detail.
2. Prove the Structure of glucose.
3. What is peptide bond/Illustrate the formation of peptide bond.
4. What are the Carbohydrates? How are they classified.
5. Mention the Biological importance of Lipids.
6. Give the structure of following sugars.
a) glucose b)Fructose c)Sucrose.
70. a) 1. An organic compound (A) of molecular formula C7H6O is not reduced by Fehling’s solution but will undergo cannizaro reaction. Compound (A) reacts with aniline to give compound (B). Compound (A) also reacts with Cl2 the presence of catalyst to give compound (C) Identify (A),(B) and (C) and explain the reactions.
2. An organic compound (A) C2H6O liberates hydrogen on treatment with metallic sodium. (A) on mild oxidation gives (B) C2H4O which answers iodoform test. (B) when treated with con. H2SO4 undergoes polymerization to give (C), a cyclic compound. Identify compound A,B and C. Explain the reactions.
3. An organic compound A (C7H6O) reduces Tollen’s reagent. On treating with an alkali compound A forms B and C. B on treating with soda lime forms benzene C (C7H8O) is an antiseptic. Identify compounds A,B and C. Explain the reactions.
4. An organic Compound A of molecular formula C3H6O on reduction with LiA1H4 gives B. Compound B gives blue colour in Victor Meyer’s test and also forms a chloride C with SOCl2. The chloride on treatment with alc. KOH gives D. Identify A,B,C and D ad explain the reactions.
5. Compound A of molecular formula C2H4O gives red colour with decolourised Schiff’s reagent. Reaction of A with NaOH gives C2H8O2 (B) which is a bifunctional compound. Compound B can undergo dehydration when treated to give red colour with decolourised Schiff’s reagent. Identify A,B and C explain the reactions.
6. An organic compound (A) of molecular formula C6H6O gives violet colour with neutral FeCl3. (A) gives maximum of two isomers (B) and (C) when an alkaline solution of (A) is refluxed with CCl4. (A) also reacts with C6H5N2Cl to give the compound (D) which is read orange dye. Identify (A),(B) and (C) and (D) Explain with suitable chemical reactions.
b) 1. An element (A) belong to group number 11 and period number 4. (A) is a reddish browm metal. (A) also reacts with dil. HCL in the presence of air and gives compound (B). (A) also reacts with cone. HNO3 to give compound (C) with the liberation of NO2 Identify (A),(B) and (C). Explain the reactions.
2. Silver reacts with dil. HN3 to give compound (A) which on heating at 723K gives (B). (B) on further heating gives (C). Further the compound (A) reacts with KBr and gives (D) which is highly useful in photography. Identify (A), (B) and (D) and write the reactions.
3. The sulphide ore of an element of group 12 when roasted gave compound A which on reduction with carbon gave the element B. The carbonate C of this element is used for skin diseases. Identify A, B and C and write the required reactions.
4. An element A occupies group number 11 and period number 4. This metal is extracted from its mixture sulphide ore B. A reacts with dil. H2SO4 in the presence of air and forms C which is colourless. With water C gives a blue compound D. Identify A,B,C and explain the reactions.
5. An element (A) belonging to group No. 11 period number 4 is extracted from the pyrite ore. (A) reacts with oxygen at two different temperatures (A) reacts with oxygen at two different temperatures forming compounds (B) and (C). Also (A) reacts with conc. HNO3 to give (D) with the evolution of NO2. Find out (A), (B), (C) and (D). Explain the reactions.
c) 1. An organic compound (A) of molecular formula C3H8O gives turbidity with 5 – 10 min on reaction with anhydrous ZnCl2/HCl. Compound (A) on treatment with sodium hypochlorite gives carbonyl compound (B) which on further clorination gives compound (C) of molecular formula C3H3OCl3. Identify (A), (B) and (C). Explain the reactions.
2. An organic compound (A) of molecular formula C2H6O on treatment with PCl5 gives compound B. Compound (B) reacts with KCN to give a compound pf molecular formula C3H5N which undergoes acid hydrolysis to give compound (D) which on treatment with soda lime gives a hydrocarbon. Identify (A),(B),(C) and (D). Explain the reactions.
3. An organic compound A of molecular formula C6H6O gives violet colouration with neutral FeCl3. Compound A on treatment with metallic Na gives compound B. Compound B on treatment with CO2 at 400K under pressure gives C. This product on acidification gives compound D (C7H8O7) which is used in medicine. Identify A,B,C and D and explain reactions.
4. An organic compound A (C6H6O) gives maximum of two isomers B and C when an alkaline Solution of a is refluxed with CHCl3 at 333K. B on Oxidation gives an acid D. The acid D is also obtained by treating sodium salt A with CO2 under pressure. Identify A, B, C and D and explain the reactions.
5. When sucrose is made to react with conc. HNO3 in the presence on V2O5, C2H2O4 (A) is obtained. It’s calcium salt may form as stony deposits in kidneys. When A is heated to 473K it undergoes decarboxylation to give (B) which is found in red ants. With PCl5, B gives an unstable compound (C) which decomposes to give CO and HCL. Indentify A,B and C. Explain the reactions.
6. An aromatic aldehyde (A) of molecular formula C7H6O which has the smell of bitter almonds on treatment with (CH3CO)2O and CH3COONa to give compound (B) which is a aromatic unsaturated acid. (A) also reacts with (A) is the presence of alc. KCN to give dimmwe (C). Identify (A),(B) and (C) and Explain the reactions.
d) 1. What is the pH of a solution containing 0.5 M propionic acid and 0.5 M Sodium propionate? The ka of propionic acid is 1.34X10-5
2. Find the pH of Butter solution containing 0.20 mole per litre sodium acetate and 0.15 mole per litre acetic acid. Ka for acetic acid is 1.8X10-5
3. Calculate the PH of the butter contining 0.04 M NH4Cl and 0.02 M NH4OH. For NH4OH Kb is 1.8X10-5
PART – III
(Problems)
31. Calculate the effective nuclear charge experienced by 4s electron in potassium atom (S=16.80)
36. A substance is found to have a magnetic moment of 3.9BM. how many unpaired electrons does it contain?
37. 1. In the following radioactive decay, 92X232 89Y220.
How many α and β particles are ejected.
2. The atomic masses of Li, He and 1H1 are 7.01823 amu, 4.00387 amu and 1.00715 amu respectively. Calculate the energy evolved in reaction 3Li7+H1 22He4+ energy [1 amu = 931 Mev]
39. 1. What is the entropy change of an engine that operates at 100oC when 453.6 KCal of heat Is a supplied to it.
40. 1. The equilibrium constant Kc for A(g) B(g) is 2.5X10-2. The rate of constant of the forward reaction is 0.05 sec-1. Calculate the rate of the constant of the reverse reaction.
2. In the equilibrium H2+I2 2HI, the number of moles of H2, I2and HI are 1,2,3 moles respectively. Total pressure of the reaction mixture is 60 atm. Calculate the partial pressure of H2 and HI in the mixture.
3. Initially 0.1 mole of each of H2 and I2 gases and 0.02 mole of HI gas are mixed in a reaction vessel of constant volume at 300k. Predict the direction towards which the reaction proceeds. Kc = 3.5X10-2
41. 1. The initial rate of first order reaction is 5.2X10-6 mole lit-1s-1 at 298K, when the initial concentration of the reactant os 2.6X10-3 mol lit-1. Calculate the first order rate constant of the reaction at the same temperature.
2. Show that for a first order reaction time required for 99% completion is twice the time required for 90% completion the reaction.
42. 1. The half life period of a first order reaction is 20mins. Calculate the rate constant.
44. 1. The mass of the substance deposited by the passage of 10 ampere of current for 2 hours 40 minutes and 50 seconds is 9.65g. Calculate the electrochemical equivalent.
50. An organic compound (A) having molecular formula C2H7N is treated with nitrous acid to give (B) of molecular formula C2H6O which answers iodoform test. Identify (A) and (B) and explain the reaction.