Page 1 : 1., , Dehydration of alcohol., , CHAPTER 1, EXERCISES AND PROBLEMS, , (conc)H2SO 4, , CH 3 - CH 2OH  ,  ?, 160ºC, , C, CH 3 - CH 2  OH  H 2 SO 4 100, ,  ?, , What happen when ethanol is heated with concentrated sulphuric acid at 160°C?, 2., , Dehydro halogenation, , CH 3 - CH 2  Cl  KOH  ,  ?, ethanol, , What happen when ethyl chloride is by heating of alcoholicsolution with potassium hydroxide, 3., , Ozonolysis, , H O, , CHCl, , 3  ? , 2 ?, CH 2  CH 2  O3  , , , What happen when ethene is passed into ozone with chloroform and then treated with water, by zinc duct., 4., , hydro halogenation (M.R), , CH 2  CH 2  HBr ,  ?, , 17, M.R, , CH 3 - CH  CH 2  HBr ,  ?, What happen when propene is passed into (halogen acid) or hydorgen bromide solution., 5., , 1%KMnO, , 4 ?, CH 2  CH 2  H 2O  [O]   , , Hydroxylation, , What happen when ethene is passed into acidic solution of 1% potassium, permanganate solution., 6., , Dehydrogenation (H 2, , ) CH 3, , C, - CH 2 - OH Cu,300, , ,  ?, , When ethanol vapour is passed over freshly reduced copper., 7., , halogenation CH 2  CH 2  Cl2 light, ,  ?, , CCl, , 4 ?, CH 2  CH 2  Br2 , , reddish brown, 8., , Dehydro halogenation, , CH 2 - Br - CH 2 - Br  KOH ethanol,  ?, , What happen when ethene dichloride is heated with alcoholic solution of, , 9., , Hydration, , potassium hydroxide., , H SO dil, , CH  CH  H2 O 2 4, , Hg 2  ,60º C, , ethyne is passed over water with dilute sulphuric acid at 60°C, M.R, , 10. Hydrohalogenation, , CH  CH  HBr (excess)  ?, How would you obtained ethylidenebromide from ethyne, , 11. B., , Substitution of Copper I chloride[Formation of acetylide], , CH  CH  NH 3  Cu 2 Cl2 ,  ?, When acetylene is passed into ammonical solution of copper(I) chloride., 12. Substitution of silver oxide, , 1. Select the Isotopes from the following and gave reasons for your answer., 35, 24, 235, (i) 17, Cl , 238, 92 U , 12 Mg , 92 U, 35, 37, 40, (ii) 17, Cl , 238, 92 U , 17 Cl , 20 Ca, 2. Determine the number of protons , neutrons and electrons in the atoms of, 35, 40, 28, (i) 17, (iii), Cl (ii), 20 Ca, 13 Al, and write down the possible isotopes ., 3. Classify the following elements as alkali methals, alkaline earth, metals halogen and noble gas., , [Formation of acetylide], , CH  CH  Ag 2O  NH 3 ,  When acetylene is passed into silver oxide in ammonia., , Cl ,, , 11, , Na , 2 He ,, , 12, , Mg, , 4. Classify the following elements in their appropriate group number., 3, , Li ,, , 17, , Cl ,, , 11, , Na ,, , 18, , Ar ,, , 12, , Mg , 8 O , 9 F , 16 S, , 5. From the following elements, select the one which has the largest radius., Give reasons., 4 Be ,, 12 Mg , 20 Ca and N , B , F, 6. Explain which of the following groups has the largest ionization energy., 2.8.1 , 2.8.5 , 2.8.7 or Na , P , Cl, 7. Explain why Be has higher ionization energy than B ., 8. Explain why N has higher ionization energy than O ., 9. What type of chemical bond is formed between NH3 and H+ ion? Explain., 10. From the following elements, select the one which has the largest radius., Give reasons., (i) Fe2+ and Fe3+ (ii) Cl and Cl- (iii) Li, Na , K (iv) C,N,O, 11. An atom A has an atomic number of 12 whereas an atom B has an, atomic number of 17. Write down the, (i) essential electronic structures, (ii) positions in the periodic table, (iii) types of element and, (iv) type of bond that is formed between A and B ., 12. An atom A has an atomic number of 6 whereas an atom B has an, atomic number of 17. Write down the, (i) electronic structure of A and B., (ii) Give the group number and period number of A and B., (iii) What type of bond can be formed between A and B., (iv) Suggest the electron dot cross formula of the compound formed.

Page 2 : 6. How would you control the conditions such as temperature and pressure, to obtain more product?, CO(g) + 2H2 (g), + heat, CH3 OH ( l ), N2 ( g ) + 3H2 ( g ), 2 NH3( g ), +, heat, , 1., , 2., , 3., , 4., , 5., , 6., , CHAPTER 7, EXERCISES AND PROBLEMS, ( i ) Define Kinetic energy., ( ii ) Calculate the heat of formation of ethanoic acid , CH3 COOH ( l ), H  (combustion of carbon , graphite), Give ,, = -484 KJmol-1, = -372 KJmol-1, H  (combustion of hydrogen gas ), , H ( combustion of CH3 COOH ( l ), = -554 KJmol-1, (i) Define Hess's Law, (ii) Calculate the heat of formation of sugar, C12 H22 O11(s), if its heat of, combustion is -5040 kJ mol-1. The heat of formation of CO2(g) and, H2O(l) are -393 kJ mol-1 and -286 kJ mol-1, respectively., (i) Define "heat of formation of a compound"., (ii) Calculate the heat of combustion of butane gas, C4H10(g), if its heat, of formation is -2878 kJ mol-1. The heat of formation of CO2(g) and, H2O(l) are -393 kJ mol-1 and -286 kJ mol-1, respectively., (i) Give an example of endothermic reactions., (ii) Calculate the heat of combustion of di methyl ether CH3-O-CH3 (l) if its, heat of formation is -1572 kJ mol-1. The heat of combustion of C(graphite), and H2(g) are -393 kJ mol-1 and -286 kJ mol-1., Calculate the heat of combustion of carbon di sulphide CS2(l), if its heat, of formation is +287 kJ mol-1. The heat of formation of CO2(g) and, SO2(g) are -393.4 kJ mol-1 and -297 kJ mol-1, respectively., Calculate the heat of formation of gasoline (C8H18) (l) if the heats, of combustion of gasoline and carbon (s) are – 5434 kmol–1 and, - 393 kJmol–1. The heat of formation of water (l) is – 286 kJmol–1., , physical state, , 10, , ** Explain why Be has higher ionization energy than B ., Be = 1s2 2s2, B = 1s2 2s22p1, Be atom has fully filled sub-shell electrons and the electrons is diffcult to, remove., So, ionization energy of Be higher than that of B., ** Explain why N has higher ionization energy than O ., N = 1s2, 2s2 2p3, O = 1s2 , 2s2 2p4, N atom has half filled p sub-shell electrons and the electrons is difficult, to remove., So, ionization energy of N higher than that of O., , CHAPTER 2, EXERCISES AND PROBLEMS, 1. Which one diffuses faster in each of the following pairs under, comparable conditions?, [ N = 14 , S = 32 , O = 16 , H =1], CO and NO , H2S and SO2 , N2 and CO, 2. The pressure of oxygen and acetylene gas storage tanks is 7400 mHg. The, pressure of oxygen is 3400 mmHg. What is the pressure of acetylene gas ?, 3. The pressure of hydrogen collected over water at 27ºC is 76.7 mmHg., The vapour pressure of water at 27ºC is 26.7 mmHg. What is the pressure, of dry hydrogen ?, 4. What will be the volume of hydrogen chloride gas when 100 cm3 of hydrogen, and 50 cm3 of chlorine are mixed?, (All gases are measureed at the same condition), 5. You are provided with 5.6dm3 of oxygen gas at STP. Find the amount of, oxygen in moles and in number of molecules., 6. How many molecules are there in 16 g of sulphur ? ( S = 32 ), 7. A gas with volume of 5.6 dm3 of weighs 7 g., What is the relative molecular mass of the gas?, 8. What is the mass of hydrogen enclosed in 2.8 dm3 at STP? ( H = 1 ), 9. Helium gas diffuses 8 times as fast as unknown gas. What is the relative, molecular mass of the gas? ( He = 4 ), 3

Page 3 : 21. An electric current is passed in turn through solution of silver nitrate and, copper II sulphate in series. If 0. 5 g of silver is deposited at the cathode of, the first cell.Calculate the mass of copper deposited in the second cell., ( Ag = 108 , Cu = 63 ), 22. An electric current is passed in turn through solution of silver nitrate and, dilute sulphuric acid in series. If 0. 8 g of silver is deposited at the cathode, of the first cell.Calculate the volume of hydrogen liberated at 30 ºC and, 720 mmHg in the second cell. ( Ag = 108 , H=1 ), 23. On passing a steady current of 0.5 A for 25 minutes through a metal I nitrate, solution, 0.839 g of the metal is deposited. Calculte the relative atomic mass of, the metal. ( 1F = 96500C ), , 23. One mole of a gas occupies 27.0 litres, and its density is 1.41 gl-1 at a, particular temperature and pressure. What is the molecular weighs ?, What is the density of the gas at STP?, 24. 8g of oxygen gas is given. Calculate the moles, molecules, volume in dm3, at STP, and density of the gas. ( O =16 ), , CHAPTER 5, EXERCISES AND PROBLEMS, 1. What is the oxidation number for the underlined elements in each of the, following substances?, (i) HNO 3, (ii), H2 SO 4, (iii), H 2 CO 3, (iv) H 3 PO 4, (i), AgNO 3, (ii), KMnO4, (iii) Al2O3, (iv), Cr 2O 3, (i), Fe 2 O 3, (ii) PbO2, (iii), SnO2, (iv), HClO3, 2(i) MnO 4, (ii), Cr 2 O7, (iii), P4, (iv), O3, , 3., , 2. Does the following reaction represent oxidation-reduction (redox) reaction?, State which one is oxidized and which one is reduced . Give reason., (i), Fe 3+, +, Al, --------Fe, +, Al3+, (ii), PbO, +, C, --------Pb, +, CO, (iii), H2 S, +, Cl2, --------HCl, +, S, (iv), Fe 2O 3, +, 3CO --------2Fe, +, 3CO 2, (v), 2H 2O, +, 2Br2 --------4HBr +, O2, , 7., , 1., 2., , 4., 5., 6., , 8., , 9., 3. State which one is oxidized and which one is reduced . Give reason., Identify the oxidizing agents and reducing agents., (i), Br 2, +, H2, --------- 2HBr, (ii), Cu, +, CuCl2 --------- 2CuCl, (iii), 2Na, +, 2H2O --------- 2NaOH + H2, (iv), FeCl2, +, Cl2, --------- FeCl3, (v), H2O + SO2 + NaClO, --------- NaCl + H2SO4, 8, , 10., , CHAPTER 3, EXERCISES AND PROBLEMS, What volume of 2.0 M sulphuric acid is required to react with 5.0 g of zinc?, ( Zn = 65.4 ), How many cubic centimetres of 1M hydrochloric acid is needed to react, with 0.60 g of magnesium ? ( Mg = 24), What volume of water is needed to dilute a 0.1 M solution to make 2 dm3, of 0.025 M solution?, If 20 cm3 of 0.5 M sulphuric acid and 60 cm3 of 0.1 M sulphuric acid are, mixed what will be the molarity of the final solution?, Calculate the molarity of solution prepared by dissolving 0.44 g of NaOH, per 100 cm3 of solution? ( Na = 23 , O =16 , H =1 ), 25 cm3 of 0.2 M sodium carbonate solution required 20 cm3 of sulphuric, acid solution .Calculate the molar concentration of sulphuric acid . What, volume of water should be added to 20 cm3 of this sulphuric acid so that, the concentration becomes exactly 0.1 M ., 100 cm3 of hydrochloric acid solution is diluted to 1dm3 with distilled water ., If 32cm3 of this diluted acid is needed tp neutralize 20 cm3 of 0.4 M sodium, carbonate solution. Calculate the molarity of the original acid solution., 20 cm3 of a sodium carbonate solution required 21.5 cm3 of 0.45 M, hydrochloric acid solution to neutralize it. Calculate the molarity of sodium, carbonate solution and convert the concentration into g dm–3., (Na = 23, C = 12, O = 16), 4.5 g of a mixture of anhydrous sodium sulphate and sodium sulphate, decahydrate on heating to constant mass produces 2.7 g of anhydrous, salt. What percentages of anhydrous and hydrated salts are present in the, mixture? (H = 1, Na = 23, S = 32, O = 16), 6 g of a mixture of sodium chloride and anhydrous sodium carbonate were, made up to 500 cm3 of aqueous solution.25 cm3 of this solution required 20 cm3, of 0.1 M sulphuric acid for neutralization. Calculate the mass of sodium, chloride in this solution.(Na=23,C= 12,O=16,S=32), 5

Page 4 : 11. Calculate the molarity of a sodium carbonate solution prepared by adding, 50 g of pure sodium carbonate and sufficient water to make 1.5 dm3solutions., 21 cm3 of this solution was needed to neutralize 24.5 cm3 of sulphuric acid, solution.What is the concentration of sulphuric acid solution ?, (C = 12, O = 16, S=32, H = 1, Na = 23), 12. An approximately 0.02M potassium permanganate solution was standardized, against exactly 0.1 M iron (II)sulphate solution. 25 cm3 of the solution of the, iron(II)salt were oxidized by 24.6 cm3 of the permanganate solution., What is the molarity of the permanganate solution., 13. 4.0g of a mixture of sodium carbonate and sand in treated with an excess, of dilute hydrochloric acid and 0.22g of carbon dioxide is produced., Calculate the percentage by mass of sodium carbonate and sand in the, original mixture. (Na = 23, C = 12, O = 16), 14. Calculate the percentage of iron in a sample of iron wire from the following data:, 1.4 g of the wire were dissolved in excess of oxygen free dilutesulphuric acid and, the solution made up to 250 cm3, 25 cm3 of this solution needed 25.37 cm3 of, 0.0196 M potassium permanganate for oxidation., 15. How many cubic centimetres of 1M HCl must be diluted with water to make, 2 dm3 of 0.25 M solution? If 25 cm3 of sodium hydroxide neutralizes 23 cm3 of, this diluted solution, what is the molarity of sodium hydroxide solution?, 16. Vinegar contain the organic acid(acetic acid) HC2H3O2 .When 6 g of vinegar, was titrated with 0.105 M sodium hydroxide, 43 cm3 of this base had to be, added to reach the equivalence point.What is the percentage by mass of, acetic acid in this sample of vinegar. ( C = 12 , O =16 , H=1), 17. How many grams of sulphur would be precipitated on mixing 5 dm3 of, sulphur dioxide with 15 dm3 of hydrogen sulphide , if both gases originally at, 756 mmHg pressure and 25ºC ? ( S = 32), CHAPTER 4, EXERCISES AND PROBLEMS, 1. Write down the reactions at the cathode and anode for the electrolysis of, molten lead II bromide using platnium electrode., 2. What is meant by electroplating? Write down the reaction at the anode, and the reaction at the cathode for silver plating., 3. Write down the reactions at the cathode and anode for the electrolysis of, aqueous sodium chloride solution using Pt electrode., 6, , 4. Write down the reactions at the copper electrode in the electrolysis of, aqueous copper II sulphate solution., 5. Write down the reactions at the cathode and anode for the electrolysis of, silver nitrate solution using platnium electrode., 6. Write down the reactions at the cathode and anode for the electrolysis of, aqueous copper II sulphate solution using Pt electrode., 7. What is meant by electroplating? Write down the reaction at the cathode for, chromium plating., 8. Write down the reactions at the cathode and anode for the electrolysis of dilute, sulphuric acid solution using platnium electrode., 9. Write down the reactions at the cathode and anode for the electrolysis of, aqueous solution of alkali (NaOH) using platnium electrode., 10. Write down the reactions at the cathode and anode for the electrolysis of, saturated sodium chloride solution using Pt electrode., 11. Name the main anode and cathode products during the electrolysis of, sodium hydroxide solution., 12. Write dwon the equation for ionization of potassiumargentocyanide KAg(CN)2, solution and the reaction at the anode for silver plating., 13. Write down the electrochemical series., 14. Write difference between conductors and non-conductor,and the difference, between electrolytes and non-electrolytes., 15. Calculate the mass of silver in grams deposited by passing a steady current, of 0.8 A for two hours through an excess of silver nitrate solution., ( Ag = 108 , one Faraday = 96500 coulombs), 16. Calculate the mass of copper in grams deposited by passing a steady current, of 0.5 A for two hours through an excess of copperIIsulphate solution., ( Cu = 63 , one Faraday = 96500 coulombs), 17. On passing a steady current of 0.22 A for one hour through a metal IIsulphate, solution, 0.25 g of the metal is deposited. Calculte the relative atomic mass of, the metal. ( 1F = 96500C ), 18. A current of 0.6 A was switched on and allowed to flow for 20 minutes through, a dilute sulphuric acid. Calculate the volume of hydrogen at STP which would be, released during electrolysis ., 19. What will be the quantity of electricity required for the deposition of 5.4 g of, silver on the cathode.( Ag = 108 , 1F = 96500 C ), 20. What will be the quantity of electricity required for the deposition of 6.3 g, of copper on the cathode.( Cu = 63 , 1F = 96500 C ), 7

Page 5 : 10. Oxygen gas diffuses twice times as slow as unknown gas. What is the, molecular mass of the gas?, 11. Helium gas diffuses twice times as fast as a gas X .What is the molar, mass of the gas and relative density of the gas ?, 12. If it takes 3 minutes for 150 cm3 of oxygen to diffuse through a pin hole,, how long will it take for the same volume of hydrogen to diffuse through, same hole ? ( H = 1 , O =16), (or), If it takes 20 minutes for 100 cm3 of SO2 gas to diffuse through a pin hole,, how long will it take for the same volume of helium to diffuse through, same hole ? ( He = 4 , S = 32 , O =16), 13. What is the relative rate of diffusion of helium and sulphur dioxide ?, ( He = 4 , S = 32 , O =16), 14. If the relative density of a certain gas is 28. Calculate the its molecular, mass and the mass of one mole of the gas in grams. What would be the, volume occupied by 16 g of that gas at STP?, 15. A certain mass of the gas occupies 300 cm3 measured at 31ºC. At what, temperature in ºC will the gas occupy 285 cm3 at the same pressure?, 16. The pressure of a gas at 27ºC is 770 mmHg., What is the pressure of the gas at 87ºC at constant volume., 17. What is meant by STP ? Give their numerical value. At 22ºC and 745 mmHg, a gas occupies 175 cm3. What is the volume of the gas at STP?, 18. How many grams of zinc will have to be treated with dilute hydrochloric, acid to liberate 1.85 dm3 of hydrogen at 27ºC and 750 mmHg? ( Zn = 65), 19. How many grams of sodium carbonate will have to be treated with dilute, hydrochloric acid to liberate 1.15 dm3 of carbon dioxide at 22ºC and 755 mmHg?, ( C =12, Na=23, O=16), 20. 10 g of calcium carbonate is treated with dilute hydrochloric acid.The liberate gas, measured at STP is 1.661 dm3. Find the percentage purity of calcium carbonate., ( Ca=40,C=12,O=16), 21. 0.2 g of the gas occupies a volume of 185 cm3 measured over water at, 756 mmHg and 22ºC. Vapour pressure of water at 22ºC is 21.3 mmHg., What is the approximate molecular mass of the gas?, 22. The volume of a certain mass of gas collected over wateris227 cm3 at 12ºC, and 762mmHg.Vapour pressure of water at 12ºC is 10.5 mmHg.What would, be the volume of dry gas at 15ºC and 757 mmHg?, 4, , 4. Balance the following equations., (1), Cu, +, CuCl2 ------ CuCl, (2), Na, +, H 2 O ------- NaOH + H2, (3), FeCl2, +, Cl2, ------ FeCl 3, (4), H2O + SO2 +, NaClO ------- NaCl + H2SO4, (5), Cr 2 O7 2+ I- + H +, ------- Cr 3+, + I2, +, (6), Cl2, + NaOH, ------ NaCl + NaClO3 +, (7), H2O2 + Cr2 O72+ H +  Cr 3+ + O2 + H2O, , , ,  Mn O2 + N O3 + O H , (8), Mn O4 + N O 2 +H2O, , 1., , 2., , 3., , 4., , 5., , H2O, H2O, , CHAPTER 6, EXERCISES AND PROBLEMS, What will be the effect of increasing pressure and decreasing temperature, on the following equilibrium ? Give reasons for your answers., Name and state principle that you have applied., Ca CO3 ( s ) + heat, CaO ( s ) + CO2 ( g ), (i) What are the factors affecting the chemical equilibria., (ii) What is the effect of reduced pressure on the following equilibrium ?, Give reason for your answer., H2 ( g ) + I2 ( g ), 2HI ( g ), There is an absorption of heat in the formation of methanol from H2 and CO., CO(g) + 2H2 (g), CH3 OH ( l ), What will be the effect of (i) increasing temperature, (ii) decreasing pressure? Give reasons., How would you change the temperature and the pressure on the following, equilibrium so that you could get highest quantity of SO3 on the right, hand side?, 2SO2(g) + O2(g), 2SO3(g) + heat, (i) Predict the effect of increasing concentration of SCN- ions on the, following equilibrium., Fe3+(aq) + SCN -(aq), FeSCN2+(aq), (ii) What will be the effect of decreasing temperature on the, following equilibrium., 4NH3(g) + 5O2(g), 4NO(g) + 6H2O(l) + heat, , 9

Page 6 : 13. From the following elements, A (2.8.1) , B (2.8.5) , C (2.8.7) , D ( 2.8.8), (i) Which element has the highest ionization energy ?, (ii) Which element has the highest electron affinity ?, (iii) Which element have a valence of 1 ?, (iv) Which element is a noble gas ?, 14. Answer the following cquestions., (i) How many electrons does a potassium atom lose in forming the K+ ?, (ii) What do we call the bonding which involves electron trasfer ?, (iii) Write down the electron dot cross structure of the compound , BCl3?, (iv) What is the charge and mass of a proton ?, (v) What type of bonding do we find in molecules ?, (vi) What do we call the bonding which involves electron sharing ?, (vii)Which partcle contain 16 neutrons, 15 protons, and 15 electrons ?, (viii)How are the elements arranged in the modern periodic table ?, (ix) What type of bond exists in the solid metals ?, , 1., , 2, , 3., , 4., 5., , (x) Describe the differences between covalent compound and, ionic compounds ?, Ans 1., 2., 3., , covalent compounds, low melting point, contain molecules, do not conduct electricity,, non electrolyte, 4. liquid and gases ,, vaporize easily, , ionic compounds, high melting point, do not contain molecules, conduct electricity ,, electrolyte, solid ,, do not vaporize easily, , ** What type of chemical bond is formed between NH3 and H+ ion? Explain., co ordinate bond, , 6., 7., 8., , 9., , 10., , CHAPTER 13, EXERCISES AND PROBLEMS, (i) Calculate the concentration of H+ and OH- in 0.0001 M solution of, caustic soda., (ii) Calculate the concentration of H+ and OH- in 0.005 M solution of, nitric acid., (i) Calculate the pH of an aqueous solution containing 0.73 g of HCl per dm3., ( H=1,Cl=35.5 ), (ii) Calculate the pH of an aqueous solution containing 0 . 2 g of NaOH per dm3., ( H=1,Na=23,O = 16 ), (i) Calculate the concentration of H+ of the solution having the pH value of, 6.699 and pOH value of 10.1, (ii) Calculate the concentration of H+ of the solution having the pH value of, 3.92 and pOH value of 8.6, Calculate the pH of a buffer solution containing 0.02 mol of methanoic acid, ( Ka= 1.8x10-7)and 0.002 mol of sodium methanoate per 100 cm3., Calculate the pOH of a buffer solution containing 0.05 mol of ethanoic acid, ( pKa= 4.6 )and 0.05 mol of sodium ethanoate per dm3., Would the pH of a solution of sodium ethanoate be greater or less than 7 ?, Explain this result clearly., Calculate the pH of a buffer solution containing 0.03 mol of ammonium, hydroxide ( Kb= 4.5 x 10-7)and 0.03 mol of ammonium chloride per 500 cm3., Calculate the pH of a buffer solution containing 0.46 g of methanoic acid, ( Ka = 4.8x10-5 ) and 0.34 g of sodium methanoate per 1000 cm3., (Na =23 , C = 12 , O = 16 , H = 1), Calculate the pOH of a buffer solution containing 0.06 g of ethanoic acid, ( pKa = 4.6 ) and 0.082 g of sodium ethanoate per dm3., (Na =23 , C = 12 , O = 16 , H = 1), Salt hydrolysis ......................................, , +, , x, , º, ºx N ºº, ºx, , H, , Nitrogen atom shares its lone pair electrons to H+ ion., , 2, , 11