Chapterwise Chemistry Question Bank-1 PDF

AK TUTORIALS Worksheet Subject : Chemistry ___________________________________________________________________________ Ionic Equilibria : 1. Explain different types of electrolytes. 2. Define Degree o...

AK TUTORIALS Worksheet Subject : Chemistry ___________________________________________________________________________ Ionic Equilibria : 1. Explain different types of electrolytes. 2. Define Degree of Dissociation. 3. Explain Arrhenius theory of acid and bases. 4. Explain Bronsted-Lowry theory of acid and bases. 5. Explain Lewis Theory of Acid and Bases. 6. Explain the Amphoteric nature of water. 7. Explain Ostwald's dilution law for weak acid and weak base. 8. What is Autoionization of water? 9. Derive pH + pOH = 14 10. Explain Acidity Basicity and Neutrality of Aqueous Solution. 11. What are Different types of salts? 12. Define Hydrolysis of Salts. 13. Define Buffer Solution and explain different types of Buffer Solution. 14. What is Henderson Hasselbalch equation ? 15. Give the properties of Buffer Solution. 16. Explain the Applications of Buffer Solution 17. Short Note on Solubility Product. 18. Obtain the Relation between Solubility and Solubility Product. 19. Give the condition for Precipitation. 20. Explain Common Ion Effect. Formulas : 𝑁𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 𝑑𝑖𝑠𝑠𝑜𝑐𝑖𝑎𝑡𝑒𝑑 1. Degree of dissociation (α) = 𝑇𝑜𝑡𝑎𝑙 𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 2. Ostwald’s dilution law : α = 1/ 𝐶 or α = 𝑉 + 3. pH of solution = − 𝑙𝑜𝑔10[𝐻3𝑂 ] + 4. pOH = − 𝑙𝑜𝑔10 𝑂𝐻 [ ] 5. pH + pOH = 14 6. Percent dissociation = α x 100 2 7. 𝐾𝑎 = 𝐾𝑏 = α 𝑐 [𝑠𝑎𝑙𝑡] 8. pH=p𝐾𝑎 + 𝑙𝑜𝑔10 [𝑎𝑐𝑖𝑑] [𝑠𝑎𝑙𝑡] 9. pH=p𝐾𝑏 + 𝑙𝑜𝑔10 [𝑏𝑎𝑠𝑒] Questions : 1. Acetic acid is 5 % ionised in its decimolar solution. Calculate its dissociation constant of acid. 2. A weak monobasic acid is 0.02 % dissociated in 0.01 M solution. Calculate dissociation constant.  −5 3. Dissociation constant of acetic acid is 1.8 x 10. Calculate percent dissociation of acetic acid in 0.01 M solution. 4. Calculate pH and pOH of 0.01 M HCl solution. 5. Calculate the pH of 0.01 M sulphuric acid. + 6. The pH of the solution is 6.06. Calculate its 𝐻 ion concentration. − −4 [ ] 7. In NaOH solution 𝑂𝐻 is 2.87 × 10. Calculate the pH of the solution. 8. The pH of rain water collected in a certain region of Maharashtra on a particular day was 5.1. + Calculate the 𝐻 ion concentration of the rain water and its percent dissociation. 9. pH of a weak monobasic acid is 3.2 in its 0.02 M solution. Calculate its dissociation Constant. −13 3 3 10. The solubility product of AgBr is 5.2 x 10. Calculate its solubility in mol/𝑑𝑚 and in g/𝑑𝑚 (Molar mass of AgBr = 187.8 g/mol). 11. A solution is prepared by mixing equal volumes of 0.1 𝑀𝑔𝐶𝑙2 and 𝑁𝑎2𝐶2𝑂4 at 293 K. Would −5 Mg𝐶2𝑂4 precipitate out ? 𝐾𝑠𝑝 of Mg𝐶2𝑂4 at 293 K is 8.64 x 10. −4 12. Calculate the pH of the Buffer solution containing 0.05 mol HF per litre. (𝐾𝑎 = 7. 2 ×10 ) 13. Calculate the pH of buffer solution composed of 0.1 M weak base BOH and 0.2 M of its salt −5 BA. (𝐾𝑏 = 1. 8 ×10 𝑓𝑜𝑟 𝑤𝑒𝑎𝑘 𝑏𝑎𝑠𝑒)  AK TUTORIALS Worksheet Subject : Chemistry ___________________________________________________________________________ Solid State : Theory : 1. Difference Between Amorphous and Crystalline Solid. 2. Define Isomorphism and Polymorphism. 3. Compare Ionic Covalent Molecular and Metallic Solids. 4. Calculate the packing efficiency of a simple cubic unit cell. 5. Calculate the packing fraction of the body centred unit cell. 6. Calculate the packing fraction of fcc/hcp/ccp. 7. Define Unit cell and Coordination Number. 8. State the Coordination number in Close packed structure. 9. Short Notes : i) Schottky defect ii) Frenkel defect iii) Vacancy Defect iv) Impurity Defect v) Non Stoichiometric Defects 10. Explain Conductors, Insulators and Semiconductors. 11. Explain Different types of Semiconductors. 12. Compare Diamagnetic , Paramagnetic and ferromagnetic. 13. Explain Valence Band, Conduction Band , Band gap. Formulas: 𝑀𝑛 Density : ρ = 3 𝑎 𝑁𝐴 Type of Unit Cell z r C.N Packing Efficiency Simple Cubic (SCC) 1 𝑎 6 52.4% 𝑟= 2 Body Centre (BCC) 2 𝑟= 3𝑎 8 68% 4 Face Centred (FCC/HCP/CCP) 4 𝑟= 2𝑎 12 74% 4 Number of Particles and unit cells in metallic crystal : 𝑥𝑛 1) Number of Particles in x gm = 3 ρ𝑎 𝑥 2) Number of unit cells in x gm metal = 3 ρ𝑎 𝑉 3) Number of unit cells in Volume V of metal : 3 𝑎 Questions :  3 1. A unit cell of iron crystal has edge length 288 pm and density 7.86 𝑔/𝑐𝑚. Find the number of −1 atoms per unit cell and type of Crystal Lattice.(Molar mass of iron = 56 g 𝑚𝑜𝑙 ) 2. An Element having bcc geometry has atomic mass 50. Calculate the density of the unit cell if its edge length is 290 pm. 3 3. An element has a bcc structure with a cell edge of 288 pm. The density of element is 7.2 𝑔/𝑐𝑚. How many atoms are present in 208 g of this element ? 𝑔 4. FCC crystal lattice of copper has density of 8.966 3.Calculate the volume of the unit cell. 𝑐𝑚 −1 (Molar mass of Copper = 63.5 g 𝑚𝑜𝑙 ) 3 5. An Atom crystallises in fcc crystal lattice and has a density of 10 𝑔/𝑐𝑚 with unit cell edge length of 100 pm. Calculate number of atoms present in 1 g of crystal 6. A compound forms hcp structure. What is the total number of voids in 0.5 mol of it? How many of these are tetrahedral voids? 7. A compound is formed by two elements M and N.The elements N formed CCP and atoms of M occupy 1/3rd of tetrahedral voids. What is the formula for the compound? 8. Atoms C and D form fcc crystalline structure.Atom C is present at the corners of the cube and D is at the faces of the cube What is the formula of the compound? 9. An element A and B constitute bcc type crystalline structure Element A occupies bcc position at the corners of the cube What is the formula of the compound? What are the coordination number of A and B? 10. What is the ratio of octahedral holes Aluminium crystallises in a cubic close packed structure. Its metallic radius is 125 pm What is the length of the side of unit cell? How many unit cells are there 3 in 1 𝑐𝑚 of aluminium ?  AK TUTORIALS Worksheet Subject : Chemistry ___________________________________________________________________________ CHEMICAL KINETICS : 1. Define Rate Law and Rate Constant and Rate of Reaction. 2. Define Order of Reaction. 3. Difference Between Order of Reaction and Molecularity. 4. What is rate determining step and Reaction Intermediate? 5. Derive the integrated rate law for first order reaction. 6. Obtain the relationship between rate constant and half-life of first order reaction. 7. How will you represent first order reactions graphically? 8. Derive the integrated rate law for first order reaction in terms of pressure. 9. What is the zeroth order reaction? Derive its integrated rate law. 10. Show that the half life of zero order reaction is directly proportional to initial concentration of reactants. 11. What are pseudo first order reactions explain with example. 12. What is the activation energy of a reaction? 13. What are requirements for the colliding reactant molecules to lead to products? 14. Write Arrhenius equation and explain terms involved in it 15. How will you determine activation energy graphically using Arrhenius equation? 16. Derive the relation between rate constant and temperature. 17. Explain graphically the effect of temperature on rate of reaction. 18. How catalysts increase the rate of reaction explain graphically. FORMULAS: 2.303 [𝐴]0 ⮚ For First order reaction : 𝑘 = 𝑡 𝑙𝑜𝑔10 [𝐴]𝑡 0.693 ⮚ Half life : 𝑡1/2 = 𝑘 −𝐸𝑎/𝑅𝑇 𝐸𝑎 ⮚ Arrhenius equation : 𝑘 = 𝐴𝑒 or 𝑙𝑜𝑔10 𝑘 = 𝑙𝑜𝑔10 𝐴 − 2.303𝑅𝑇 −𝐸𝑎/𝑅𝑇 ⮚ Fraction of successful collision : 𝑓 = 𝑒 𝑘2 𝐸𝑎 ⮚ Temperature dependence : 𝑙𝑜𝑔10 = ⎡ 1 − 1 ⎤ 𝑘1 2.303𝑅𝑇 ⎢𝑇 𝑇2 ⎥ ⎣ 1 ⎦ Questions : a. For the reaction 2𝑁2𝑂5→4𝑁𝑂2 + 𝑂2 in liquid bromine , 𝑁2𝑂5 𝑑𝑖𝑠𝑎𝑝𝑝𝑒𝑎𝑟𝑠 𝑎𝑡 a rate of 0.02 −3 −1 𝑚𝑜𝑙 𝑑𝑚 𝑠𝑒𝑐. At what rate 𝑁𝑂2 𝑎𝑛𝑑 𝑂2 𝑎𝑟𝑒 𝑓𝑜𝑟𝑚𝑒𝑑 ? What would be the rate of reaction? − 2− − 2− b. For the reaction 3 𝐼 + 𝑆2𝑂8 ⟶𝐼3 + 2𝑆𝑂4 − − 2− Calculate the rate of formation of 𝐼3 , the rates of consumption of 𝐼 and 𝑆2𝑂8 and the overall 2− −3 −1 rate of reaction if the rate of formation of 𝑆𝑂4 is 0.022 𝑚𝑜𝑙 𝑑𝑚 𝑠𝑒𝑐. c. Write the rate law for the reaction A + B ⟶ P from the following table : −3 −1 −3 −1 Initial rate [A] 𝑚𝑜𝑙 𝑑𝑚 𝑠𝑒𝑐 [B] 𝑚𝑜𝑙 𝑑𝑚 𝑠𝑒𝑐 −3 −1 (Initial) (Initial) 𝑚𝑜𝑙 𝑑𝑚 𝑠𝑒𝑐 i. 0.4 0.2 −5 4 x 10 ii. 0.6 0.2 −5 6 x 10 iii. 0.8 0.4 −4 3.2 x 10 For the reaction 2A + B ⟶ P Find the rate law : [A] [B] Rate 0.3 0.05 0.15 0.6 0.05 0.30 0.6 0.2 1.20 2 d. For the reaction 2𝑁𝑂𝐵𝑟⟶2𝑁𝑂2 + 𝐵𝑟2 , the rate law is rate = 𝑘[𝑁𝑂𝐵𝑟]. If the rate of the −6 −1 −1 −3 −1 reaction is 6.5 x 10 mol 𝐿 𝑠 when the concentration of NOBr is 2 x 10 mol 𝐿 , what would be the rate constant for the reaction ? −2 −3 −1 −3 e. The rate of the reaction A + B ⟶ P is 3.6 x 10 mol 𝑑𝑚 𝑠 when [A] = 0.2 mol 𝑑𝑚 and[B] = −3 0.1 mol 𝑑𝑚. Calculate the rate constant if the reaction is first order in A and second order in B. f. The half life of the first order reaction is 990 s. If the initial concentration of the reactant is 0.08 3 mol/𝑑𝑚 what concentration would remain after 35 min ? −2 −1 g. Consider a reaction A ⟶ Products , with k = 2 x 10 𝑠𝑒𝑐. Calculate the concentration of A −3 remaining after 100 s if the initial concentration of A is 1 𝑚𝑜𝑙 𝑑𝑚. −3 h. In a first order reaction the concentration of reactant decreases from 20 𝑚𝑜𝑙 𝑑𝑚 to 8 −3 𝑚𝑜𝑙 𝑑𝑚 in 38 minutes. What is the half life of reaction. i. In a first order reaction 60 % of the reactant decomposes in 45 minutes. Calculate the half life for the reaction ? j. A first order reaction takes 40 minutes for 30 % decomposition. Calculate its half life. k. The half life of the first order reaction is 1.7 hours. How long will it take for 20 % of the reactant to react. l. Show that the time required for 99.9 % completion of first order reaction is 3 times the time required for 90 % completion. m. What fraction of molecules in a gas at 300 K collide with an energy equal to activation energy of 50 kJ/mol ? 3 −1 −1 n. The rate constant of a reaction at 500 ℃ is 1.6 x 10 𝑀 𝑠.What is the frequency factor of the reaction if its activation energy is 56 kJ/mol ? 4 o. The rate constant for the first order reaction is given by 𝑙𝑜𝑔10 𝑘 = 14. 34 − 1. 25 ×10 T.Calculate activation energy of the reaction. p. The energy of activation for the first order reaction is 104 kJ/mol. The rate constant at 25℃ is −5 −1 3.7 x 10 𝑠. What is the rate constant at 30 ℃ ? ( R = 8.314 J/K mol ) q. What is the energy of activation of a reaction whose rate constant doubles when the temperature changes from 303 K to 313 K ?  AK TUTORIALS Worksheet Subject : Chemistry ___________________________________________________________________________ SOLUTIONS 1. Define Solubility and explain the factors affecting solubility. 2. Explain Henry’s Law and its exception. 3. Derive the equation for Raoult Law. 4. Explain Positive and Negative Deviations from Raoult’s law. 5. Define Colligative Properties. 6. Difference Between Ideal and Non-Ideal Solution. 7. Using Raoult’s law how will you show that ∆𝑃 = 𝑃1° 𝑥2 ? 8. Explain Relative Lowering of Vapour Pressure. 9. Explain Boiling point elevation with a diagram 10. Explain Freezing point elevation with a diagram 11. Define and write the SI units of ebullioscopic and cryoscopic constant. 12. Short Note: i) Osmosis ii) Reverse Osmosis iii) Osmotic Pressure 13. Derive the relation between osmotic pressure and concentration of solution. 14. Define Hypotonic, Isotonic and Hypertonic Solutions. 15. Explain van’t Hoff factor. 16. Derive the relation between van’t hoff factor and the degree of dissociation. Formulas: 1. S =𝐾𝐻 𝑃 𝑛𝑜 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 (𝑠𝑜𝑙𝑢𝑡𝑒 𝑜𝑟 𝑠𝑜𝑙𝑣𝑒𝑛𝑡) 2. Mole fraction = 𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 𝑜 𝑜 3. Partial pressure 𝑃1 = 𝑃1𝑥1 , 𝑃2 = 𝑃2𝑥2 , 𝑃 = 𝑃1 + 𝑃2 4. No of moles = mass/molar mass 𝑜 𝑃1−𝑃1 𝑊2𝑀1 5. 𝑜 = 𝑊1𝑀2 𝑃1 ∆𝑇𝑏 6. 𝑚= 𝐾𝑏 Here m =molality 1000𝐾𝑏𝑊2 7. 𝑀2 = ∆𝑇𝑏𝑊1 ∆𝑇𝑏 8. 𝑚 = 𝐾𝑓 1000𝐾𝑓𝑊2 9. 𝑀2 = ∆𝑇𝑏𝑊1 𝑛2𝑅𝑇 𝑊2𝑅𝑇 10. π = 𝑉 = 𝑀𝑅𝑇 = 𝑀2𝑉 1000 𝑊2 11. 𝑚 = 𝑊1𝑀2  ∆𝑇𝑓 ∆𝑇𝑏 ∆𝑃 π 12. 𝑖 = = (∆𝑇𝑓)0 (∆𝑇𝑏)0 = (∆𝑃)0 = (π)0 𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒 𝑎𝑓𝑡𝑒𝑟 𝑑𝑖𝑠𝑠𝑜𝑐𝑖𝑎𝑡𝑖𝑜𝑛 13. 𝑖 = 𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠 𝑑𝑖𝑠𝑠𝑜𝑙𝑣𝑒𝑑 𝑖−1 14. ∝ = 𝑛−1 Questions: −4 1. The solubility of 𝑁2 gas in water at 25 ℃ and 1 bar is 6.85 x 10 mol/L. Calculate Henry’s constant and molarity of 𝑁2 gas dissolved in water under atmospheric conditions when the partial pressure of 𝑁2 in the atmosphere is 0.75 bar. −2 2. Henry’s constant for solubility of methane in benzene is 3.25 x 10 mol/L atm at constant temperature. Calculate the solubility of methane at 1 bar pressure and at the same temperature. 3. A mixture of benzene and toluene contains 30% by mass of toluene. At 30 ℃ , the vapour pressure of pure toluene is 36.6 mm Hg and that of pure benzene is 118.2 mm Hg. Assuming that the two liquids form ideal solutions calculate the total pressure and the partial pressure of each constituent above the solution at 30℃. 4. The vapour pressure of water at 20 ℃ is 17 mm Hg. What is the vapour pressure of a solution containing 2.8 g urea in 50 g of water? 5. A solution is prepared by dissolving 394 g of a nonvolatile solute in 622 g of water. The vapour pressure of solution is found to be 30.74 mm Hg at 30℃. If the vapour pressure of water at 30 ℃ is 31.8 mm Hg, what is the molar mass of the solute? 6. The vapour pressure of benzene (molar mass 78 g/mol) at a certain temperature is 640mm of Hg. A non-volatile and non-electrolyte solid weighing 2.315 g is added to 40 g of benzene. The vapour pressure of the solution is 600mm of Hg. What is the molecular mass of the solid substance? 7. A solution of citric acid 𝐶6𝐻8𝑂7 in 50 g of acetic acid has a boiling point elevation of 1.76 K. If 𝐾𝑏 for the acetic acid is 3.07 K kg/mol, what is the molality of the solution? 8. The normal boiling point of ethyl acetate is 77.06 ℃. A solution of 50 g of a non-volatile solute is 150 g of ethyl acetate boils at 84.27 ℃. Evaluate the molar mass of solute if 𝐾𝑏 for ethyl acetate is 2.77 ℃ kg/mol. 9. A 5 % aqueous solution (by mass) of cane sugar (molar mass 342 g/mol) has freezing point of 271 K. Calculate the freezing point of 5 % aqueous glucose solution. 10. An aqueous solution of a certain organic compound has a density of 1.063 g/mL, an osmotic pressure of 12.16 atm at 25 ℃ and a freezing point of -1.03℃. What is the molar mass of the compound? 11. 3.4 g of 𝐶𝑎𝐶𝑙2 is dissolved in 2.5 L of water at 300 K. What is the osmotic pressure of the solution ? van’t Hoff factor for 𝐶𝑎𝐶𝑙2 is 2.47. 12. 0.2 m aqueous solution of KCl freezes at -0.680 ℃. Calculate van’t Hoff factor and osmotic pressure of solution at 0 ℃ (𝐾𝑓 for water is 1.86 K kg /mol). 13. A 0.15 m aqueous solution of KCl freezes at -0.510 ℃. Calculate van’t Hoff factor and osmotic pressure of solution at 0 ℃. Assume volume of solution equal to that of water.  14. At 25 ℃ , a molal solution of 𝐶𝐻3𝐶𝑂𝑂𝐻 is 1.35 % dissociated in an aqueous solution. Calculate freezing point and osmotic pressure of the solution assuming molality and molarity to be identical. AK TUTORIALS Worksheet Subject: Chemistry ___________________________________________________________________________ THERMODYNAMICS : 1. Define System and Surrounding and explain different types of System. 2. Difference between Intensive and Extensive property. 3. Define State Function and Path Function. 4. Define the Reversible Process and State its features. 5. Derive the expression for Pressure-Volume Work. 6. Derive the expression for Maximum Work 7. State the First law of Thermodynamics and explain all the processes. 8. Define Enthalpy and derive the relation between ∆𝐻 𝑎𝑛𝑑 ∆𝑈 9. How Work done is related to the number of moles. 10. Explain all the enthalpy with an example. 11. Explain Hess law and its Application. 12. Give the key points of the Spontaneous process 13. Define Spontaneous and Non Spontaneous Processes 14. Define Entropy State its formula and SI unit. 15. Explain the Second law of Thermodynamics. 16. Explain how change in entropy is related to Spontaneous and Non Spontaneous Processes. 17. Obtain the relationship between ∆𝐺 𝑎𝑛𝑑 ∆𝑆𝑡𝑜𝑡𝑎𝑙 18. Obtain the relation between Gibbs function and Equilibrium constant. Numericals 3 3 1. Three moles of an ideal gas are expanded isothermally from 15 𝑑𝑚 to 20 𝑑𝑚 at 3 constant external pressure of 1.2 bar. Estimate the amount of work done in 𝑑𝑚 bar and J. 3 3 2. Two moles of an ideal gas are expanded isothermally from a volume of 300 𝑐𝑚 to 2500 𝑐𝑚 at 300 K 3 against a pressure of 2 bar. Calculate the work done in 𝑑𝑚 bar and joules. 3 3 3. Calculate the work done during synthesis of 𝑁𝐻3 in which volume changes from 8 𝑑𝑚 to 4 𝑑𝑚 at a constant external pressure of 43 bar. In what direction the work energy flows ? 3 5 4. One mole of an ideal gas is compressed from 500 𝑐𝑚 against a constant pressure of 1.2 x 10 Pa. The work involved in the pressure in 36 J. Calculate the final volume. 5. Calculate the maximum work when 24 g of 𝑂2 are expanded isothermally and reversibly from the pressure of 1.6 bar to 1 bar at 298 K. 6. 2 moles of an ideal gas are expanded isothermally and reversibly from 20 L to 30 L at 300 K. Calculate the work done. 7. 22 g of 𝐶𝑂2 are compressed isothermally and reversibly at 298 K from initial pressure of 100kPa when the work obtained is 1.2 kJ Find the final pressure. 8. Three moles of an ideal gas are compressed isothermally and reversibly to a volume of 3 2 𝑑𝑚. The work done is 2983 J at 295 K. Calculate the initial volume of a gas. 9. Calculate ∆𝑈 at 298 K for the reaction 𝐶2𝐻4 + 𝐻𝐶𝑙→𝐶2𝐻5𝐶𝑙 ∆𝐻 =− 72. 3 𝑘𝐽 How much PV work is done ? 10. Calculate the amount of work done in the a) Oxidation of 1 mole of HCl at 200℃ according to the reaction. 4HCl + 𝑂2 ⟶ 2𝐶𝑙2 + 2𝐻2𝑂 b) Decomposition of one mole of NO at 300℃ for the reaction. 2NO ⟶ 𝑁2 + 𝑂2 11. Calculate the work done and comment whether the work is done on or by the system for the decomposition of 2 moles of 𝑁𝐻3𝑁𝑂3 at 100℃. 𝑁𝐻4𝑁𝑂⟶𝑁2𝑂 + 2𝐻2𝑂 12. Calculate the decomposition of 132 g of 𝑁𝐻3𝑁𝑂3 at 100℃. Same reaction as above. 13. Calculate the standard enthalpy 2𝐶2𝐻6 + 7𝑂2⟶4𝐶𝑂2 + 6𝐻2𝑂 0 −1 0 −1 Given that : ∆𝑓𝐻 (𝐶𝑂2) =− 393. 5 𝑘𝐽𝑚𝑜𝑙 , ∆𝑓𝐻 (𝐻2𝑂) =− 285. 8 𝑘𝐽𝑚𝑜𝑙 , 0 −1 ∆𝑓𝐻 (𝐶2𝐻6) =− 84. 9 𝑘𝐽𝑚𝑜𝑙 14. Calculate the standard enthalpy of reaction : 𝐹𝑒2𝑂3 + 3𝐶𝑂⟶2𝐹𝑒 + 3𝐶𝑂2 0 −1 0 −1 Given that : ∆𝑓𝐻 (𝐹𝑒2𝑂3) =− 824 𝑘𝐽𝑚𝑜𝑙 , ∆𝑓𝐻 (𝐶𝑂) =− 110 𝑘𝐽𝑚𝑜𝑙 , 0 −1 ( ) ∆𝑓𝐻 𝐶𝑂2 =− 393 𝑘𝐽𝑚𝑜𝑙  AK TUTORIALS Worksheet Subject: Chemistry ___________________________________________________________________________ ELECTROCHEMISTRY: 1. Difference between Electrolytes and Non-Electrolytes. 2. Define Molar conductivity. Give its Significance. 3. Explain Kohlrausch's Law of independent migration of ions with its Application. 4. Define cell constant State its SI unit. 5. Difference between Electrolytic and Galvanic cells. 6. Explain the Electrolysis of Molten NaCl. 7. Short note on Salt Bridge. 8. Define Electrode Potential and Cell Potential. 9. Derive Nernst Equation. 10. Obtain the relation between Gibbs Energy and cell Potential. 11. Define Reference Electrode. Short Note on SHE. 12. What are Primary and Secondary Voltaic Cells? 13. Define Electrochemical Series. State its Applications. 14. Explain different cells: i) Fuel cells ii) Dry cells iii) Lead Storage Battery 15. Explain the Mercury battery and NiCAD Storage Battery cell. Formulas: ° ° ° 1. 𝐸𝑐𝑒𝑙𝑙 = 𝐸𝑐𝑎𝑡ℎ𝑜𝑑𝑒 − 𝐸𝑎𝑛𝑜𝑑𝑒 ° 0.059 2. 𝐸 =𝐸 − 𝑛 log 𝑙𝑜𝑔 𝐾 ° 3. ∆𝐺 =− 𝑛𝐹𝐸𝑐𝑒𝑙𝑙 4. ∆𝐺 =− 2. 303 𝑅𝑇 log 𝑙𝑜𝑔 𝐾 ρ𝑙 1 𝑙 5. 𝑅= 𝐴 = 𝑘 𝐴 1 6. 𝐶𝑜𝑛𝑑𝑢𝑐𝑡𝑎𝑛𝑐𝑒 𝐺 = 𝑅 𝑙 7. 𝑘=𝐺 𝐴 1000𝑘 8. Λ= 𝐶 𝑙 9. Cell constant = 𝐴 𝐼 ×𝑡 10. 𝑊 = 96500 ×𝑚𝑜𝑙𝑒 𝑟𝑎𝑡𝑖𝑜 ×𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 Questions : 1. Calculate the resistance of 0.01 M solution of an electrolyte whose equivalent conductivity is 420 −1 2 −1 𝑜ℎ𝑚 𝑐𝑚 (cell constant of the cell is 0.88𝑐𝑚. −1 2. The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 S 𝑐𝑚.Calculate its molar conductivity.  −1 2 −1 3. The molar conductivity of 0.05 M 𝐵𝑎𝐶𝑙2 solution at 25℃ is 223 Ω 𝑐𝑚 𝑚𝑜𝑙.What is its conductivity? −3 −1 2 −1 4. The conductivity of 0.02 M 𝐴𝑔𝑁𝑂3 at 25℃ is 2.428 x 10 Ω 𝑐𝑚 𝑚𝑜𝑙.what is its molar conductivity? 5. Resistance and conductivity of a cell containing 0.001 M KCl solution at 298 K are 1500 −4 −1 Ω 𝑎𝑛𝑑 1. 46 𝑥 10 S 𝑐𝑚.What is cell constant? 6. A conductivity cell filled with 0.2 M 𝐻2𝑆𝑂4 gives at 25℃ a resistance of 122 ohms. If the molar −1 2 −1 conductivity of 0.02 M 618 Ω 𝑐𝑚 𝑚𝑜𝑙 , what is cell constant ? −5 −1 −1 7. Conductivity of a solution is 6.23 x 10 Ω 𝑐𝑚 and its resistance is 13710 ohms. If the electrodes are 0.7 cm apart calculate the cross sectional area of the electrode. 8. A conductivity cell is filled with 0.01 M KCl gives at 25℃the resistance of 604 ohms.The conductivity −1 −1 of KCl at 25℃ is 0.00141 Ω 𝑐𝑚. The same cell filled with 0.001 M 𝐴𝑔𝑁𝑂3 gives a resistance of 6529 ohms. Calculate the molar conductivity of 0.001 M 𝐴𝑔𝑁𝑂3 solution at 25℃. 9. The molar conductivities at zero concentration of 𝑁𝐻4𝐶𝑙 , 𝑁𝑎𝑂𝐻 𝑎𝑛𝑑 𝑁𝑎𝐶𝑙 𝑎𝑟𝑒 respectively 149.7 −1 2 −1 −1 2 −1 −1 2 −1 Ω 𝑐𝑚 𝑚𝑜𝑙 , 248 Ω 𝑐𝑚 𝑚𝑜𝑙 and 126.5 Ω 𝑐𝑚 𝑚𝑜𝑙. What is the molar conductivity of 𝑁𝐻4𝑂𝐻 at zero concentration? 10. What is the molar conductivity of AgI at zero concentration if the Λ0 values of NaI , 𝐴𝑔𝑁𝑂3 −1 2 −1 −1 2 −1 −1 and 𝑁𝑎𝑁𝑂3 are respectively 126.9 Ω 𝑐𝑚 𝑚𝑜𝑙 , 133.4 Ω 𝑐𝑚 𝑚𝑜𝑙 and 121.5 Ω 2 −1 𝑐𝑚 𝑚𝑜𝑙 ? 11. If a current of 0.5 A flows through a metallic wire of 2 hours , then how many electrons would flow through the wire ? 12. What is the mass of Cu metal produced at the cathode during the passage of 5 A current through 𝐶𝑢𝑆𝑂4 solution for 100 minutes ? Molar mass of Cu is 63.5 g/mol. 13. How many moles of electrons are passed when 0.8 A current is passed for 1 hour Through molten 𝐶𝑎𝐶𝑙2? 14. How long will it take to produce 2.415 g of Ag metal from its salt solution by passing a current of 3 amperes? Molar mass of Ag is 107.9 g/mol. 15. What current strength in amperes will be required to produce 2.4 g of Cu from 𝐶𝑢𝑆𝑂4 solution in 1 hour ? Molar mass of Cu is 63.5 g/mol? +2 16. How many moles of electrons are required for reduction of 3 moles of 𝑍𝑛 to Zn? How many Faradays of electricity will be required? +3 17. How many moles of electrons are required for reduction of 5 moles of 𝐶𝑟 to Cr ? How many Faradays of electricity will be required ? 18. What is the standard cell potential for the reaction? 3+ 2+ ° ° 3𝑁𝑖 + 2𝐴𝑙 →3𝑁𝑖 + 2𝐴𝑙 , 𝑖𝑓 𝐸𝑁𝑖 =− 0. 25𝑉 𝑎𝑛𝑑 𝐸𝐴𝑙 =− 1. 66 𝑉 ? 2+ 19. Given that 𝑀𝑛 𝑀𝑛 | || 𝐶𝑜3+|𝐶𝑜 𝐸°𝐶𝑜 = 1. 82𝑉 𝑎𝑛𝑑 𝐸°𝑀𝑛 =− 1. 18 𝑉 𝐶𝑎𝑙𝑐𝑢𝑙𝑎𝑡𝑒 𝐸°𝐶𝑒𝑙𝑙 20. Calculate the emf of the cell at 25℃ 2+ 3+ ° ° | || | 𝑍𝑛 𝑍𝑛 (0. 08𝑀) 𝐶𝑟 (0. 1 𝑀) 𝐶𝑟 𝐸𝑍𝑛 =− 0. 76 𝑉 𝑎𝑛𝑑 𝐸𝐶𝑟 =− 0. 74 𝑉 2+ 2+ 6 21. Equilibrium constant of the reaction , 2𝐶𝑢 → 𝐶𝑢 + 𝐶𝑢 𝑖𝑠 1. 2 ×10. What is the standard potential of the cell in which the reaction takes place ?  AK TUTORIALS Worksheet Subject: Chemistry ___________________________________________________________________________ COORDINATION COMPOUNDS: 1. What are ligands? What are their types? Give one example of each. 2. Define : a) Coordination sphere b) Complex ion c) Counter ion 3. Define Coordination number 4. What is the difference between a complex ion and double salt? Give one example. 5. Write the postulates of Werner theory of coordination complexes. 6. How are coordination complexes classified on the basis of types of ligands attached to central metal atoms or ions? 7. What are cationic anionic and neutral complexes? Give one example. 8. State and explain EAN Number. 9. What are isomers? Explain classification of isomers. 10. Explain the factors which affect the stability of coordination compounds. 11. Difference between strong and weak field ligands. 12. Explain the formation of octahedral complexes using CFT. 13. State the factors affecting CFT. 14. Write a note on colours in Coordination compounds. 15. Explain the formation of tetrahedral complexes using CFT. 16. Give the applications of coordination compounds. RECENTLY ASKED QUESTIONS: 1. Explain monodentate and ambidentate ligands with examples. 2. Write two postulates of Werner’s Theory. 3. Explain Homoleptic and Heteroleptic complexes with examples. 4. Define Destereoisomers. 5. Explain linkage isomerism in complexes with one example. 6. [ Explain the formation of 𝐶𝑜𝐹6 ]3− complex with respect to Hybridisation, Magnetic properties, Inner/outer complex and Geometry. 7. Write the name of the platinum complex used in the treatment of cancer.  AK TUTORIALS Worksheet Subject: Chemistry ___________________________________________________________________________ POLYMERS: 1. Explain the classification of polymers on the basis of : a) Source b) Chemical structure c) Mode of Polymerization d) Molecular forces e) Types of monomers f) Biodegradability 2. Define Polymerization. 3. Explain Natural Rubber and the Vulcanization of Rubber. 4. Explain Preparation properties and uses. a) HDPE and LDPE b) Polyacrylonitrile c) Nylon 6,6 d) Nylon 6 e) Terylene f) Bakelite g) Teflon h) Buna S i) PHVB 5. Explain the preparation of Neoprene and Vulcanisation of Neoprene. RECENTLY ASKED QUESTIONS: 1. Write the preparation of Terylene. 2. What is the name of the monomer used for the preparation of Nylon 6? 3. Write the chemical composition of the Zieglar-Natta catalyst. 4. Write chemical reaction for preparation of Teflon. 5. Write the reaction for the formation of nylon 6,6 polymer. 6. Define Vulcanization. 7. Define non-biodegradable polymer. 8. Write the name of the biodegradable polyamide copolymer.  AK TUTORIALS Worksheet Subject: Chemistry ___________________________________________________________________________ GREEN CHEMISTRY 1. Define a. Green Chemistry b. Nanochemistry c. Nanoscience d. Nanomaterials e. Nanotechnology f. Atom Economy 2. Explain less hazardous chemical synthesis with suitable example. 3. Explain the role of Green Chemistry. 4. What are the 12 principles of Green Chemistry? 5. Green chemistry plays an important role in sustainable development.Explain. 6. How are nanomaterials classified? 7. What are zero, one and two-dimensional nanoscale system? 8. What are the characteristic features of nanoparticles? 9. What are the different applications of nanomaterials? 10. Give the advantages and disadvantages of nanoparticles and nanotechnology. 11. Write the name of the technique used to know the geometry of nanoparticles. 12. Name the nanoparticles used in sunscreen. 13. Name the nanoparticles used in the purification of water. 14. Give the name of the wet chemical synthetic process for nanomaterials. 15. Name the nanoparticles used as catalysts in hydrogenation reaction. 16. What is the colour of gold nanoparticles? 17. Write the formula to calculate % atom economy. 18. Name the γ 𝑖𝑠𝑜𝑚𝑒𝑟 of BHC. 19. Which nanomaterial is used for the tyres of car to increase the life of tyres? 20. Which flower is an example of self-cleaning? 21. Give the full form of a. XRD - X-ray Diffraction b. TEM - Tunneling Electron Microscope c. STM - Scanning Tunneling Microscope d. FTIR - Fourier Transform Infrared Spectroscopy e. SEM - Scanning Electron Microscope  AK TUTORIALS Worksheet Subject: Chemistry ___________________________________________________________________________ HALOGEN DERIVATIVES OF ALKANES AND ARENES : 1. Give the structural formula and IUPAC name of isobutylbromide. 2. Write the structures of : a. 3-Chloro-3-ethylhex-1-ene b. 1-Iodo-2,3-dimethylbutane c. 1,3,5-Tribromobenzene 3. How is propene converted into 1-bromopropane and 2-bromopropane? 4. Convert ethyl bromide to: a. Ethyl iodide b. Ethyl fluoride 5. Explain optical activity of 2-chlorobutane. 6. Explain the term : Optical Activity. 7. Define Racemic mixture. 8. Define Enantiomers. 9. Define optical activity. 10. Write a note of Wurtz reaction. 11. What happens when following reagents react with ethyl iodide? a. Aqueous KOH b. Alcoholic KCN c. Silver Acetate 12. Difference between 𝑆𝑁 1 𝑎𝑛𝑑 𝑆𝑁 2 mechanisms. 13. Discuss the mechanism of alkaline hydrolysis of bromomethane. 14. Discuss the mechanism of alkaline hydrolysis of tert-bromomethane. 15. What is Grignard Reagent? How is it prepared? 16. How is chlorobenzene converted into diphenyl? 17. What is the action of the following on ethyl bromide a. Alc KOH b. Silver acetate 18. Write the product formed when alkyl halide reacts with silver nitrite. 19. What is the action of following on ethyl bromide: a. Na in dry ether b. Mg in dry ether 20. Write chemical reactions for the following conversions: a. ethyl bromide to ethyl methyl ether b. Ethyl bromide to ethene c. Bromobenzene to toluene d. Chlorobenzene to biphenyl 21. What is the structure of the product formed when chlorobenzene is treated with sodium metal in the presence of dry ether? 22. Explain the dehydrohalogenation reaction of 2-chlorobutane. 23. Write chemical reaction for the following : a. Chlorobenzene is heated with fuming 𝐻2𝑆𝑂4 b. Ethyl bromide is heated with silver acetate. 24. Draw the structure of DDT. Write its environmental effects. 25. Write use and environmental effect of CFC. 26. Complete the following : 𝑃𝐵𝑟3 𝑁𝐻3 𝐸𝑥𝑐𝑒𝑠𝑠 a. Isopropyl alcohol > A >B 𝐻𝐵𝑟 𝑎𝑙𝑐 𝐾𝑂𝐻 b. 𝐶𝐻3 − 𝐶𝐻 = 𝐶𝐻2 >A >B 𝑎𝑙𝑐 𝐾𝑂𝐻 𝐻𝐵𝑟 𝑁𝑎 c. 𝐶𝐻3 − 𝐶𝐻2 − 𝐶𝐻2 − 𝐶𝑙 ∆ > A >B 𝑑𝑟𝑦 𝑒𝑡ℎ𝑒𝑟 >C ℎν d. 𝐶𝐻4 + 𝐶𝑙2 >? 𝐻𝐶𝑙 e. 𝐶𝐻3 − 𝐶𝐻 = 𝐶𝐻2 > ? 𝐻𝐵𝑟 f. 𝐶𝐻3 − 𝐶𝐻 = 𝐶𝐻2 𝑝𝑒𝑟𝑜𝑥𝑖𝑑𝑒 > ? 𝐶𝐶𝑙2 g. 𝐶𝐻3 − 𝐶𝐻 = 𝐶𝐻2 + 𝐵𝑟2 > ? 27. Haloarenes are less reactive than Haloalalkanes. 28. What is chiral carbon?  AK TUTORIALS Worksheet Subject: Chemistry ___________________________________________________________________________ ALCOHOLS PHENOLS AND ETHER : 1. How will you prepare phenol from cumene? 2. How will you prepare phenol from Aniline? 3. How will you prepare phenol using Benzene Sulphuric acid? 4. What is Dow’s Process? 5. Short Note on Kolbe’s Synthesis. 6. Short Note on Reimer Tiemann Reaction. 7. How will you prepare Picric acid from phenol? 8. How will you prepare Aspirin using phenol? 9. How can we differentiate primary, secondary and tertiary alcohol using Cu? 10. Short Note on Esterification. 11. What are Phenols? 12. How is Benzoquinone prepared from phenol? 13. What happens when Phenol reacts with Zn? 14. Short Note on Williamson’s Synthesis 15. Explain why phenol is more acidic than ethyl alcohol. Previous Year Questions : 1. What are ethers? How are they classified? 2. Draw the structure of 2-methylpropan-2-ol. 3. Write the IUPAC name of the pyrogallol. 4. Write a chemical test to distinguish alcohol and Phenol. 5. From methyl magnesium iodide, how ethanol and propan-2-ol are prepared? 6. What is the action of conc 𝐻2𝑆𝑂4 on Phenol at 373 K? 7. How is ethanol prepared from methanal by using the Grignard reagent? 8. How is phenol converted into the following? a. Benzene b. Benzoquinone c. Picric acid 9. How is ethanol prepared from the following? a. Ethanal b. Ethene c. Bromoethane 10. Write a balanced chemical reaction of the following reagents on carbolic acid : a. 𝐵𝑟2 𝑤𝑎𝑡𝑒𝑟 b. Concentrated 𝐻𝑁𝑂3 𝑜 𝑜 11. What happens when vapours of 1 and 2 alcohols are passed over hot Cu metal? 12. Write the name of the reaction during the conversion of phenol to salicylic acid.  13. Convert Ethyl alcohol to Ethyl acetate. 14. What is the action of Bromine water on Phenol? 15. How is methoxybenzene prepared from phenol? 16. How is methoxy ethane prepared from methyl iodide? 17. What is the action of hot HI on isopropyl methyl ether? 18. Write chemical reactions of the following reagents on methoxy ethane: a. Hot HI b. 𝑃𝐶𝑙5 c. Dilute 𝐻2𝑆𝑂4. 19. Convert Diethyl ether into ethyl chloride. __________________________________________________________________________________