Table Of Content

I m B IB ^ ^ S ^ I I a b l i ^ a S e n al Problems in AND ALL OTHER ENGINEERING ENTRANCE EXAMINATIONS Problems in AND ALL OTHER ENGINEERING ENTRANCE EXAMINATIONS 1. GASEOUS STATE Chapter at a glance Basic Problems with Solution Selected Problems with Solution Problems for self assessment IIT-JEE Problems with Solution I 2. MOLE AND EQUIVALENT CONCEPT 61-146 • Chapter at a glance 61 • Basic Problems with Solution 63 Til Tiriaip ' PtR?!- • Selected Problems with Solution 96 • Problems for self assessment 130 • IIT-JEE Problems with Solution 135 H! l i' 3. ATOMIC STRUCTURE Chapter at a glance Basic Problems with Solution Selected Problems.with Solution Problems for self assessment IIT-JEE Problems with Solution « i j MI 4 1 1 L LI t i ll MS • "> ' 4. RADIOACTIVITY 203-247 | Chapter at a glance 203 Basic Problems with Solution 204 Selected Problems with Solution 215 Problems for self assessment 234 IIT-JEE Problems with Solution 237 I 6. REDOX TITRATIONS 273-338 I 1 • Chapter at a glance 273 • Basic Problems with Solution 274 KPB • Selected Problems with Solution 283 • Problems for self assessment 316 liP) . • IIT-JEE Problems with Solution 321 7. ELECTROCHEMISTRY 339-404 • Chapter at a glance 339 • Basic Problems with Solution 340 • Selected Problems with Solution 356 • Problems for self assessment 383 • IIT-JEE Problems with Solution 387 8. DILUTE SOLUTIONS AND COLLIGATIVE PROPERTIES 405-462 Chapter at a glance Basic Problems with Solution Selected Problems with Solution Problems for self assessment IIT-JEE Problems with Solution j i lt HI i ig 9. CHEMICAL KINETICS r " Chapter at a glance 463 i v, V Basic Problems with Solution 466 Selected Problems with Solution 487 V K " Problems for self assessment 507 % Ttm- IIT-JEE Problems with Solution 510 • Chapter at a glance • Basic Problems with Solution • Selected Problems with Solution • Problems for self assessment • IIT-JEE Problems with Solution 11. IONIC EQUILIBRIUM • Chapter at a glance • -Basic Problems with Solution 4 Selected Problems with Solution • Problems for self assessment • IIT-JEE Problems with Solution 12. THERMODYNAMICS 705-747 I wi It T pesi- • Chapter at a glance 705 F • Basic Problems with Solution 707 Ji- ~ - - • Selected Problems with Solution 714 9 • Problems for self assessment 735 • IIT-JEE Problems with Solution 742 13. THERMOCHEMISTRY Chapter at a glance Basic Problems with Solution Selected Problems with Solution Problems for self assessment IIT-JEE Problems with Solution 14. CRYSTALLOGRAPHY Chapter at a glance Basic Problems with Solution Selected Problems with Solution Problems for self assessment IIT-JEE Problems with Solution • Chapter at a glance • Basic Problems with Solution • Selected Problems with Solution • Problems for self assessment • Selected Problems with Solution • Problems for self assessment • IIT-JEE Problems with Solution • SOME IMPORTANT TABLES 865-872 • LOG TABLE 873-876 Gaseous State Chapter at a Glance 1. lioyles1 law: /'V = constant (at constant T and n) 2. ( limit's law: V/T = constant (at constant P and n) .1. (>ay Lussac-Charles's law: P/T - constant (at constant V and n) 4. Avogadro's hypothesis: V oc No. of molecules (at constant pressure and temperature) 5. (•as equalion: PV= nRT oi PV=(w/m)RT or P = ~RT (where <1 is density of gas) m (>. Graham's law of diffusion: ; n -W MI (at constant P and T) r ~ M\ 2 (at constant T) n y m i p 2 7. Dalton's law of partial pressure: PT = FA + P'B + P'c + and P\ = Pj x mole fraction of A 8. Absolute density: , mass . . . . .. -i a = — ; expressed usually in g litre volume 9. Vapour density: Molecular weight = Vapour density x 2 (For gases only) 10. Different speed terms for molecular motion: "AV = "V j^/ ' w^ere "AV 's average speed -x/3 RT where « is root mean square speed "rm.= V rms 2 RT "MP = V ; where m^p is most probable speed M "MP : "AV : "rms : : ' : 1.128 : 1.224 NUMERICAI I 'I lYSK ;AL CHEMIST HY 11. Kinetic equation: 2 PV = (l/3)m.n.u (m is mass of one molecule and n is number of molecule) ms 12. Kinetic energy: K.E./mol = |RT 3 RT 3 Average K.E. or K.E./molecule = - — = ~kT (k is Boltzman constant) 13. Van der Waals' Equation: [V-b)=RT (for 1 mole) v2 2 n a p + [V-nb] = nRT (for n mole) V2 a is van der Waals' constant for attraction ; b is van der Waals' constant for volume. Also b = 4-N-v 14. Boyle's temperature (7b): a Th = Rb 15. Critical constants T c 27 Rb' Pc = 21b Vc = 3 b r P and V are critical temperature, critical pressure and critical volume respectively. c> c c 16. Inversion temperature (7^): 2 a Ti Rb 17. Law of corresponding state: [3V- I] = 8r r r P, V and T are reduced pressure, reduced volume and reduced temperature respectively. r r t 18. Mean free path (X): (a is molecular diameter) P.d. = v 2< -tio1 2 N 19. Collision frequency (c.f.): c r ' = "rms 20. Speciflc heat and molar heat capacities: R Cp- Cv : ~ M c -C = R p v £E : = Y c "Cv v c and r are specific heat at constant pressure and constant volume respectively, p v C and C are molar heat capacities at constant P and V respectively. p v GASEOUS STATE 6 The Basic Problems with Solutions I'roblcm I. A vessel of 120 mL capacity contains a certain amount of gas at 35°C' and 1.2 bar pressure. The gas is transferred to another vessel of volume 180 mL at 35°C. What would be its pressure? > I'roblcm 2. What will be the minimum pressure required to compress 500 dm1 of air at 1 bar to 200 dm3 at 30°C? >• I'roblcm 3. A gas occupies 300 mL at 127°C and 730 mm pressure. What would be its volume at STP? > I'roblcm 4. Calculate the volume occupied by 7g CO at 27°C and 750 mm Hg. >• I'roblcm 5. Calculate the temperature of 4.0 moles of a gas occupying 5 dm at 3.32 bar. (R = 0.083 bar dm3 K"1 mol-1). >• I'roblcm 6. Calculate the weight of CH in a 9 dm3 cylinder at 16 bar and 27"(\ 4 (R = 0.083 bar dm3 K-1) I'roblcm 7. A desiccator of internal volume one litre containing N at 1 atm is 2 partially evacuated to final pressure of 78 mm of Hg, while T remains constant. What is the volume of gas at this stage? •J • I'roblcm 8. In a certain region of space, there are only 5 molecules per cm of an average. The temperature is 3 K. What is the average pressure of this gas. > Problem 9. Using the equation of state PV=nRT, show that at a given temperature density of a gas is proportional to gas pressure P. > Problem 10. Calculate the density of C0 at 100°C and 800 mm Hg pressure. 2 > Problem 11. At 0°C, the density of a gaseous oxide at 2 bar is same as that of nitrogen at 5 bar. What is the molecular mass of the oxide? > Problem 12. The density of helium is 0.1784 kg/m3 at STP. If a given mass of helium at STP is allowed to expand to 1.400 times of its initial volume by changing P and T, compute its resultant density. > Problem 13. Density of a gas is found to be 5.46 g/dm3 at 27°C at 2 bar pressure. What will be its density at STP? > Problem 14. Calculate the volume occupied by 8.8 g of C0 at 31.1 °C and 1 bar 2 pressure. R = 0.083 bar litre K_l mof1. > Problem 15. 2.9 g of a gas at 95°C occupied the same volume as 0.184 g of hydrogen at 17°C, at same pressure. What is the molar mass of the gas? « > Problem 16. Assuming the same pressure in each case, calculate the mass of hydrogen required to inflate a balloon to a certain volume Fat 100°C if 3.5 g helium is required to inflate the balloon to half the volume V at 25°C. >- I'roblcm 17. The densities of an unknown gas and 0 were find 0.2579 kg/m3 and 2 0.2749 kg/m3 at the same P and T. Calculate the mol. weight of unkown gas.