- \n
- Candidates are allowed additional 15 minutes for only reading the paper.<\/li>\n
- They must NOT start writing during this time.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n
- \n
- All questions are compulsory.<\/li>\n
- Question 1 is of 20 marks having four subparts, all of which are compulsory.<\/li>\n
- Question numbers 2 to 8 carry 2 marks each, with two questions having an internal choice.<\/li>\n
- Question numbers 9 to 15 carry 3 marks each, with two questions having an internal choice.<\/li>\n
- Question numbers 16 to 18 carry 5 marks each, with an internal choice.<\/li>\n
- All working, including rough work, should be done on the same sheet as, and adjacent to the rest of the answer.<\/li>\n
- The intended marks for questions or parts of questions are given in brackets [ ].<\/li>\n
- Balanced equations must be given wherever possible and diagrams where they are helpful.<\/li>\n
- When solving numerical problems, all essential working must be shown.<\/li>\n
- In working out problems, use the following data:<\/li>\n
- Gas constant R = 1.987 cal deg-1<\/sup> mol-1<\/sup> = 8.314 JK-1<\/sup> mol-1<\/sup> = 0.0821 dm3<\/sup> atm K-1<\/sup> mol-1<\/sup><\/li>\n
- 11 atm = 1 dm3<\/sup> atm = 101.3 J. 1 Faraday = 96500 coulombs.<\/li>\n
- Avogadro\u2019s number = 6.023 \u00d7 1023<\/sup>.<\/li>\n<\/ul>\n
Question 1.
\n(a) Fill in the blanks by choosing the appropriate word\/words from those given in the brackets: [4 \u00d7 1]
\n(square pyramidal, electrical, 74, 26, sp3<\/sup>d2<\/sup>, sp3<\/sup>d, chemical, 68, 32, tetrahedral, yellow, white, iodoform, Lucas)
\n(i) A Galvanic cell converts …….. energy into ………… energy.
\n(ii) The percentage of unoccupied spaces in bcc and fee arrangements are ……….. and …….. respectively.
\n(iii) Propan-2-ol on reaction with iodine and sodium hydroxide gives ……….. precipitate and the reaction is called ………. test.
\n(iv) The geometry of XeOF4<\/sub> molecule is ………… and the hybridisation of xenon atom in the molecule is<\/p>\n(b) Complete the following statements by selecting the correct alternative from the choices given: [4 \u00d7 1]
\n(i) During the course of an SN<\/sub>1 reaction, the intermediate species formed is:
\n(1) a carbocation
\n(2) a free radical
\n(3) a carbarn on
\n(4) an intermediate complex<\/p>\n(ii) Purification of aluminium by electrolytic refining is called:
\n(1) Speck’s process
\n(2) Hoppe’s process
\n(3) Hall\u2019s process
\n(4) Baeyer\u2019s process<\/p>\n(iii) An aqueous solution of urea freezes at -0.186\u00b0C, Kf<\/sub> for water = 1.86 K kg mol-1<\/sup>, Kb<\/sub> for water = 0.512 K kg mol-1<\/sup>. The boiling point of the urea solution will be:
\n(1) 373.065 K
\n(2) 373.186 K
\n(3) 373.512 K
\n(4) 373.0512 K<\/p>\n(iv) In the dehydration of alcohols to alkenes by heating with concentrated sulphuric acid, the initiation step is:
\n(1) formation of carbocation
\n(2) formation of an ester
\n(3) protonation of the alcohol molecule
\n(4) elimination of water<\/p>\n(c) Match the following: [4 \u00d7 1]<\/p>\n
\n\n
\n (i) Rate constant<\/td>\n (a) Dialysis<\/td>\n<\/tr>\n \n (ii) Biodegradable polymer<\/td>\n (b) Glycine<\/td>\n<\/tr>\n \n (iii) Zwitter ion<\/td>\n (c) Arrhenius equation<\/td>\n<\/tr>\n \n (iv) Purification of colloids<\/td>\n (d) PHBV<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n (d) Answer the following questions:
\n(i) (1) Why does the density of transition elements increase from Titanium to Copper? (at. no. Ti = 22, Cu = 29)
\n(2) Why is zinc not regarded as a transition element?
\n(at. no. Zn = 30)
\n(ii) Identify the compounds A, B, C and D.
\n\\(\\mathrm{CH}_{3} \\mathrm{CN} \\stackrel{\\mathrm{H}_{2} \\mathrm{O} \/ \\mathrm{H}^{+}}{\\longrightarrow} \\mathrm{A} \\stackrel{\\mathrm{NH}_{3}}{\\longrightarrow} \\mathrm{B} \\stackrel{\\text { heat }}{\\longrightarrow} \\mathrm{C} \\frac{\\mathrm{Br}_{2} \/ \\mathrm{KOH}}{\\mathrm{m}}>\\mathrm{D}\\)
\n(iii) Calculate the osmotic pressure of a solution prepared by dissolving 0.025g of K2<\/sub>SO4<\/sub> in 2.0 litres of water at 25\u00b0C assuming that K2<\/sub>SO4<\/sub> is completely dissociated, (mol. wt. of K2<\/sub>SO4<\/sub> = 174 g mol-1<\/sup>)
\n(iv) What type of isomerism is shown by the following coordination compounds:
\n[Pt Cl2<\/sub>\u00a0(NH3<\/sub>)4<\/sub>)] Br2<\/sub> and [Pt Br2<\/sub>(NH3<\/sub>)4<\/sub>] Cl2<\/sub>.
\nWrite their IUPAC names.
\nAnswer:
\n(a) (i) A Galvanic cell converts chemical energy into electrical energy.
\n(ii) The percentage of unoccupied spaces in bcc and fee arrangements are 32 and 74 respectively.
\n(iii) Propan-2-ol on reaction with iodine and sodium hydroxide gives yellow precipitate and the reaction is called iodoform test.
\n(iv) The geometry of XeOF4<\/sub> molecule is square pyramidal and the hybridisation of xenon atom in the molecule is sp3<\/sup>d2<\/sup>.<\/p>\n(b) (i) (1)
\n(ii) (2)
\n(iii) (4)
\n(iv) (3)<\/p>\n(c) (i) (c)
\n(ii) (d)
\n(iii) (b)
\n(iv) (a)<\/p>\n(d) (i) (1) This is due to increase in mass and decrease in size.
\n(2) This is because neither zinc atom nor its ion (Zn2+<\/sup>) has 1 to 9d-electrons in the (n -1) d-subshell.
\n(ii) A – CH3<\/sub>COOH (Acetic acid)
\nB – CH3<\/sub>COONH4<\/sub> (Ammonium acetate)
\nC – CH3<\/sub>CONH2<\/sub> (Acetamide)
\nD – CH3<\/sub>NH2<\/sub> (Methyl amine)
\n(iii) R = 00821 L – atm\/K\/mol
\nT = 273 + 25 = 298K
\nVan\u2019t Hoff factor, i = 3 (\u03b1 = 100%)
\nV = 2L
\nWB<\/sub> = 0.025 g
\nMB<\/sub> = 174
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-1.png\")
\n(iv) Ionisation isomerism.<\/p>\n\n\n
\n Complex<\/strong><\/td>\n IUPAC name<\/strong><\/td>\n<\/tr>\n \n [Pt Cl2<\/sub> (NH3<\/sub>)4<\/sub>] Br2
\n<\/sub>[Pt Br2<\/sub> (NH3<\/sub>)4<\/sub>] Cl2<\/sub><\/td>\ntetraammine dichlorido platinum (IV) bromide
\ntetraammine dibromidoplatinum (IV) chloride.<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\nQuestion 2. [2]
\n(a) (i) Write the rate law expression for the reaction A + B + C \u2192 D + E, if the order of the reaction is first, second and zero with respect to A, B and C, respectively.
\n(ii) How many times the rate of reaction will increase if the concentration of A, B and C are doubled in the equation given in (i) above?
\n(b) The rate of reaction becomes four times when the temperature changes from 293 K to 313 K. Calculate the energy of activation (Ea<\/sub>) of the reaction assuming that it does not change with temperature. (R = 8.314 J K-1<\/sup> mol-1<\/sup>)
\nAnswer:
\n(a) (i) Rate law expression is given as
\nr \u221d [A]1<\/sup> [B]2<\/sup>[C]\u00b0
\n\u221d [A]1<\/sup> [B]2<\/sup>
\nor r = [A]1<\/sup> [B]2<\/sup>
\n(ii) Conc of A, B, C is doubled. The rate of a reaction in the equation given in (i) above will become 8 (2 \u00d7 22<\/sup>) times.
\nOr
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-2.png\")
<\/p>\nQuestion 3. [2]
\n(a) How do antiseptics differ from disinfectants?
\n(b) State the role of the following chemicals in the food industry:
\n(i) Sodium benzoate
\n(ii) Aspartame
\nAnswer:
\n(a) Antiseptics: These are the chemical substances which prevent the growth of micro-organisms and may even kill them and are safe to be applied to living tissues. Examples: furacin, tobramycin etc.<\/p>\nDisinfectants: These are the chemical substances which kill micro-organisms but are not safe to be applied to living tissues but are used for non-living substances such as drains, toilet etc. For example 1% solution of phenol.<\/p>\n
(b) (i) Food preservative
\n(ii) Artificial sweetener<\/p>\nQuestion 4. [2]
\nAn aromatic organic compound [A] on heating with NH3<\/sub> and Cu2<\/sub>O at high pressure gives [B], The compound [B] on treatment with an ice-cold solution of NaNO2<\/sub> and HCl gives [C], which on heating with Cu\/HCl gives compound [A] again. Identify the compounds [A], [B] and [C]. Write the name of the reaction for the conversion of [B] to [C].
\nAnswer:
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-3.png\")
\nA – Chlorobenzene
\nB – Benzenamine or Aniline
\nC – Benzene diazonium chloride<\/p>\nQuestion 5. [2]
\nWrite the names of the monomers for each of the following polymers:
\n(a) Bakelite
\n(b) Nylon – 2 – Nylon – 6
\nAnswer:
\n(a) Bakelite
\nMonomers: Phenol and formaldehyde
\n(b) Nylon – 2 – Nylon – 6
\nGlycine and \u2208 – Amino Caproic acid<\/p>\nQuestion 6. [2]
\nName the purine bases and pyrimidine bases present in RNA and DNA.
\nAnswer:<\/p>\n\n\n
\n Nucleic acid<\/strong><\/td>\n Purine bases<\/strong><\/td>\n Pyrimidine bases<\/strong><\/td>\n<\/tr>\n \n RNA
\nDNA<\/td>\nAdenine, Guanine
\nAdenine, Guanine<\/td>\nUracil, Cytosine
\nThymine, Cytosine<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\nQuestion 7. [2]
\n(a) How will you obtain the following? (Give balanced equation.)
\n(i) Picric acid from phenol.
\n(ii) Ethyl chloride from diethyl ether.
\nOr
\n(b) How will you obtain the following? (Give balanced equation.)
\n(i) Anisole from phenol
\n(ii) Ethyl acetate from ethanol.
\nAnswer:
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-4.png\")
<\/p>\nQuestion 8. [2]
\n40% of a first-order reaction is completed in 50 minutes. How much time will it take for the completion of 80% of this reaction?
\nAnswer:
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-5.png\")
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-6.png\")
<\/p>\nQuestion 9. [3]
\n(a) The freezing point of a solution containing 5.85 g of NaCl in 100 g of water is -3.348\u00b0C. Calculate Van\u2019t Hoff factor \u2018i\u2019 for this solution. What will be the experimental molecular weight of NaCl? (Kf<\/sub> for water = 1.86 K kg mol-1<\/sup>, at. wt. Na = 23, Cl = 35.5)
\nOr
\n(b) An aqueous solution containing 12.48 g of barium chloride (BaCl2<\/sub>) is 1000g of water, boils at 100.0832\u00b0C. Calculate the degree of dissociation of barium chloride. (Kb<\/sub> for water = 0.52 K kg mol-1<\/sup>, at. wt. Ba = 137, Cl = 35.5)
\nAnswer:
\n(a) \u0394Tf<\/sub> = 3.348\u00b0C
\nWB<\/sub> = 5.85g
\nWA<\/sub> = 100g
\nKf<\/sub> = 1.86 K kg mol-1<\/sup>
\nObserved mol. mass of NaCl(MB<\/sub>)
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-7.png\")
\nObserved mol. mass of NaCl = 32.5 g mol-1<\/sup>
\nNormal mol. mass of NaCl = 23 + 35.5 = 58.5 g mol-1<\/sup>
\nVan\u2019t Hoff factor, i = \\(\\frac{58 \\cdot 5}{32 \\cdot 5}\\) = 1.8
\nOr
\nKb<\/sub> = 0.52 K kg mol-1<\/sup>
\nWB<\/sub> = 100 g = 0.01 kg
\n\u0394Tb<\/sub> = 100.0832 – 100 = 0.0832\u00b0C = 0.0832 K
\nMolality of BaCl2<\/sub>
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-8.png\")
\nMolality after dissociation = 5.99 \u00d7 10-2<\/sup>(1 + 2\u03b1)
\n\u0394Tb<\/sub> = Kb<\/sub> \u00d7 m
\n0.0832 = 0.52 \u00d7 5.99 \u00d7 10-2<\/sup> (1 + 2\u03b1)
\n0.0832 = 0.0312 + 0.0624\u03b1
\n\u03b1 = 0.833 = 83.3%<\/p>\nQuestion 10.
\nExamine the defective crystal given below and answer the question that follows: [3]
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-9.png\")
\nState if the above defect is stoichiometric or non-stoichiometric. How does this defect affect the density of the crystal? Also, write the term used for this type of defect.
\nAnswer:
\n(i) 1. Stoichiometric defect
\n2. Density decreases
\n3. Schottky defect<\/p>\nQuestion 11.
\nGive the reason for each of the following: [3]<\/p>\n- \n
- For ferric hydroxide sol, the coagulating power of phosphate ion is more than chloride ion.<\/li>\n
- Medicines are more effective in their colloidal form.<\/li>\n
- Gelatin is added to ice creams.<\/li>\n<\/ol>\n
Answer:<\/p>\n
- \n
- This is because \\(\\mathrm{PO}_{4}^{3-}\\) ion has more charge than Cl–<\/sup> ion.<\/li>\n
- Phosphate ion \\(\\mathrm{PO}_{4}^{3-}\\)<\/li>\n
- To stabilise ice creams.<\/li>\n<\/ol>\n
Question 12.
\n(a) For the complex ion [Fe(CN)6<\/sub>]3-<\/sup> state: [3]
\n(i) the type of hybridisation.
\n(ii) the magnetic behaviour.
\n(iii) the oxidation number of the central metal atom.
\n(b) Write the IUPAC name of [Co(en)2<\/sub>Cl2<\/sub>]+<\/sup> ion and draw the structures of its geometrical isomers.
\nAnswer:
\n(a) (i) d2<\/sup>sp3<\/sup>
\n(ii) Paramagnetic due to one unpaired electron
\n(iii) +3
\n(b) dichlorobis (ethylene diamine) cobalt (III) ion.
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-10.png\")
<\/p>\nQuestion 13.
\n(a) Explain why: [3]
\n(i) Mn2+<\/sup> is more stable than Fe2+<\/sup> towards oxidation to +3 state.
\n(At. no. of Mn = 25, Fe = 26)
\n(ii) Transition elements usually form coloured ions.
\n(iii) Zr and Hf exhibit similar properties.
\n(At. no. of Zr = 40, Hf = 72)
\nOr
\n(b) Complete and balance the following chemical equations:
\n(i) KMnO4<\/sub> + KI + H2<\/sub>SO4<\/sub> \u2192 ____ + ____ + ____ + _____
\n(ii) K2<\/sub>Cr2<\/sub>O7<\/sub> + H2<\/sub>SO4<\/sub> + H2<\/sub>S \u2192 ____ + _____ + _____ + ____
\n(iii) KMnO4<\/sub> + H2<\/sub>SO4<\/sub> + FeSO4<\/sub> \u2192 _____ + _____ + _____ + ____
\nAnswer:
\n(a) (i) This is because Mn2+<\/sup>(3d5<\/sup>) has extra stable electronic configuration but Fe2+<\/sup>(3d6<\/sup>) does not.
\n(ii) This is due to the presence of impaired electrons in their (n-1) d – orbitals.
\n(iii) This is due to lanthanide contraction or ineffective shielding but intervening 4f- electrons in Hf.
\nOr
\n(b) (i) 2KMnO4<\/sub> + 10KI + 8H2<\/sub>SO4<\/sub> \u2192 6K2<\/sub>SO4<\/sub> + 2MnSO4<\/sub> + 8H2<\/sub>O + 5I2<\/sub>
\n(ii) K2<\/sub>Cr2<\/sub>O7<\/sub> + 4H2<\/sub>SO4<\/sub> + 3H2<\/sub>S \u2192 K2<\/sub>SO4<\/sub> + Cr2<\/sub>(SO4<\/sub>)3<\/sub> + 7H2<\/sub>O + 3S
\n(iii) 2KMnO4<\/sub> + 8H2<\/sub>SO4<\/sub> + 10FeSO4<\/sub> \u2192 K2<\/sub>SO4<\/sub> + 2MnSO4<\/sub> + 5Fe2<\/sub>(SO4<\/sub>)3<\/sub> + 8H2<\/sub>O<\/p>\nQuestion 14.
\n(a) Arrange the following in the increasing order of their basic strength: [3]
\nC2<\/sub>H5<\/sub>NH2<\/sub>, C6<\/sub>H5<\/sub>NH2<\/sub>, (C2<\/sub>H5<\/sub>)2<\/sub>NH
\n(b) Give a balanced chemical equation to convert methyl cyanide to ethyl alcohol.
\n(c) What happens when benzene diazonium chloride reacts with phenol in weak alkaline medium? (Give balanced equation).
\nAnswer:
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-11.png\")
<\/p>\nQuestion 15.
\nName the sulphide ore of Copper. Describe how pure copper is extracted from this ore. [3]
\nAnswer:
\nThe sulphide ore of copper is copper pyrite (CuFeS2<\/sub>). The extraction of pine copper from copper pyrite ore involves the following steps.
\n1. Crushing and grinding
\n2. Concentration by the froth-floatation process to remove gangue particles.
\n3. Roasting in the presence of free supply of air or O2<\/sub> during roasting the reactions taking place are
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-12.png\")
\nThe roasted ore mainly contains a number of Cu2<\/sub>S, FeS and FeO.<\/p>\n4. Smelting: The roasted ore is mixed with powdered coke and sand and is heated strongly in a blast furnace.
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-13.png\")
\nThe mixture thus obtained contains Cu2<\/sub>S and some FeS. It is called the molten matte.<\/p>\n5. Bessemerisation: In Bessemer converter, a hot blast of air mixed with sand is blown through molten matte. The reactions taking place are:
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-14.png\")
\nOn cooling molten copper, we get blister copper.<\/p>\n6. Refining of Copper: The copper obtained above is refined by poling and then by electrolyte refining containing acidified copper sulphate solution as an electrolyte.<\/p>\n
Question 16.
\n(a) (i) Calculate the emf and \u0394G\u00b0 for the cell reaction at 25\u00b0C: [5]
\n\\(\\begin{array}{cl}{\\mathrm{Zn}(s) | \\mathrm{Zn}_{(a q)}^{2+} \\|} & {\\mathrm{Cd}_{(a q)}^{2+} | \\mathrm{Cd}_{(s)}} \\\\ {(0 \\cdot 1 \\mathrm{M})} & {(0 \\cdot 01 \\mathrm{M})}\\end{array}\\)
\nGiven E\u00b0 Zn2+<\/sup>\/Zn = – 0-763 and E\u00b0Cd2+<\/sup>\/Cd = -0.403
\n(ii) Define the following terms:
\n(1) Equivalent conductivity
\n(2) Corrosion of metals
\nOr
\n(b) (i) The specific conductivity of a solution containing 5 g of an hydrous BaCl2<\/sub> (mol. wt. = 208) in 1000 cm3<\/sup> of a solution is found to be 0.0058 ohm-1<\/sup> cm-1<\/sup>. Calculate the molar and equivalent conductivity of the solution.
\n(ii) What is an electrochemical series? How is it useful in predicting whether a metal can liberate hydrogen from acid or not?
\nAnswer:
\n(a) (i) The given electrochemical cell is
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-15.png\")
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-16.png\")
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-17.png\")
\n(ii) (1) Equivalent Conductivity: It is the conducting power of all the ions present in a solution containing one gram equivalent of the electrolyte.
\n(2) Corrosion of Metals: It is the process involving the conversion of the metal surface into undesirable compounds on exposure to atmospheric conditions i.e. moisture and air. It is also called weeping of metals.
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-18.png\")
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-19.png\")
\n(ii) It is a series or table in which the various electrodes are arranged in the increasing order of standard reduction potential values. With the help of the electrochemical series, we can predict whether a given metal can liberate hydrogen from acid or not. The metals which lie above hydrogen in the electrochemical series i.e. having negative standard reduction potential values can liberate hydrogen from dilute acids whereas metals which lie below hydrogen in the electrochemical series i.e., have positive standard reduction potential values cannot liberate hydrogen from dilute acids.<\/p>\nQuestion 17.
\n(a) (i) Explain why: [5]
\n(1) Nitrogen does not form pentahalides.
\n(2) Helium is used for filling weather balloons.
\n(3) ICl is more reactive than I2<\/sub>.
\n(ii) Draw the structures of the following:
\n(1) HClO4<\/sub>
\n(2) H3<\/sub>PO3<\/sub>
\nOr
\n(b) (i) Explain why:
\n(1) Mercury loses its meniscus in contact with ozone.
\n(2) Halogens are coloured and the colour deepens on moving down in the group from fluorine to iodine.
\n(3) Hydride of sulphur is a gas while hydride of oxygen is a liquid.
\n(ii) Complete and balance the following reactions:
\n(1) NaCl + MnO2<\/sub> + H2<\/sub>SO4<\/sub> \u2192 _____ + _____ + ______ + _____
\n(2) KMnO4<\/sub> + SO2<\/sub> + H2<\/sub>O \u2192 _____ + ______ + ______ + ______
\nAnswer:
\n(a) (i) (1) Nitrogen does not form pentahalides because it has no vacant d-orbitals in its valence shell.
\n(2) This is because it is lighter than air.
\n(3) This is because ICl is polar and has lower bond energy than I2<\/sub> (non-polar)
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-20.png\")
\n(b) (i) (1) This is due to the formation of mercurous oxide (Hg2<\/sub>O) which dissolves in mercury.
\n(2) This is because halogen molecules (X2<\/sub>) absorb light in the visible region and transmit complementary colour. This is because on moving from fluorine to iodine ionisation enthalpy decreases.
\n(3) This is because in H2<\/sub>S there are weak Van der Waals forces of attraction but in H2<\/sub>O there are strong intermolecular H-bonds.
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-21.png\")
<\/p>\nQuestion 18.
\n(a) (i) Give balanced equations for the following reactions: [5]
\n(1) Benzaldehyde reacts with hydrazine.
\n(2) Acetic acid reacts with phosphorous pentachloride.
\n(3) Acetone reacts with sodium bisulphite.
\n(ii) Give one chemical test each to distinguish between the following pairs of compounds:
\n(1) Ethanol and acetic acid
\n(2) Acetaldehyde and benzaldehyde
\nOr
\n(b) (i) Write chemical equations to illustrate the following name reactions:
\n(1) Clemmensen\u2019s reduction
\n(2) Rosenmund\u2019s reduction
\n(3) HVZ reaction
\n(iii) Explain why:
\n(1) Acetaldehyde undergoes aldol condensation but formaldehyde does not.
\n(2) Acetic acid is a weaker acid as compared to formic acid.
\nAnswer:
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-22.png\")
\n![\"ISC](\"https:\/\/cbselibrary.com\/wp-content\/uploads\/2020\/12\/ISC-Chemistry-Question-Paper-2018-Solved-for-Class-12-image-23.png\")
<\/p>\nISC Class 12 Chemistry Previous Year Question Papers<\/a><\/h4>\n","protected":false},"excerpt":{"rendered":"
- This is because \\(\\mathrm{PO}_{4}^{3-}\\) ion has more charge than Cl–<\/sup> ion.<\/li>\n
- 11 atm = 1 dm3<\/sup> atm = 101.3 J. 1 Faraday = 96500 coulombs.<\/li>\n