{"id":6599,"date":"2024-02-28T05:34:56","date_gmt":"2024-02-28T00:04:56","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=6599"},"modified":"2024-02-28T14:40:30","modified_gmt":"2024-02-28T09:10:30","slug":"icse-previous-papers-solutions-class-10-chemistry-2008","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/icse-previous-papers-solutions-class-10-chemistry-2008\/","title":{"rendered":"ICSE Chemistry Question Paper 2008 Solved for Class 10"},"content":{"rendered":"
(Two Hours)<\/strong><\/em> SECTION-I \u00a0(40 Marks)<\/span><\/strong> Question 1:<\/strong> ** Answer has not given due to out of present syllabus.<\/p>\n (b)<\/strong> The equation for the burning of octane is: (c)<\/strong> Name<\/strong> the organic compound prepared by each of the following reactions:<\/p>\n (d)<\/strong> Identify the following substances:<\/p>\n (e)<\/strong> Write the equation for the following reactions: (f)\u00a0<\/strong>Here is an electrode reaction:<\/p>\n (g)<\/strong>\u00a0What are the terms defined in (g) (1) – (5) below?<\/p>\n Answer:<\/strong> (b)\u00a0<\/strong> (c)<\/strong><\/p>\n (d)<\/strong><\/p>\n (f) <\/strong><\/p>\n (g)<\/strong><\/p>\n SECTION-II \u00a0(40 Marks)<\/strong><\/span> Question 2:<\/strong> Answer:<\/strong> Question 3:<\/strong> (b)<\/strong> Supply the missing word from those in the brackets (Do not write out the sentence).<\/p>\n (c)<\/strong><\/p>\n Answer:<\/strong> (b)<\/strong><\/p>\n (c)<\/strong><\/p>\n Question 4:<\/strong> (d)<\/strong><\/p>\n Answer:<\/strong> (c)<\/strong><\/p>\n (d)<\/strong><\/p>\n Question 5:<\/strong> (b)<\/strong> From the equation Answer:<\/strong> Empirical formula = CHCl2<\/sub> (b)<\/strong> Question 6:<\/strong> (b)<\/strong> Making use only of substances chosen from those given below: Answer:<\/strong> Question 7:<\/strong> (b)<\/strong> Write the equations for the following reactions: Answer:<\/strong>
\nAnswers to this Paper must be written on the paper provided separately.<\/em>
\nYou will not<\/strong> be allowed to write during the first 15<\/strong> minutes.<\/em>
\nThis time is to be spent in reading the Question Paper.<\/em>
\nThe time given at the head of this Paper is the time allowed for writing the answers.<\/em>
\nSection I<\/strong> is compulsory. Attempt any four<\/strong> questions from Section II<\/strong>.<\/em>
\nThe intended marks for questions or parts of questions are given in brackets [ ].<\/em><\/p>\n
\n(Attempt all<\/strong> questions from this Section)<\/em><\/p>\n
\n(a)\u00a0<\/strong>For part (a) (1) – (a) (10), select the correct answer from the choices A, B, C, D which are given. Write down only the letter corresponding to the correct answer. \u00a0 \u00a0 \u00a0 \u00a0 [10]<\/strong><\/p>\n\n
\n(A) Atomic size increases from left to right across a period.
\n(B) Ionization potential increases from left to right across a period.
\n(C) Electron affinity increases going down a group.
\n(D) Electro-negativity increases going down a group.<\/li>\n
\n(A) High melting point.
\n(B) Conducts electricity when molten.
\n(C) Consists of oppositely charged ions.
\n(D) Ionizes when dissolved in water.<\/li>\n
\n(A) Copper nitrate \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 (B) Zinc nitrate
\n(C) Lead nitrate \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 (D) Sodium nitrate<\/li>\n
\n(A) Iron (III) sulphate \u00a0 \u00a0 \u00a0 \u00a0 (B) Iron (II) sulphate
\n(C) Iron (II) chloride \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 (D) Iron (III) chloride<\/li>\n
\n(A) Avogadro\u2019s Law \u00a0 \u00a0 \u00a0 \u00a0 \u00a0(B) Gay-Lussac\u2019s Law
\n(C) Boyle\u2019s Law \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 (D) Charles\u2019Law<\/li>\n
\n(A) Bromine is released at the cathode
\n(B) Lead is deposited at the anode
\n(C) Bromine ions gain electrons
\n(D) Lead is deposited at the cathode<\/li>\n
\n(A) Copper and tin \u00a0 \u00a0 \u00a0 \u00a0(B) Copper and zinc
\n(C) Zinc and lead \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 (D) Lead and tin<\/li>\n
\n(A) Ammonium chloride \u00a0 \u00a0 \u00a0(B) Ammonium nitrate
\n(C) Magnesium nitrade \u00a0 \u00a0 \u00a0 \u00a0 (D) Magnesium nitrate<\/li>\n
\n(A) Adding concentrated sulphuric acid to a chloride.
\n(B) Passing sulphur dioxide through a solution of chlorine.
\n(C) Reacting dry sulphur dioxide and dry chlorine.
\n(D) Beading dilute sulphuric acid with a solution of chlorine.<\/li>\n
\n(A) Substitution \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0(B) Dehydration
\n(C) Dehydrohalogenation \u00a0 \u00a0 (D) Addition<\/li>\n<\/ol>\n
\n2C8<\/sub>H18\u00a0<\/sub>+ 25O2 \u00a0 \u00a0<\/sub>\u2192 \u00a0 \u00a016CO2<\/sub> + 18H2<\/sub>O
\n(i) How many moles of carbon dioxide are produced when one<\/strong> mole of octane barns?
\n(ii) What volume, at sip, is occupied by the number of moles determined in (b) (i) ?
\n(iii) If the relative molecular mass of carbon dioxide is 44, what is the mass of carbon dioxide produced by burning two<\/strong> moles of octane?
\n(iv) What is the empirical formula of octane? [5]<\/strong><\/p>\n\n
\n
\n** Answer has not given due to out of present syllabus.<\/li>\n<\/ol>\n
\n(i) Aluminium nitride and water.
\n(ii) Calcium carbide and water.
\n(iii) Ethene and water (steam).
\n(iv) Sulphur dioxide and water. **
\n(v) Bromoethane and an aqueous solution of sodium hydroxide. [5]<\/strong><\/p>\n\n
\nAt which electrode (anode or cathode) would such a reaction take place? Is this an example of oxidation or reduction?<\/li>\n\n
\n(a) <\/strong><\/p>\n\n
\n<\/p>\n\n
\n
\n<\/p>\n\n
\nCu++<\/sup> + 2e–<\/sup>\u00a0 \u00a0 \u2192 \u00a0 \u00a0Cu (at cathode).<\/li>\n\n
\n(Answer any four<\/strong> questions from this section)<\/em><\/p>\n
\nCopy and complete the following table relating to important industrial processes. Output refers to the product of the process not the intermediate steps.
\n<\/p>\n
\n<\/p>\n
\nThe following questions refer to the Periodic Table:
\n(a)<\/strong><\/p>\n\n
\n
\n
\n(a)<\/strong><\/p>\n\n
\nLast element \u2014 Neon<\/li>\n\n
\n
\n(a)<\/strong> Distinguish between the saturated hydrocarbon ethane and the unsaturated hydrocarbon ethene by drawing their structural formulae. [2]<\/strong>
\n(b)<\/strong> Addition reactions and substitution reactions are types of organic reactions. Which type of reaction is shown by:
\n(1) ethane (2) ethene [2]<\/strong>
\n(c) <\/strong><\/p>\n\n
\n
\n(a) Saturated hydrocarbon:<\/strong> Ethane has single covalent bond between carbon atoms.
\nUnsaturated hydrocarbon:<\/strong> Ethene has a double covalent bond between carbon atoms.
\n
\n(b)<\/strong><\/p>\n\n
\n
\n
\n(a) <\/strong>(i) A compound has the, following percentage composition by mass:
\ncarbon 14.4%, hydrogen 1.2% and chlorine 84.5%. Determine the empirical formula of this compound. Work correct to 1 decimal place. (H = 1; C = 12; Cl = 35.5).
\n(ii) The relative molecular mass of this compound 168, so what is its molecular formula?
\n(iii) By what type reaction could this compound be obtained from ethyne? [6]<\/strong><\/p>\n
\nC + 2H2<\/sub>SO4 \u00a0\u00a0<\/sub> \u2192 \u00a0 \u00a0CO2<\/sub> + 2H2<\/sub>O + 2SO2<\/sub>
\nCalculate:
\n(i) The mass of carbon oxidized by 49 g of sulphuric acid (C = 12; relative molecular mass of sulphuric acid = 98).
\n(ii) The volume of sulphur dioxide measured at stp. liberated at the same time.
\n(Volume occupied by 1 mole of a gas at stp is 22.4 dm3<\/sup>)<\/p>\n
\n(a) <\/strong>(i)<\/p>\n\n\n
\n Element<\/strong><\/td>\n Percentage<\/strong><\/td>\n At. Mass<\/strong><\/td>\n Relative No.of atoms<\/strong><\/td>\n Simplest ratio<\/strong><\/td>\n<\/tr>\n \n C<\/td>\n 14.4<\/td>\n 12<\/td>\n 14.4\/12 = 1.2<\/td>\n 1.2\/1.2 = 1<\/td>\n<\/tr>\n \n H<\/td>\n 1.2<\/td>\n 1<\/td>\n 1.2\/1 = 1.2<\/td>\n 1.2\/1.2 = 1<\/td>\n<\/tr>\n \n Cl<\/td>\n 84.5<\/td>\n 35.5<\/td>\n 84.5\/35.5 = 2.4<\/td>\n 2.4\/1.2 = 2<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n
\n(ii) Relative molecular mass = 168
\nEmpirical formula mass = 12 + 1 + 71 = 84
\n\\(n=\\frac{\\text{Relative molecular mass}}{\\text{empirical formula mass }}=\\frac{168}{84}=2\\)
\nMolecular formula = (Empirical formula)n<\/sub>
\n= (CHCl2<\/sub>)2<\/sub>
\n= C2<\/sub>H2<\/sub>Cl4<\/sub>.
\n(iii) By addition reaction.<\/p>\n
\n
\n<\/p>\n
\n(a) The following is a sketch of an electrolytic cell used in the extraction of aluminium:
\n<\/p>\n\n
\nDilute sulphuric acid \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 sodium carbonate
\nZinc \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 sodium sulphite
\nLead \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0calcium carbonate
\ngive the equations for the reactions by which you could obtain:
\n(i) hydrogen
\n(ii) sulphur dioxide **
\n(iii) carbon dioxide
\n(iv) zinc carbonate (two steps required)<\/p>\n
\n (a)<\/strong><\/p>\n\n
\n<\/strong>
\n<\/p>\n
\n(a)<\/strong><\/p>\n\n
\n(i) Dilute nitric acid and copper.
\n(ii) Dilute sulphuric acid and barium chloride.
\n(iii) Dilute hydrochloric acid and sodium thiosulphate.
\n(iv) Dilute hydrochloric acid and lead nitrate solution.
\n(v) Dilute sulphuric acid and sodium sulphide. [5]<\/strong><\/p>\n
\n(a)<\/strong><\/p>\n