{"id":6805,"date":"2019-12-29T09:43:40","date_gmt":"2019-12-29T04:13:40","guid":{"rendered":"https:\/\/versionweekly.com\/?p=6805"},"modified":"2019-12-29T09:43:40","modified_gmt":"2019-12-29T04:13:40","slug":"icse-chemistry-question-paper-2019-solved-for-class-10-pdf-download","status":"publish","type":"post","link":"https:\/\/versionweekly.com\/news\/icse\/icse-chemistry-question-paper-2019-solved-for-class-10-pdf-download\/","title":{"rendered":"ICSE Chemistry Question Paper 2019 Solved for Class 10 PDF Download"},"content":{"rendered":"
Section -1 [40 Marks]<\/strong> Question 1. (ii) The most electronegative element from the following elements is : (iii) The reason for using Aluminium in the alloy duralumin is: (iv) The drying agent used to dry HCl gas is : (v) A hydrocarbon which is a greenhouse gas is : (b) Fill in the blanks with the choices given in brackets: [5]<\/strong> (ii) When sodium chloride is heated with concentrated sulphuric acid below 200\u00b0C, one of the products formed is ……………… (iii) Ammonia reacts with excess chlorine to form ……………….. (iv) Substitution reactions are characteristic reactions of …………….. (v) In Period 3, the most metallic element is …………….. (c) Write a balanced chemical equation for each of the following reactions: [5]<\/strong> (ii) Action of dilute sulphuric acid on sodium hydroxide. (iii) Action of dilute sulphuric acid on zinc sulphide. (iv) Ammonium hydroxide is added to ferrous sulphate solution. (v) Chlorine gas is reacted with ethene. (d) State one observation for each of the following: [5]<\/strong> (ii) Ammonia gas is passed over heated copper (II) oxide. (iii) Copper sulphate solution is electrolysed using copper electrodes. (iv) A small piece of zinc is added to dilute hydrochloric acid. (v) Lead nitrate is heated strongly in a test tube. (e) (i) Calculate: [5]<\/strong> 2. 6.022 x 1023<\/sup> atoms of carbon weigh \u2192 12 g (ii) Molecular formula of a compound is C6<\/sub>H18<\/sub>O3<\/sub>. Find its empirical formula. (f) (i) Give the IUPAC name of the following organic compounds: [5]<\/strong> (ii) What is the special feature of the structure of ethyne ? (iii) Name the saturated hydrocarbon containing two carbon atoms. (iv) Give the structural formula of Acetic acid. (g) Give the appropriate term defined by the statements given below: [5]<\/strong> (ii) The substance that releases hydronium ion as the only positive ion when dissolved in water. (iii) The tendency of an atom to attract electrons totvards itself when combined in a covalent compound. (iv) The process by which certain ores, specially carbonates, are converted to oxides in the absence of air. (v) The covalent bond in-which the electrons are shared equally between the combining atoms. (h) Arrange the following according to the instructions given in brackets : [5]<\/strong> (ii) Mg2+<\/sup>, Cu2+<\/sup>, Na1+<\/sup>, H1+<\/sup> (In the order of preferential discharge at the cathode) (iii) Li, K, Na, H (In the decreasing order of their ionization potential) (iv) F, B, N, O (In the increasing order of electron affinity) (v) Ethane, methane, ethene, ethyne. (In the increasing order of the molecular weight) Section – II [40 Marks]<\/strong> Question 2. (ii) Sodium chloride [Na = 11, Cl = 17] (iii) Ammonium ion [N = 7, H = 1] Formation of proton (b) The pH values of three solutions A, B and C are given in the table. Answer the following questions: [3]<\/strong> (c) Study the extract of the Periodic Table given below and answer the questions that follow. Give the alphabet corresponding to the element in question. DO NOT repeat an element. [4]<\/strong> Question 3. (b) Distinguish between the following pairs of compounds using the reagent given in the bracket. [3]<\/strong> (ii) Ferrous sulphate solution-and ferric sulphate solution, (using sodium hydroxide solution) Question 4. (b) Write a balanced chemical equation for the preparation of: [3]<\/strong> (ii) Ethyne using calcium carbide (iii) Methane from sodium acetate. (c) Name the following organic compounds : [4]<\/strong> Question 5. (b) Answer the following questions based on the extraction of aluminium from alumina by Hall – Heroult\u2019s Process: [3]<\/strong> (c) Match the alloys given in column I to the uses given in column II: Question 6. (b) Copper sulphate solution reacts with sodium hydroxide solution to form a precipitate of copper hydroxide according to the equation : [3]<\/strong> (ii) What is the colour of the precipitate formed ? (c) Find the empirical formula and the molecular formula of an organic compound from the data given below: Question 7. (b) Study the flow chart given and give balanced equations to represent the reactions A, B and C. (c) Copy and complete the following table which refers to the industrial method for the preparation of ammonia and sulphuric acid : [4]<\/strong> ICSE Chemistry Previous Year Question Paper 2019 Solved for Class 10 Answers to this Paper must be written on the … <\/p>\n
\n(Attempt all questions from this Section)<\/p>\n
\n(a) Choose the correct answer from the options given below: [5]<\/strong>
\n(i) An electrolyte which completely dissociates into ions is :
\n(A) Alcohol
\n(B) Carbonic acid
\n(C) Sucrose
\n(D) Sodium hydroxide
\nAnswer:
\n(D) Sodium hydroxide<\/p>\n
\n(A) Magnesium
\n(B) Chlorine
\n(C) Aluminium
\n(D) Sulphur
\nAnswer:
\n(B) Chlorine<\/p>\n
\n(A) Aluminium is brittle
\n(B) Aluminium gives strength
\n(C) Aluminium brings lightness
\n(D) Aluminium lowers melting point
\nAnswer:
\n(C) Aluminium brings lightness<\/p>\n
\n(A) Cone. H2<\/sub>SO4<\/sub>
\n(B) ZnO
\n(C) Al2<\/sub>O3<\/sub>
\n(D) CaO
\nAnswer:
\n(A) Cone. H2<\/sub>SO4<\/sub><\/p>\n
\n(A) Acetylene
\n(B) Ethylene
\n(C) Ethane
\n(D) Methane
\nAnswer:
\n(D) Methane<\/p>\n
\n(i) Conversion of ethanol to ethene by the action of concentrated sulphuric acid is an example of ……………..
\n(dehydration \/ dehydrogenation \/ dehydrohalogenation)
\nAnswer:
\ndehydration<\/p>\n
\n(sodium hydrogen sulphate \/ sodium sulphate \/ chlorine)
\nAnswer:
\nsodium hydrogen sulphate<\/p>\n
\n(nitrogen \/ nitrogen trichloride \/ ammonium chloride)
\nAnswer:
\nnitrogen trichioride<\/p>\n
\n(alkynes \/ alkenes \/ alkanes)
\nAnswer:
\nalkanes<\/p>\n
\n(sodium \/ magnesium \/ aluminium)
\nAnswer:
\nsodium<\/p>\n
\n(i) Reduction of copper (II) oxide by hydrogen.
\nAnswer:
\nCuO+H2\u00a0<\/sub>\u2192 Cu+H2<\/sub>O<\/p>\n
\nAnswer:
\n2NaOH + H2<\/sub>S04<\/sub> \u2192 Na2<\/sub>SO4<\/sub> + 2H2<\/sub>O<\/p>\n
\nAnswer:
\nZnS + H2<\/sub>SO4<\/sub> \u2192 ZnSO4<\/sub> + H2<\/sub>S<\/p>\n
\nAnswer:
\nFeSO4<\/sub> + 2NH4<\/sub>0H \u2192 (NH4<\/sub>)SO4<\/sub> + Fe(OH)2<\/sub>\u2193<\/p>\n
\nAnswer:
\n<\/p>\n
\n(i) Concentrated nitric acid is reacted with sulphur.
\nAnswer:
\n
\nDense brown fumes of nitrogen dioxide gas will be released<\/p>\n
\nAnswer:
\n
\nThe black colour copper oxide will change to reddish pink copper.<\/p>\n
\nAnswer:
\nWhen copper sulphate solution is electrolysed using copper electrodes, reddish pink deposit of copper metal takes place on cathode.<\/p>\n
\nAnswer:
\nZn + 2HCl > ZnCl2<\/sub> + H2<\/sub>\u2191
\nZinc metal dissolves forming solution with the liberation of hydrogen gas which bums with blue flame and gets extinguished with pop sound.<\/p>\n
\nAnswer:
\n
\nWhite powder of lead nitrate decompose to form yellow coloured lead oxide and liberating dense brown fumes of nitrogen dioxide gas.<\/p>\n
\n1. The number of moles in 12 g of oxygen gas. [O = 16]
\n2. The weight of 1022 atoms of carbon.
\n[C = 12, Avogadro\u2019s No. = 6 \u00d7 1023<\/sup>]
\nAnswer:
\n1. Oxygen gas (O2<\/sub>)
\nMolecular mass = 16 x 2 = 32 g
\n32 g of oxygen gas \u2192 1 mole
\n1 g of oxygen gas \u2192 [latex]\\frac { 1 }{ 32 }[\/latex] mole
\n12 g of oxygen gas \u2192 [latex]\\frac { 1 }{ 32 }[\/latex] \u00d7 12mole = 0.375 mole<\/p>\n
\n1 atom of carbon weighs \u2192 [latex]\\frac{12}{6 \\times 10^{23}}[\/latex]
\n1022<\/sup> atoms of carbon will weigh \u2192 [latex]\\frac{12}{6 \\times 10^{23}} \\times 10^{22}=\\frac{12}{60}=\\frac{1}{5}[\/latex] = 0.2 g<\/p>\n
\nAnswer:
\nMolecular formula = C6<\/sub>H18<\/sub>O3<\/sub>
\nTake the common multiple
\nMolecular formula = (C2<\/sub>H6<\/sub>0)3<\/sub>
\nMolecular formula = (Empirical formula)\u201e
\nThus, empirical formula = C2<\/sub>H6<\/sub>O<\/p>\n
\n1.
\n2.
\nAnswer:
\n1. Prop – 1 – yne or propyne
\n2. Ethanal<\/p>\n
\nAnswer:
\nEthanal
\n
\nSpecial feature of the structure of ethyne is the presence of triple bond.<\/p>\n
\nAnswer:
\nEthane<\/p>\n
\nAnswer:
\nAcetic acid (CH3<\/sub>COOH)<\/p>\n
\n(i) The formula that represents the simplest ratio of the various elements present in one molecule of the compound.
\nAnswer:
\nEmpirical formula<\/p>\n
\nAnswer:
\nAcid<\/p>\n
\nAnswer:
\nElectronegativity<\/p>\n
\nAnswer:
\nCalcination<\/p>\n
\nAnswer:
\nNon-polar covalent bond<\/p>\n
\n(i) K, Pb, Ca, Zn. (In the increasing order of the reactivity)
\nAnswer:
\nPb < Zn < Ca < K
\n(According to the position in reactivity series)<\/p>\n
\nAnswer:
\nNa1+<\/sup> < Mg2+<\/sup> < H1+<\/sup> < Cu2+<\/sup>
\n(According to electrochemical series of metals)<\/p>\n
\nAnswer:
\nH > Li > Na > K
\n(Smaller the size greater is the ionization potential)<\/p>\n
\nAnswer:
\nB < N < O < F
\n(Smaller the size more is the electron affinity)<\/p>\n
\n[H = 1, C = 12]
\nAnswer:
\n<\/p>\n
\n(Attempt any four questions from this Section)<\/p>\n
\n(a) Draw the electron dot structure of : [3]<\/strong>
\n(i) Nitrogen molecule [N = 7]
\nAnswer:
\nNitrogen molecule
\n
\nNitrogen atom shares three electrons forming a triple covalent bond.<\/p>\n
\nAnswer:
\nSodium chloride
\n
\nSodium loses one electron to chlorine forming a positive ion and chlorine gains one electron forming a negative ion. These ions form an electrovalent bond and are held strongly by electrostatic forces of attraction.<\/p>\n
\nAnswer:
\nAmmonium ion
\nN (7) \u2192
\nH (1) \u2192 Hx<\/sup>
\nFormation of ammonia<\/p>\n
\nH – 1e–<\/sup> H+<\/sup>
\nFormation of ammonium ion
\nAmmonia donates its lone pair to proton forming ammonium ion.<\/p>\n
\n
\n(i) Which solution will have no effect on litmus solution?
\n(ii) Which solution will liberate CO2<\/sub>\u00a0when reacted with sodium carbonate?
\n(iii) Which solution will turn red litmus solution blue?
\nAnswer:
\n(i) C (Because pH 7 is neutral).
\n(ii) B (Because acids liberate CO2<\/sub> gas when treated with carbonates and acids have pH less than 7)
\n(iii) A (Bases turn red litmus blue and they have pH more than 7)<\/p>\n
\n(i) Which element forms electrovalent compound with G?
\n(ii) The ion of which element will migrate towards the cathode during electrolysis?
\n(iii) Which non-metallic element has the valency of 2?
\n(iv) Which is an inert gas?
\nAnswer:
\n(i)
\n
\n(ii) A [Positive ions migrate towards cathode, hence A will form A+ and migrate towards cathode]
\n(iii) E
\n(iv) F<\/p>\n
\n(a) Name the particles present in:
\n(i) Strong electrolyte
\n(ii) Non-electrolyte
\n(iii) Weak electrolyte
\nAnswer:
\n(i) Only ions
\n(ii) molecules
\n(iii) Ions as well as molecules<\/p>\n
\n(i) Manganese dioxide and copper (II) oxide, (using concentrated HCl)
\nAnswer:
\n<\/p>\n
\nAnswer:
\n
\n(iii) Dilute hydrochloric acid and dilute sulphuric acid, (using lead nitrate solution)
\nAnswer:
\n
\n(c) Choose the method of preparation of the following salts, from the methods given in the list: [4]<\/strong>
\n[List: A. Neutralization
\nB. Precipitation
\nC. Direct combination
\nD. Substitution]
\n(i) Lead chloride
\n(ii) Iron (II) sulphate
\n(iii) Sodium nitrate
\n(iv) Iron (III) chloride
\nAnswer:
\n(i) Lead chloride \u2192 Precipitation(B)
\n(ii) Iron (II) sulphate \u2192 Substitution (D)
\n(in) Sodium nitrate \u2192 Neutralisation (A)
\n(iv) Iron (III) chloride \u2192 (Direct combination) (C)<\/p>\n
\n(a) Complete the following equations : [3]<\/strong>
\n(i) S + cone. HNO3<\/sub> \u2192
\n(ii) C + cone. H2<\/sub>SO4<\/sub> \u2192
\n(iii) Cu + dil.HNO3<\/sub> \u2192
\nAnswer:
\n(i) S + 6HNO3<\/sub> \u2192 H2<\/sub> SO4<\/sub> + 6NO2<\/sub> + 2H2<\/sub>O
\n(ii) C + 2H2<\/sub> SO4<\/sub> \u2192 2H2<\/sub>O\u00a0+ CO2<\/sub> + 2S02<\/sub>
\n(iii) 3Cu + 8HNO3<\/sub> \u2192 3CU(NO3<\/sub> )2<\/sub> + 2NO + 4H2<\/sub>O<\/p>\n
\n(i) Ethene from bromoethane
\nAnswer:
\n+ KOHf (alc.) CH2<\/sub> = CH2<\/sub> + KBr+H2<\/sub>O<\/p>\n
\nAnswer:
\n<\/p>\n
\nAnswer:
\n<\/p>\n
\n(i) The compound with 3 carbon atoms whose functional group is a carboxyl.
\n(ii) The first homologue whose general formula is Cn<\/sub>H2n<\/sub>.
\n(iii) The compound that reacts with acetic acid to form ethyl ethanoate.
\n(iv) The compound formed by complete chlorination of ethyne.
\nAnswer:
\n(i) propanone
\n(ii) ethene
\n(iii) ethanol
\n(iv) 1,1,2,2 tetrachloro ethane<\/p>\n
\n(a) Give the chemical formula of: [3]<\/strong>
\n(i) Bauxite
\n(ii) Cryolite
\n(iii) Sodium aluminate
\nAnswer:
\n(i) Al2<\/sub>O3<\/sub>. 2H2<\/sub>O
\n(ii) Na3<\/sub>AlF6<\/sub>
\n(iii) NaAlO92<\/sub><\/p>\n
\n(i) What is the function of cryolite used along with alumina as the electrolyte?
\n(ii) Why is powdered coke sprinkled on top of the electrolyte?
\n(iii) Name the electrode, from which aluminium is collected.
\nAnswer:
\n(i) Cryolite acts as a solvent and lower the fusion temperature from 2050\u00b0C to 950\u00b0C.
\n(ii) A layer of powdered coke is sprinkled over the surface of the electrolyte to reduce the heat loss by radiation and prevent the carbon rod from binning in air.
\n(iii) Cathode<\/p>\n
\n
\nAnswer:
\n(i) Duralumin \u2192 Aircraft body
\n(ii) Solder \u2192 Electrical fuse
\n(iii) Brass \u2192 Decorative articles
\n(iv) Stainless steel \u2192 Surgical instruments<\/p>\n
\n(a) Identify the substances underlined: [3]<\/strong>
\n(i) The catalyst<\/span> used to oxidise ammonia.
\n(ii) The organic compound<\/span> which when solidified- forms an ice like mass.
\n(iii) The dilute acid<\/span> which is an oxidizing agent.
\nAnswer:
\n(i) Platinum
\n(ii) Acetic acid
\n(iii) Nitric acid<\/p>\n
\n2NaOH + CuSO4<\/sub> \u2192 Na2<\/sub>SO4<\/sub> + Cu(OH)2<\/sub>\u2193
\n(i) What mass of copper hydroxide is precipitated by using 200 gm of sodium hydroxide ? [H = 1, O = 16, Na = 23, S = 32, Cu = 64]
\nAnswer:
\n
\n98 g of CU(OH)2<\/sub> is precipitated by using 80 g of NaOH
\nl g of CU(OH)2<\/sub> is preapitated by using [latex]\\frac { 80 }{ 98 }[\/latex]g of NaOH
\n200 g of CU(OH>2 is preapitated by using [latex]\\frac{80}{98} \\times 200 g[\/latex] = 163.26 g of NaOH<\/p>\n
\nAnswer:
\nPale blue precipitates<\/p>\n
\nC = 75.92%, H = 6.32% and N = 17.76%
\nThe vapour density of the compound is 39.5.
\n[C= 12, H= 1,N= 14] [4]<\/strong>
\nAnswer:
\n
\nEmpirical Formula \u21d2 C5<\/sub>H5<\/sub> N
\nVapour density = 39.5
\nMolecular Mass = 2 \u00d7 V.D.
\n= 2 \u00d7 39.5 = 79
\nEmpirical formula Mass = 12 \u00d7 5 + 5 \u00d7 1 + 1 \u00d7 14
\n= 60 + 5 + 14
\n= 79
\nn = [latex]\\frac { Molecular formula mass }{ Empirical formula mass }[\/latex]= [latex]\\frac { 79 }{ 79 }[\/latex]
\nThus, both Empirical formula and Molecular formula are C3<\/sub>H5<\/sub>N.<\/p>\n
\n(a) Name the gas evolved in each of the following cases : [3]<\/strong>
\n(i) Altunina undergoes electrolytic reduction.
\n(ii) Ethene undergoes hydrogenation reaction
\n(iii) Ammonia reacts with heated copper oxide
\nAnswer:
\n(i) Oxygen
\n(ii) Ethane
\n(iii) Nitrogen<\/p>\n
\nAnswer:
\n(A) Mg3<\/sub>N2<\/sub> + 6H2<\/sub>O \u2192 3Mg(OH)2<\/sub> + 2NH3<\/sub>
\n(B) NH3<\/sub>+ HCl \u2192 NH4C1
\n(C) <\/p>\n
\n
\nAnswer:
\n(i) Haber\u2019s process
\n(ii)
\n
\n(iii) Contact process
\n(iv)
\n<\/p>\nICSE Class 10 Chemistry Previous Years Question Papers<\/a><\/h4>\n","protected":false},"excerpt":{"rendered":"