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ICSE Class X Mid-term 2024 : Chemistry : 2ND MOCK

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2nd MOCK TEST CHEMISTRY FM-80 TIME-2Hrs Maximum Marks : 40 Time allowed : One hour and half hours Answers to this Paper must be written on the paper provided separately. You will not be allowed to write during the first 10 minutes. This time is to be spent in reading the question paper The time given at the head of this Paper is the time allowed for writing the answers. Attempt all questions from Section A and any three questions from Section B The intended marks for questions or parts of questions are given in brackets. [ ] SECTION I- 40 MARKS (Answer all the questions from this section) Question1Choose the most appropriate answer. (i) [15] A salt which in solution gives a bluish white precipitate with NaOH solution and a white precipitate with BaCl2 solution is: A CuSO4 B C FeSO4 Fe2(SO4)3 D CuCl2 (ii) Hydrogen chloride can be obtained by adding concentrated Sulphuric acid to: NaCl A B Na2SO4 C Na2CO3 D NaNO3 (iii) Which of the following reactions gives copper as a product A Passing dry ammonia over heated copper oxide. B C D Adding dilute hydrochloric acid to copper oxide. Heating copper oxide. Passing oxygen over heated copper oxide. (iv) The particles present in dilute nitric acid are: A. Ions only B. Molecules only C. Both ions and molecules D. Atoms only (v) The aim of the fountain experiment is to prove A HCl turns blue litmus red B HCl is denser than air C HCl is soluble in water D HCl is soluble in toluene (vi) (vii) Polarity of a molecule depends on difference A. electropositivity B. electro affinity C. size difference D. electronegativity The molecule containing a triple covalent bondis: A. ammonia Cwater B. methane D .nitrogen (viii) If an element A belongs to Period 3 and Group II then it willhave: A. 3 shells and 2 valenceelectrons B. 2 shells and 3 valenceelectrons C. 3 shells and 3 valenceelectrons D. 2 shells and 2 valenceelectrons (ix) When fused lead bromide is electrolysed weobserve: A.a silver grey deposit at anode and a reddish brown deposit atcathode B. a silver grey deposit at cathode and a reddish brown deposit atanode C. a silver grey deposit at cathode and reddish brown fumes atanode D.silver grey fumes at anode and reddish brown fumes at cathode. (x)The ratio between the number of molecules in 2g of hydrogen and 32g of oxygen is: A1:2 B1 : 0.01 C1:1 [Given that H = 1, O = 16] D 0.01 : 1 (xi) A reagent that can be used to distinguisg between ammonia and hydrogen chloride A.Alkaline pyragallol C.Copper chloride solution B.Starch iodide paper D.Lime water (xii) The cause of back suction while dissolving ammonia or hydrogen chloride A. B. C. D. Rate of production < Rate of absorption Rate of production > Rate of absorption Rate of production = Rate of absorption Both A & B (xiii)The electrolyte used for electroplating an article with silveris: (A) silvernitratesolution (B) silver cyanidesolution (C) sodiumargentocyanidesolution (D) nickel sulphate solution (xiv) The impurity that can poison the catalyst in Contact Process A. Silica B. Arsenic oxide (xv) B. Ferric hydroxide D.Vanadium pentoxide The particles present in strong electrolytes are: A Only molecules B Mainly ions C Ions and molecules D Only atoms 2.(a). Complete the following statements: [5] a. The reduced product obtained when sulphur dioxide gas is passed through the chlorine water is_____________. b. _____________ reacts with conc. nitric acid to form sulphuric acid. c. An acid contains a replaceable _______ atom/ d. Sodium chloride ____________ in water. e. ____________ molecule contains a lone pair of electrons. b. Match the following : Column A a. Contact process b. Nessler s reagent 3. Nitric acid c. Nitrogen trichloride d. Silver chloride [5] Column B 1. Ammonia 2. Azeotrope 3.Platinum 4. Ammonia solution 5. Yellow liquid (c).State one relevant observation for each of the following reactions: [5] (i) When ammonium hydroxide is added to copper nitrate solution till in excess. (ii) When hydrogen sulphide gas is passed through conc. Sulphuric acid. (iii) At anode during the electrolysis of acidified water. (iv) When zinc is treated with conc. Nitric acid. (v) Aluminium metal is boiled with potassium hydroxide solution. (d)(i) A compound X has the following percentage composition: C=26.7%,O=71.1%,H=2.2% [C =12,O = 16, H = 1] [3] Determine the molecular empirical and molecular formula of X, If its R.M.M is 90. (ii) 560 ml of Carbon monoxide is mixed with 500 ml of oxygen and ignited.The chemical equation for the reaction as follows: [2] 2CO + O2 2CO2 Calculate the volume of the oxygen used and carbon dioxide formed in the above reaction. (e)(i) The given set up in the diagram is for the preparation of an acid. [5] a. Name the acid prepared in the set up. b. Name the reactants used. c. State the purpose of using the empty flask. d. State the significance of using the funnel arrangement. e. Name an experiment which demonstrates high solubility of the gas prepared in the flask . SECTION II- 40 MARKS (Answer any 4 questions from this section) 3. (a) Namethefollowing: [2] 1. A mixture that boils without any change in itscomposition. 2. A yellow monoxide that dissolves in hot and concentrates alkali. (b) State the property of sulphuric acid being shown when itreactswith (i) Carbon [2] (ii)Coppercarbonate (c) Correct the following incorrect statements: (i) Lead bromide conducts electricity. (ii) Copper reacts with nitric acid to produce nitrogen dioxide. (ii) Chlorine turns starch iodide paper blue black. [3] (d)Write balanced chemical equation for the following reactions: [3] (i) Precipitation of a lead salt. (ii) Preparation of a soluble salt by the action of dilute acid on insoluble base. (iii) Reaction at cathode during the electrolysis of concentrated sodium chloride solution. 4.a.Write equations for the reactions taking place at the anode during the electrolysis of: [2] 1. Acidified copper sulphate solution with copper electrodes. 2. Molten lead bromide with inert electrodes. b.Name (i) An alkali preferred for the laboratory preparation of ammonia. (ii) The solid formed when excess of ammonia reacts with chlorine. c. Study the figure given below and answer the questionsthatfollow: (i) Identify the gasY. (ii) What property of gas Y does this experimentdemonstrate? [2] [3] (iii) Name another gas which has the same property and can be demonstrated through thisexperiment. d. A gas cylinder contains 12 1024 molecules of oxygen gas. [3] If Avogadro s number is 6 1023; Calculate: (i) the mass of oxygen present in the cylinder. (ii) the volume of oxygen at S.T.P. present in the cylinder. [O = 16] (iii) the number of moles of oxygen present in the cylinder. 5.a.Give reasons: (i) Dilute nitric acid is generally considered as a typical acid but not so in the reaction with metals. (ii) Hydrogen chloride gas fumes in moist air. b. Draw the electron dot structure of the following : (i) Ammonium (ii) Hydronium c. Arrange the following elements according to the instruction given in the brackents : (i) Na, Cl, S, Al, P (ii) Sr, Ra, Be , Mg, Ca (iii) K, Cu, Al, Fe, Zn [2] [2] [3] d. Answer the following questions regarding contact process for the manufacture of sulphuric acid. [3] (i) (ii) (iii) Why is vanadium pentoxide is considered better catalyst than platinised asbestos? Why is heating of catalyst discontinued, as soon as sulphur dioxide starts reacting with oxygen? Write balanced chemical equation for the reaction taking place in the contact tower. 6. a. How would you chemically distinguish between the following pairs ? [2] (i) Sulphuric acid and hydrochloric acid. (ii) Sodium sulphite and sodium thiosulphate b. Here is an electrode reaction: Cu Cu2+ + 2e[2] (i) At which electrode (cathode or anode ) would such a reaction take place)? (ii) Is this an example of oxidation or reduction ? c. Give the missing word . [3] (i) A (n) (i) _____ ( acid/ basic) salt is one in which the hydrogen of an acid has been replaced by a (ii) ____________ (metal/nonmetal). (ii) Superphosphate is an example of a compound called ______(acid salt/ basic salt/normal salt). (iii) Ammonium chloride is a soluble salt prepared by ______( precipitation/ neutralization). d.The following questions are referred to the laboratory preparation of ammonia using slaked lime: [3] (i) Write the balanced equation for the reaction . (ii) Which ammonium salt is not used for the preparation of ammonia and why ? (iii) State the method of collection of ammonia. 7.a. Define: (i) Electron affinity [2] (ii) Basicity of an acid b. Substances X,Y&Z are three solids soluble in water.The solution X does not conduct electricity, the solution of Y is a poor conductor of electricity whereas solution Z is a good conductor of electricity. (i) Which solution contains only molecules ? (ii) Which solution is a strong electrolyte ? c. Identify the cation present in the solution A, B & C [2] [3] (i)Sodium hydroxide is added to salt A gives a gas which forms dense white fumes with moist hydrogen chloride gas. (ii)Ammonium hydroxide is added in excess to salt B giving a white ppt which is not soluble with excess ammonium hydroxide but soluble in excess sodium hydroxide. (iii)Ammonium hydroxide is added in excess to salt C and does not form any ppt .but with sodium hydroxide white ppt is formed. d.Aluminium carbide reacts with water according to the following reaction: [3] Al4C3 + 12H2O 4Al(OH)3 + 3CH4 (i) Calculate the mass of Aluminium hydroxide obtained from 12 g of Aluminium carbide. (ii) Calculate the mass of methane obtained from12g of Aluminium carbide. (iii) Calculate the volume of methane at s.t.p obtained from 12g of Aluminium carbide. [ Al= 27, C = 12, H = 1, O = 16] 8.a. Give reasons: [2] (i) Ionisation potential of element increases across a period. (ii) Electrolysis of molten lead bromide is a redox reaction. b. Calculate the percentage of hydrogen in methane : [ C = 12, H = 1] [2] c. Name a suitable method for the preparation of the following salts of iron : [3] (i) Ferrous chloride (ii) Ferric chloride (iii) Ferrous carbonate d.(i) State the purpose of Haber s process . [3] (ii) State the conditions i.e, catalyst, temperature and pressure in the reaction taking place in the above process. (iv) Write balanced chemical equation for the reaction taking place in Haber s process .

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