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ICSE SUGGESTIVE PAPER CHEMISTRY FOR CLASS 10 FOR ICSE 2016 EXAM MARKS:80 FULL TIME:2 Hours SECTION A. QUESTION1 a. Name the following.[5] 1. 2. 3. 4. 5. The compound having all the three bonds. An acid which turns blue litmus pink. The industrial process by which nitric acid is manufactured. A salt soluble in hot water but insoluble in cold water. The gas liberated when sodium reacts with ethanol. b. State one relevant observation in each case.[5] 1. Hydrogen chloride gas is passed through silver nitrate solution. 2. 3. 4. 5. Ethylene is passed through a solution of bromine in carbon tetrachloride. A glowing splint is introduced in a gas jar containing oxygen. Lead nitrate is heated. Excess ammonia solution is added to a salt obtained when dry chlorine is passed through iron. c. Write balanced chemical equation for the following.[5] 1. Ammonia and excess chlorine. 2. Potassium nitrate is heated. 3. Laboratory preparation of acetylene. 4. Dilute sulphuric acid and zinc. 5. Manganese dioxide and conc. Hydrochloric acid. d. 1.)State Avogadro s [1] ii) Calculate the mass of 3x1025 molecules of carbon dioxide at S.T.P (C= 12; O=16)[1] iii) The combustion of acetylene in the presence of air is as follows. [C2H2 + O2 CO2 + H2O] Calculate the volume of air required for complete combustion of 100 cm3 acetylene. e. Fill in the blanks (do not copy the sentence) [5] Covalent compounds are generally soluble in ________ solvent. (Polar, non polar) For the formation of an ionic bond between a metal and a non-metal, the metal should have ________(high, low) ionisation energy and the nonmetal should have ________ electron affinity (high, low). The ferrous ion _________ an electron to form the ferric ion.( loses, gains) The bond between two elements in the right side of the periodic table is likely to be _______ (ionic, covalent). The most electronegative element is ________ (chlorine, fluorine). f. Give reasons for the following [3] 1. Iron nail kept in a closed jar containing calcium chloride does not rust. 2. Copper does not displace hydrogen from dilute acids. 3. Highly reactive metals cannot be obtained from their oxides by heating them with Carbon g. The reaction between metal X and Fe2O3 is highly exothermic and is used to join railway(iron girdles) [2] 1. Identify metal X and name the reaction. 2. Write the chemical equation of its reaction with Fe2O3. h. . A group of periodic table is given below: Fluorine, chlorine, bromine and iodine Answer the following questions in relation to this group of elements:[5] (i) Which element has the most non-metallic character? (ii) Which would you expect to have highest I.P. (iii) Name the type of bond and type of compound formed between iodine and hydrogen. (iv) Which of the element has largest atomic size. (v) Give the formula of compound formed between chlorine and an element with atomic no 6 and draw its electronic configuration. i. Draw the structural formula of: [2] 1. 1,2,dichloroethene 2. Acetone. j. Rewrite each incorrect statement, correctly in full. 1. Copper reacts with dilute nitric on heating evolving nitrogen dioxide gas. 2. Pure water is a weak electrolyte and hence acidified with dilute nitric acid. 2. Gay Lussacs law establishes the relationship between volume and number of molecules. SECTION B.[40 Marks] Q2. a. The following diagram of catalytic oxidation of ammonia. With reference to this ansew the following questions. [5] 1. 2. 3. 4. 5. Write a balanced chemical equation for the reaction. Name the catalyst and the required temperature for the reaction. What do you observe in flask C. The catalyst continues to glow even if heating is discontinued. Write an equation for the formation of Nitric acid using the product C. b. Draw the electron dot diagram to show the formation of ammonium ion from ammonia molecule.[2] c. Arrange the following as per instruction given in the bracket[3] 1. Mg, Na, Al, Si (increasing order of electropositive character) 2. F, Cl, I, Br ( decreasing order of nuclear charge) 3. SO4 2- , OH- , Br- , NO3 (decreasing ease of reduction) QUESTION 3. a. 1. 2. 3. b. c. d. Name the metal which is common in the following alloys.[3] Bronze and Solder. Type metal and Bronze Stainless and German silver Two elements M and N belong to group 1 and 2 respectively and are in the same period of the periodic table. How do the following properties of M and N vary?[3] 1. Size of their atoms 2. Their metallic character. 3. Molecular formula of their chlorides. What do you observe if Hydrogen chloride gas is reacted with Ammonium solution. Also give its equation. [2] What do you understand by.[2] 1. water of crystallization 2. Redox reaction. QUESTION 4. a. With reference to the given picture .Answer the following questions[5] 1. 2. 3. 4. Name the acid prepared and the name of the process shown above. State the colour of flame seen when the first equation above takes place. Why vanadium pentaoxide is chosen as the suitable catalyst. Write two equation. fisrt react SO3 with H2SO4 . and second the product formed to give sulphuric acid . An acid of phosphorus has the following percent composition H=2.47%, P=38.27% 0=59.26% [4] 1. Find the empirical formula of acid and its molecular formula. Given that its relative molar mass is 162 (H = 1, P = 31, 0 = 16). b. c. Why do ionic compounds have high melting point[1] QUESTION 5 a. Give the following equations.[3] 1. Bromoethane to Ethyl alcohol 2. Acetic acid and ethyl alcohol. 3. Catalytic oxidation of methane to give methanol. b. c. Give reasons[3] 1. Acetic acid is called glacial acetic acid. 2. Almost 90% of compounds are organic. 3. Methane is collected by downward displacement of water,during its laboratory preparation. Name them[4] 1. The property of metals by virtue of which they can be beaten into sheets. 2. Drying agent used during the preparation of Hydrogen chloride during its laboratory preparation. 3. 4. The colour of the precipitate when Ferric chloride reacts with caustic alkali. The electrolyte best suited for the electroplating an article with silver. QUESTION 6 a. The following questions refer to electrolysis of fused lead bromide. [5] 1. What is the nature of electrode used. 2. Write the reaction for dissociation of the electrolyte. 3. Give reason why the electrolytic cell is made up of silica. 4. Write the reaction taking place at the Cathode. 5. Write the observation made at the anode. b. With reference to acids , answer these questions.[5] 1. Define the term acid. 2. Name the acid used as an eye wash. 3. 4. 5. Write a balanced equation to show how Sulphuric acid is prepared using Nitric acid. State the colour change when acid is added to methyl orange solution. Name the acid which is called the king of acids. QUESTION 7 a. b. c. d. e. f. State Gay Lussacs Law.[1] A hydrocarbon contains 82.8% Carbon. If its vapour density is 29, find its molecular formula. [3] What is meant by denatured alcohol[1] Name the gas which smells like a rotten eggs[1] Give a chemical test to distinguish between Sulphur dioxide and Carbon dioxide[2] If there are two test tubes of which one contains Ammonium hydroxide solution and other contains Sodium hydroxide solution, doing one specific test how would you determine which test tube contains which solution.[2]
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