ICSE BOARD PAPER - 2010 - X - Chemistry 2010 Set 1

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  • Q1

    (a)    From the list given below, select the word(s) required to correctly complete the blanks (i) to (v) in the following passage:

    Note: Words chosen from the list are to be used only once. Write only the answers. Do not copy the passage.

    [reddish brown, ammonium, nitrogen dioxide, hydroxyl, dirty green, ammonia, acidic, alkaline]

     

    Nitrogen and hydrogen combine in the presence of a catalyst to give (i) _____ gas. When the above mentioned gas is passed through water, it forms a solution which will be (ii) ______ in nature and the solution contains (iii) ______ ions and (iv)_______ ions. The above solution when added to iron (II) sulphate solution, gives a (v) _______ coloured precipitate of iron (II) hydroxide.  [5]

     

    (b)    Select from the list given (A to E) one substance in each case which matches the description given in parts (i) to (v). (Note: Each substance is used only once in the answer.)

    (A)    Nitroso Iron (II) sulphate (B) Iron (III) Chloride (C) Chromium sulphate (D) Lead (II) Chloride (E) Sodium chloride.

     

    (i)     A compound which is deliquescent.

    (ii)    A compound which is insoluble in cold water but soluble in hot water.

    (iii)    The compound responsible for the brown ring during the brown ring test of nitrate ion.

    (iv)   A compound whose aqueous solution is neutral in nature.

    (v)    The compound which is responsible for the green colouration when sulphur dioxide is passed through acidified potassium dichromate solution.  [5]

     

    (c)    For part (c)(i) – (c)(x), select the correct answer from the choices A,B,C and D which are given. Write only the letter corresponding to the correct answer.

     

    (i)          A particular solution contains molecules and ions of the solute, so it is a:

    (A) weak acid.                    (B) strong acid.

    (C) strong base.                  (D) salt solution.

    (ii)        A compound which liberates reddish brown gas around the anode during electrolysis in its molten state is:

    (A) sodium chloride.            (B) copper(II) oxide.

    (C) copper(II) sulphate.       (D) lead(II) bromide.

    (iii)        An organic compound undergoes addition reaction and gives a red colour precipitate with ammonical cuprous chloride. Therefore, the organic compound could be:

    (A) ethane.   (B) ethene.   (C) ethyne.   (D) ethanol.

    (iv)       An organic weak acid is:

    (A) formic acid.                  (B) sulphuric acid.

    (C) nitric acid.                    (D) hydrochloric acid.

    (v)        During ionization metals lose electrons, this change can be called:

    (A) oxidation    (B) reduction   (C) redox    (D) displacement

    (vi)       Which one of the following is not true of metals:

    (A) Metals are good conductors of electricity.

    (B) Metals are malleable and ductile.

    (C) Metals from non-polar covalent compounds.

    (D) Metal will have 1 or 2 or 3 electrons in their valence shell.

    (vii)      An example of a complex salt is:

    (A) zinc sulphate.                                (B) sodium hydrogensulphate.

    (C) iron(II) ammonium sulphate.   (D) tetrammine copper(II) sulphate.

    (viii)    Aqua regia is a mixture of:

    (A) dilute hydrochloric acid and concentrated nitric acid.

    (B) concentrated hydrochloric acid and dilute nitric acid.

    (C) concentrated hydrochloric acid [1 part] and concentrated nitric acid [3 parts].

    (D) concentrated hydrochloric acid [3 parts] and concentrated nitric acid [1 part].

    (ix)       The organic compound mixed with ethanol to make it spurious is:

    (A) methanol.                             (B) methanoic acid.

    (C) methanal.                             (D) ethanoic acid.

    (x)        The number of electrons present in the valence shell of a halogen is:

    (A) 1.                (B) 3.                (C) 5.                (D) 7.               [10]

     

    (d)    State your observation for the following cases:  [5]

    (i)      Moist blue litmus is introduced into a gas jar of sulphur dioxide.

    (ii)    Dry red rose petals are placed in the jar of sulphur dioxide.

    (iii)   Paper soaked in potassium permaganate solution is introduced into a gas jar of sulphur dioxide.

    (iv)  Ammonia gas is burnt in an atmosphere of oxygen in the absence of a catalyst.

    (v)    Glass rod dipped in ammonium hydroxide is brought near the mouth of the concentrated hydrochloric acid bottle.

     

    (e)    Match the column A with column B.   [5]

     

    Column A

    Column B

    (i)

    Sodium chloride

    Increases

    (ii)

    Ammonium ion

    Covalent bond

    (iii)

    Electro negativity across the period

    Ionic bond

    (iv)

    Non metallic character down the group

    Covalent and Coordinate bond

    (v)

    Carbon tetrachloride

    Decreases

     

              Answer as follows:

    (i)                  Correct item from B matching sodium chloride.

    (ii)                 Correct item from B matching ammonium ion and so on.

     

    (f)    Write the equation for each of the following reactions: [5]

            (i) Sulphur is heated with concentrated sulphuric acid.

            (ii) Zinc oxide is treated with sodium hydroxide solution.

            (iii) Ammonium chloride is heated with sodium hydroxide. 

            (iv) Concentrated sulphuric acid is poured over sugar.

    (v) Magnesium sulphate solution is mixed with barium chloride solution.

     

    (g)   (i)     LPG stands for liquefied petroleum gas. Varieties of LPG are marketed including a mixture of propane (60%) and butane (40%). If 10 litre of this mixture is burnt, find the total volume of carbon dioxide gas added to the atmosphere. Combustion reaction can be represented as:

           

            (ii)    Calculate the percentage of nitrogen and oxygen in ammonium nitrate. [Relative molecular mass of ammonium nitrate is 80, H=1, N=14, O=16] [5]

    Marks:40
    Answer:

    (a)   (i)     Ammonia                           (ii)    Alkaline

            (ii)    Ammonium                         (iii)    Hydroxyl

            (v)    Dirty green

     

    (b)   (i) B  (ii) D  (iii) A  (iv) E  (v) C

     

    (c)    (i) A  (ii) D  (iii) C  (iv) A  (v) A  (vi) C  (vii)  D (viii) D  (ix) A  (x) D

     

    (d)   (i)     Litmus turns blue to red then gets bleached.

            (ii)    Red rose petals turn white.

            (iii)    Paper turns pink to white.

            (iv)   Ammonia burns with a green flame.

            (v)    Dense white fumes are observed.

     

    (e)   (i)     Ionic bond.                

    (ii)    Covalent and coordinate bond.

            (iii)    Increases.                 

    (iv)   Decreases.

            (v)    Covalent bond.

     

     

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  • Q2

    (a)    Give the equations for the following conversation A to E.  [5]

    (b)    The questions below are related to the manufacture of ammonia.  [5]

            (i)     Name the process.

            (ii)    In what ratio must the reactants be taken?

            (iii)    Name the catalyst used.

            (iv)   Give the equation for the manufacture of ammonia.

            (v)    Ammonia can act as a reducing agent – write a relevant equation for such a reaction. 

    Marks:10
    Answer:

       

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  • Q3

    (a)    Draw the structural formula for each of the following: [2]

            (i) Ethanoic acid (ii) But-2-yne     

    (b)    Mr. Ramu wants to electroplate his key chain with nickel to prevent rusting. For this electroplating: [5]

            (i)     Name the electrolyte.

            (ii)    Name the cathode.

            (iii)    Name the anode.

            (iv)   Give the reaction at the cathode.

            (v)    Give the reaction at the anode.

     

    (c)    Three different electrolytic cells A, B and C are connected in separate circuits. Electrolytic cell A contains sodium chloride solution. When the circuit is completed, a bulb in the circuit glows brightly. Electrolytic cell B contains acetic acid solution and in this case the bulb in the circuit glows dimly. The electrolytic cell C contains sugar solution and the bulb does not glow. Give a reason for each of these observations.  [3]

    Marks:10
    Answer:

    a)

    (c)   

    In Cell A: Sodium chloride being strong electrolyte dissociates completely and therefore current flows better.

    In Cell B: Acetic acid being weak electrolyte ionises only partially and therefore, only a weak current flows. In Cell C: Sugar being a covalent compound does not ionise at all and therefore, no current flows. 

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  • Q4

    (a)    4.5 moles of calcium carbonate are reacted with dilute hydrochloric acid. [5]

            (i) Write the equation for the reaction.

            (ii) What is the mass of 4.5 moles of calcium carbonate? (Relative molecular mass of calcium carbonate is 100).

            (iii) What is the volume of carbon dioxide liberated at STP?

            (iv) What mass of calcium chloride is formed? (Relative molecular mass of calcium chloride is 111).

            (v) How many moles of HCl are used in this reaction?

     

    (b)    The diagram shows an apparatus for the laboratory preparation of hydrogen chloride. [5]

     

              (i) Identify A and B.

            (ii) Write the equation for the reaction.

            (iii) How would you check whether or not the gas jar is filled with hydrogen chloride?

            (iv) What does the method of collection tell you about the density of hydrogen chloride? 

    Marks:10
    Answer:

     

               (iii)    If a moist blue litmus is brought near the mouth of gas jar it turns red, it shows that the gas jar is filled with HCl.

            (iv)   Hydrogen chloride is denser than air. 

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  • Q5

    (a)    Name the main constituent metal in the following alloys:   [3]

            (i) Duralumin (ii) Brass (iii) Stainless Steel

    (b)    An element has an atomic number 16. State:[3]

            (i)     the period to which it belongs.

            (ii)    the number of valence electrons.

            (iii)    whether it is a metal or non-metal.

    (c)    Solution A is a sodium hydroxide solution. Solution B is a weak acid. Solution C is dilute sulphuric acid. Which solution will:         [3]

            (i)     liberate sulphur dioxide from sodium sulphite.

            (ii)    give a white precipitate with zinc sulphate solution.

            (iii)    contain solute molecules and ions?

    (d)    By the addition of only one solution how would you distinguish between dilute hydrochloric acid and dilute nitric acid?   [1]

    Marks:10
    Answer:

    (a)   (i) Aluminium       (ii) Copper                 (iii) Iron

    (b)   (i) 3rd period        (ii) six electrons         (iii) Non-metal

    (c)    (i) C                  (ii) A                         (iii) B

    (d)   Silver nitrate solution when added to dil. hydrochloric acid will give a white ppt. and when added to dil. nitric acid no change will be observed. 

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  • Q6

    (a)  Give the equation for the preparation of each of the following salts from the starting material given. [5]

    (i)   Copper sulphate from copper(II) oxide.

    (ii)  Iron(III) chloride from Iron.

    (iii) Potassium sulphate from potassium hydroxide solution.

    (iv) Lead chloride from lead carbonate (two equations).

     

     

    (b) Compound A is bubbled through bromine dissolved in carbon tetrachloride and the product is CH2 Br-CH2Br.

               
    (i)    Draw the structural formula of A.
    (ii)   What type of reaction has A undergone?
    (iii)  What is your observation?
    (iv)  Name (not formula) the compound formed when steam reacts with A in the presence of phosphoric acid.
    (v)   What is the procedure for converting the product of (b)(iv) back to A?[5]

    Marks:10
    Answer:

    (b)   (i)  

            (ii)    Addition reaction.

            (iii)    Bromine solution gets decolourised.

            (iv)   Ethanol.

            (v)    By heating it (ethanol) with concentrated sulphuric acid at 170OC.

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  • Q7

    (a) The diagram shows a simple arrangement of the fountain experiment:                                             [3]

    (i) Name the two gases you have studied which can be used in this experiment.

     

    (ii) What is the common property demonstrated by this experiment?

     

    (b) Define the following terms:                                [2]

    (i) Ionization potential.

     

    (ii) Electron affinity.
     

    (c) The action of heat on the blue crystalline solid L gives a reddish brown gas M, a gas which relights a glowing splint and leaves a black residue. When gas N (which has a rotten egg smell) is passed through a solution of L, a black precipitate is formed.   [5]

     

    (i) Identify L, M and N (Name or formula).

     

     

    (ii) Write the equation for the action of heat on L. 

     

    (iii) Write the equation for the reaction between the solution of L and the gas N. 

    Marks:10
    Answer:

    (a) (i) Hydrogen chloride and ammonia gas.

     

         (ii)    High solubility of the gas in water.
     

    (b) (i) Ionization potential : It is the amount of energy required to remove an electron from the outer most(valence) shell of an isolated gaseous atom. 

    (ii) Electron affinity : It is the amount of energy released when an electron is added to the outer most (valence) shell of an isolated gaseous atom. 

    (c) (i) L is copper nitrate.

             M is nitrogen dioxide gas.

             N is hydrogen sulphide gas.

     

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