Chemistry — Suggested Paper 2

1(i). The organic compound which undergoes substitution reaction is:

1(ii). The most electronegative element from the following elements is:

1(iii). Assertion (A): In the electrolysis of acidified water, the volume of hydrogen liberated is twice the volume of oxygen formed. Reason (R): Water has hydrogen and oxygen in the ratio of 1:2 by volume.

1(iv). Which of the following is a tribasic acid?

1(v). The percentage of hydrogen present in NaOH is: (Relative Molecular Mass of NaOH = 40) (At. Wt. of H = 1)

1(vi). Copper, Zinc and Tin are the metals alloyed to form:

1(vii). Rotten egg smell is due to the liberation of:

1(viii). Which of the following is a common characteristic of a covalent compound?

1(ix). Anhydrous iron (III) chloride is prepared by:

1(x). he drying agent used to dry HCl gas is:

1(xi). An aqueous solution of ammonia is:

1(xii). An atom of X forms an ion according to the equation X ⟶ X⁺2. The atomic number of the atom X is:

1(xiii). The element with highest ionization potential, is:

1(xiv). The electrolysis of acidified water is an example of:

1(xv). Hydracids are those acids which contain:

2(i)(i). Concentrated nitric acid is reacted with sulphur.

2(i)(ii). Ammonia gas is passed over heated copper (II) oxide.

2(i)(iii). Copper sulphate solution is electrolysed using copper electrodes.

2(i)(iv). A small piece of zinc is added to dilute hydrochloric acid.

2(i)(v). Lead nitrate is heated strongly in a test tube.

2(ii)(i). Action of warm water on AlN.

2(ii)(ii). Action of hot and concentrated Nitric acid on copper.

2(ii)(iii). Action of Hydrochloric acid on sodium bicarbonate.

2(ii)(iv). Action of dilute Sulphuric acid on Sodium Sulphite.

2(ii)(v). Preparation of ethanol from Ethyl Chloride.

2(iii)(a). The salt that can be prepared by Direct Combination is ............... . [FeCl₃ / FeCl₂]

2(iii)(b). The metallic oxide which can be reduced by using common reducing agents is ............... .[ Fe₂O₃ / Al₂O₃]

2(iii)(c). The metal nitrate which on thermal decomposition forms a black residue is ............... . [zinc nitrate / copper nitrate]

2(iii)(d). During the electrolysis of copper sulphate solution, if ............... is used as electrodes, the colour of the electrolyte does not fade. [copper / platinum]

2(iii)(e). The process of heating the concentrated ore in a limited supply or absence of air is ............... . [roasting / calcination]

2(iv)(i)(1). 2, 3 – dimethyl butane

2(iv)(i)(2). Diethyl ether

2(iv)(i)(3). Propanoic acid

2(iv)(ii)(1). Crushing of the ore into a fine powder.

2(iv)(ii)(2). Heating of the ore in the absence of air to a high temperature.

2(v)(a). The energy released when an atom in the gaseous state accepts an electron to form an anion.

2(v)(b). Tendency of an element to form chains of identical atoms.

2(v)(c). The name of the process by which Ammonia is manufactured on a large scale.

2(v)(d). A type of salt formed by partial replacement of hydroxyl radicals with an acid radical.

2(v)(e). The ratio of the mass of a certain volume of gas to the same volume of hydrogen measured under the same conditions of temperature and pressure.

3(i)(a). Duralumin

3(i)(b). Stainless steel

3(ii)(a). Sulphuric acid and Nitric acid (using barium chloride solution)

3(ii)(b). Unsaturated and Saturated hydrocarbons (type of bond present)

3(iii)(a). What is the mass of 5 moles of calcium carbonate? (Relative molecular mass of calcium carbonate is 100)

3(iii)(b). How many moles of HCl will react with 5 moles of calcium carbonate?

3(iii)(c). What is the volume of carbon dioxide liberated at S.T.P. at the same time?

3(iv)(a). Methane undergoes complete combustion.

3(iv)(b). Copper carbonate is heated.

3(iv)(c). MnO₂ reacts with concentrated HCl.

4(i)(a). Ammonium hydroxide solution when added to Solution B gives a white precipitate which does not dissolve in excess of ammonium hydroxide solution.

4(i)(b). Sodium hydroxide solution when added to Solution C gives a white precipitate which is insoluble in excess of sodium hydroxide solution.

4(ii)(a). During electrolysis, the compound ............... in its molten state liberates reddish brown fumes at the anode. [NaCl/PbBr₂]

4(ii)(b). The ion which could be discharged most readily during electrolysis is ............... [Fe²⁺/Cu²⁺]

4(iii)(a). Al, K, Mg, Ca (decreasing order of its reactivity)

4(iii)(b). N, Be, O, C (increasing order of non-metallic character)

4(iii)(c). P, Si, F, Be (decreasing order of valence electrons)

4(iv)(a). NH₄Cl + Ca(OH)₂ ⟶

4(iv)(b). CuSO₄ + NH₄OH ⟶

4(iv)(c). Cu + Conc. HNO₃ ⟶

5(i)(a). The ore which can be concentrated by magnetic separation.

5(i)(b). Empirical formula of Ethyne.

5(ii)(a). Copper reacts with concentrated Nitric acid.

5(ii)(b). Aluminium nitride is treated with warm water.

5(iii). Match the salts underlined in Column A with the most suitable method of preparation given in Column B.

5(iv)(a). Give balanced chemical equation for the above reaction.

5(iv)(b). State the method of collection of the gas formed above.

5(iv)(c). What is the property of sulphuric acid that makes it a suitable reagent for the reaction?

6(a). Certain blank spaces are left in the following table and these are labelled as A, B, C, D and E. Identify each of them.

6(c). Write balanced chemical equations to show how SO₃ is converted to Sulphuric acid in the contact process.

6(b)(i). The oxidizing action of conc. Sulphuric acid on Carbon.

6(b)(ii). The behavior of H₂SO₄ as an acid when it reacts with Magnesium.

6(b)(iii). The dehydrating property of conc. Sulphuric acid with sugar.

7(i)(a). Name the acid P used by Seema.

7(i)(b). Write a balanced chemical equation for the reaction that took place.

7(ii)(a). Name the process used to concentrate the ore.

7(ii)(b). Give a balanced chemical equation for the conversion of aluminium hydroxide to pure alumina.

7(iii)(a). An ionic compound formed when Mg reacts with the dilute HCl.

7(iii)(b). A covalent compound formed when H₂ reacts with Cl₂.

7(iii)(c). The positive ion produced when ammonia gas is dissolved in water.

7(iv)(a). Why is dilute sulphuric acid added to water?

7(iv)(b). Write the reaction taking place at the cathode.

7(iv)(c). What is the observation at the anode?

8(i)(a). State Avogadro’s Law.

8(i)(b). Define Co⁻ordinate bond.

8(ii)(a). Ammonium chloride and Sodium chloride (using an alkali)

8(ii)(b). Zinc Nitrate solution and Calcium Nitrate solution (using excess sodium hydroxide solution)

8(iii)(a). A colourless gas which turns acidified K₂Cr₂O₇ from orange to green.

8(iii)(b). A yellow explosive oily liquid formed when excess chlorine gas reacts with ammonia gas.

8(iii)(c). A yellow metallic oxide formed on thermal decomposition of PbCO₃.

8(iv)(a). PbCl₂

8(iv)(b). FeCl₃

8(iv)(c). Na₂SO₄