Chemistry - 1997 ( I.C.S.E)
You are on question 1 of Set I

-Answer to this paper must be written on the paper provided separately .
-You will NOT be allowed to write during the first 15 muintes .
-This time is to be spent in reading the question paper.
-The time given at the head this paper is the time allowed for writing the answer.

- This question paper is divided into two section. Section I contains One question with eight   parts (a) to (h):    all eight parts are to be answered. Section II contains six questions,   numbered 2 to 7.
- You are to answer four of these questions.

The intented marks for questions or parts of questions are given in brackets [ ]. All working, including rough work, Should be done on the same sheet as the rest of the answer 5.

SCIENCE
SECTION - I (40 - Marks)
Answer all questions.

Q 1. (a) Answer the questions below, relating your answers only to salts in the following list :
Sodium Chloride, anhydrous calcium chloride, copper sulphate - 5- water.
(i) What name is given to the water in the compound copper sulphate - 5-water?

(ii) If copper sulphate -5 - water is heated, the water is driven off leaving anhydrous copper sulphate.

(A) What is the colour of anhydrous sulphate?
(B) By what means, other than heating, could you dehydrate copper sulphate -5-water and obtain anhydrous copper sulphate?

(iii) What is deliquescence ?

(iv) Which one of  the salts in the given list is deliquescent ?

Q 1(b) State what you see when :
(i)  a piece of moist blue litmus paper is placed in a gas jar of chlorine.
(ii) a piece of moist red litmus paper is placed in a gas jar of ammonia .
(iii)Silver nitrate solution is added to dilute hydrochloric acid.
(iv)Zinc oxide is heated.
(v) A glowing splint is introduced into a gas jar containing oxygen.
Q 1 (c) Write correctly balanced equations for the following reactions :
(i) Molten sodium and chlorine.
(ii) Nitrogen and oxygen when lightning strikes.
(iii) Iron and dilute sulphuric acid.
(iv) Decomposition of hypochlorous acid in sunlight.
(v) Action of heat on potassium nitrate.

Q 1(d) Water can be split into hydrogen and oxygen under suitable conditions.
The equation representing the change is :
2H₂O(l)        ---------------> 2H₂(g) + O₂(g).
(i) If  a given experiment result in 2500 cm³ of hydrogen being produced, what value of oxygen is liberated at the same time under the same conditions of temperature and pressure?

(ii) The 2500 cm³ of hydrogen is subjected to 2 _1/2   times increases in pressure (temperature remaining constant ). What volume will the hydrogen now occupy ?

(iii) Taking the volume of hydrogen calculated in (d) (ii), what change must be made in the kelvin (absolute) temprature to return the volume to  2500 cm³ (pressure remaining constant)?

Q 1 (e). The compound Na₂B₄O₇.10H₂O is commonly known as borax. When litmus is added to a solution of borax solution, it turns blue
(i) What can you say about the pH of borax solution?
(ii) Calculate the precentage of boron (B) in borax. (H = 1, B = 11, O = 16, Na = 23. Answer correct to 1 decimal place.) 

Q 1 (f). (i) Sodium hydoxide solution can be used to distinguish between iron (II) sulphate solution and iron (III) sulphate solution because these solution give different coloured precipitates with sodium hydroxide solutions. Give the colour of the precipitate formed with :
(1) iron (II) sulphate solution ;
(2) iron (III) sulphate solution.

(ii) What will you see when barium chloride solution is addded to iron (II) sulphate solution?

(iii) How will the action of dilute hydrochloride acid on sodium carbonate and sodium sulphite enable you to distinguish between these two compounds?

Q 1(g). Choosing only words from the following list write down the appropriate words to fill in the blanks (i) to (v) below :
anions, anode cathode, cations, electrode, electrolyte, nickel, voltameter.

To electroplate an article with nickel requires an (i) ..............................which must be a solution containing (ii)...................... ions. The article to be plated is placed as the(iii).................................. of the cell in which the plating is carried out .The (iv)............................ of the cell is made from pure nickel. The ions which are attracted to the negative electrodes and discharged are called (v) .......................................... .

Q 1(h).The following question result to the Nitrogen Cycle.
(i) What are the soluble nitrogen compounds absorbed by the roots of plants ?
(ii) What kind of plants directly absorb nitrogen from the atmosphere ?
(iii) What term is applied to the conversion of atmosphere nitrogen to useful compounds of nitrogen?
(iv) Compounds such as ammonium nitrate. urea and super - phosphate are used to replace nitrogen and other elements loss from the soil as a result of cultivation. What is the common name given to these compounds ?
(v) What insoluble substance is used in making superphosphate?

SCIENCE
SECTION - II (40 Marks )
Answer any four questions

Q 2(a) (i) Name the oxide of sulphur which react with water to give sulphuric acid.
(ii) In the contact Process the direct reaction between the oxide of sulphur and water is avoided. In the process, what dfoes the oxide of sulphur react with instead of water and what is the name of the product?
(iii) Give the name and formula of the acid salt which can give sodium ions and sulphate ions in solution.

Q 2(b) The metal zinc is extracted from the ore zinc blende.
(i) Name the zinc compound in zinc blende.
(ii) Zinc blend when rosted in air gives off a gas which, iff allowed to escape, would constitute an atmospheric pollutant. What is this gas?
(iii) What particular polluting effect does this gas have?

Q 2 (c) Write correctly balanced equations for the   reaction in dilute sulphuric acid with each of the following :
(i) Copper carbonate (ii) Lead nitrate solution (iii) Zinc hydroxide

Q 3 (b) Industrically ammonia is obtained by direct combination between nitrogen and hydrogen.
(i) Write the correctly balance equation for the direct combination of nitrogen and hydrogen?
(ii) Which of the metals - iron, platinum. copper catalyse - this direct combination?
(iii) Is the formation of ammonia promoted by the use of high pressure or low pressure?


Q 3 (c) (i) Is ammonia more dense or less dense than air?
(ii) What property of ammonia is demonstrated by the Fountain Experiment?
(iii) Write the correctly balanced equation for the reaction between ammonia and sulpuric acid.

Q 4 (b) Ammonia burn in oxygen and the combustion, in the presence of a catalyst,may be represented by :
2NH₃ + 2_1/2O₂ ® 2NO + 3H₂O
(i) What mass of steam is prodused when 1.5g of nitrogen monooxide is formed?
(ii) What volume of oxygen, at stp, is required to form 10 moles of products? [H = 1: N = 14 : O = 16. 1mole of gas occupies 22.4dm³ (22.4 liter) at stp].

Q 5 (c) (i) How many valence electrons are present in :
(1) Metals
(2) Non - Metals?

(ii) Name all the particles found in a solution of sodium chloride?

Q 6 (a) (i) Ethane and chlorine react together to form monochloroethane(ethyl chloride).
(1) Write down the structural formula of ethane.
(2) What type of reaction has taken place between ethane and chlorine.

Q 6 (a)(ii) The type of reaction between ethene and chlorine is different from that between ethane and chlorine.
(1) What is the type of reaction between ethene and chlorine?
(2) What fercture of the ethene structure makes such a reaction possible ?
(3) Name the product of the reaction between ethene and chlorine.

Q 6 (b) Ethane burns completely in air or oxygen to give carbon dioxide(and water vapour). With a limited supply of air/oxygen carbon monoxide is formed. The same gases are found in automobile exhaust gases. Both gases can be considered as atmospheric pollutants.
(i) Write the equation of the complete combustion of ethane.
(ii) What danger is associated with carbon monoxide.
(iii) What effect is associated with too much carbon dioxide in the atmosphere
(iv) Burning acetylene (ethyne) in oxygen under appropriate condition produces a very hot flame. What is this hot flame used for?

Q 7(a) Solution P has a pH of 13,solution Q has a pH of 6 and solution R has a pH of 2.
(i) Which solution will liberate ammonia from ammonium sulphate on heating?
(ii) Which solution is a strong acid?
(iii) Which solution contains solute molecules as well as ions?

Q 7(b) From the list of substances given below ,choose the pair required to prepare the salts (i) to (iii) in the laboratory and write down the relevant equations .

The substance are :
chlorine , iron, lead, lead nitrate solution, sodium nitrate solution, iron (III) carbonate, lead carbonate, iron (III) hydroxide, sodium hydroxide solution and dilute hydrochloric acid.

The salts are :
(i) sodium chloride.
(ii) lead chloride.
(iii) anhydrous iron (III) chloride.

Q 7(c) All ammonium salts are decomposed on heating. What other property do ammonium salts have in common?

Chemistry - 1997( I.C.S.E)
You are on questions 1 to 2 of Set II

Section -A

-Answers to this paper must be written on the paper provided separately.
-You will NOT be allowed to write during the first 15 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 answer.

-This question paper is divided into two sections.
- Section I contains one question with eight parts (a) to (h): all eight parts to be answered. Section II  contains six questions, numbered 2 to 7. You are to answer four of these questions.
-The intended marks for questions or parts of questions are given in [].
-All working, including rough work, should be done on the same sheet as the rest of the answers.

Q 1 (a) Name one element, in each case, to which the following descriptions could  apply: (i) the molten metal which gives white fumes when reacting with chlorine; (ii) the burning metal which combines directly with nitrogen; (iii) the metal which directly combines with sulphur on heating; (iv) the non-metal which forms two compounds when reacting with chlorine. Q 1 (b) Name the gas that you can obtain in the laboratory from each of the following and write the equation for the reaction taking place in each case: (i) ammonium nitrite; (ii) ammonium chloride; (iii) ammonium nitrate. Q 1(c) (i) Name the two crystalline allotropes of sulphur. For each allotrope give a sketch of the shape of its crystals.    (ii) Which sulphur allotrope is stable at room temperature ? Q 1(d) (i) What is the mass of nitrogen in 1000 kg of Urea[CO(NH2)2] ? (Answer correct to the nearest kg.) (H=1;C=12;N=14;O=16) (ii) Is it possible to change the temperature and pressure of a fixed mass of gas without changing its volume ? Explain your answer. Q 1(e) (i) What should be the physical state of lead bromide if it is to conduct electricity? (ii) What particles are  present in pure lead bromide? (iii) Write the equation for the reaction which take place at the electrodes during the electrolysis of lead bromide. Q 1(f)Three test-tubes contain calcium nitrate solution , zinc nitrate solution and lead nitrate solution respectively. Each solution is divided into two portions (f) (i) and (f) (ii). Describe the effect of : (i) adding sodium hydroxide solution to each portion in turn till it is in excess. (ii) adding ammonium hydroxide to each portion in turn till it is in excess. Q 1(g) State three tests by which you could identify a gas as being chlorine. Q 1(h) Define or explain the meaning of the following terms : (i) Molar volume; (ii) Fixation of nitrogen; (iii) Acid salt; (iv) Vulcanisation; (v) Ore.                                              Section -II(40 marks)                                   Answer any four questions            Q 2(a) (i) What is the purpose of the pH scale? (ii) What is the pH of pure water? (iii) A is a soluble acidic oxide; B is a soluble base. Compared to the pH of pure water, what will be the pH of : (1) a solution of A  (2) a solution of B? Q 2(b) Taking sodium carbonate as an example, give the meaning of the following terms: (i) Water of crystallization; (ii) anhydrous; (iii) efflorescence. Q 2(c) (i) Barium chloride solution can be used to distinguish between a sodium sulphate solution and a sodium nitrate solution. How is this done? (ii) Write the equation for the action of heat on sodium nitrate.

Q 3 (a)Write equations for the following reactions:
(i) burning of ammonia in oxygen;
(ii) catalytic  oxidation of ammonia.

Q 3 (b)(i) What would you see in(a)(i) above?
(ii) Name the catalyst used in(a)(ii).
(iii) In the reaction referred to in (a)(ii) the catalyst glows red hot. Why?
(iv) What is the name of the industrial process which starts with the reaction referred to in (a)(ii)?

Q 3(c) (i) How soluble is ammonia in water?
(ii) Give two reasons to show that the solution of ammonia in water contains hydroxide ions.
(iii) Name a simple method you would employ  to prepare ammonium salt in your laboratory.

Q 4(b)The empirical formula of a compound is C₂H₅. It has a vapour density of 29. Determine the relative molecular mass of the compound and hence its molecular formula.

Q 4(c) Solid ammonium dichromate (relative molecular mass = 252) decomposes according to the following equation:
(NH₄)₂Cr₂O₇®  N₂ + Cr₂O₃ + 4H₂O
(i) What volume of nitrogen, at STP will be evolved when 63g of ammonium dichromate is decomposed?
(ii) If 63g of ammonium dichromate is heated above 100⁰c , what will be the loss of mass? (H=1;N=14;O=16;Cr=52).

Q 5(b)(i) What is the main impurity present in the iron produced in the blast furnace?
(ii) By what chemical process is this impurity removed  in steelmaking?
(iii) What is added to steel to make stainless steel?  

Q 6(b)Write one equation in each case to show the action of sulphur dioxide?
(i) a reducing agent;
(ii) an oxidizing agent;
(iii) an acid anhydride.

Q 6(c)(i) what is the similarity  in the use of sulphur dioxide and chlorine as bleaching agents?
(ii) When chlorine is involved  in bleaching , what is the type of chemical reaction that changes the coloured compound to a colourless one?
(iii) What is the reason  for not using chlorine to bleach wool?

Q7.(a)Outline the steps required to convert hydrogen chloride to anhydrous Iron (III) Chloride. Write the equations for the reactions which take place.


7(b)(i) What are the two steps necessary to change Lead Carbonate into Lead Chloride?
(ii) Give the name of soluble lead salt and write the equation for the action of heat on this salt.
(iii)Write the equation for the preparation of nitric acid from potassium nitrate.