Lakhmir Singh & Manjit Kaur - Chemistry

Book: Lakhmir Singh & Manjit Kaur - Chemistry

Chapter: 1. Chemical Reations and Equations

Subject: Chemistry - Class 10th

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Chapter Exercises

Very Short Answer Type Questions-Pg-18
Short Answer Type Questions-Pg-19
Long Answer Type Questions-Pg-20
Multiple Choice Questions (MCQs)-Pg-21
Questions Based on High Order Thinking Skills (HOTS)-Pg-22
Very Short Answer Type Questions-Pg-45
Short Answer Type Questions-Pg-46
Long Answer Type Questions-Pg-48
Multiple Choice Questions (MCQs)-Pg-48
Questions Based on High Order Thinking Skills (HOTS)-Pg-49

Very Short Answer Type Questions-Pg-18

1 Why is respiration considered an exothermic process?
2 On what basis is a chemical equation balanced?
3 What happens chemically when quicklime is added to water filled in a bucket?
4 Why should magnesium ribbon be cleaned before burning in air?
5 State whether the following statement is true or false:

A chemical equation can be balanced easily by altering the formula of a reactant or product.
6 What is wrong with the following chemical equation?

Mg + 0 MgO


Correct and balance it.
7 What does the symbol (aq) represent in a chemical equation?
8 Why is photosynthesis considered an endothermic reaction?
9

How will you indicate the following effects in a chemical equation?


(a) A solution made in water


 


(b) Exothermic reaction


 


(c) Endothermic reaction
10 Translate the following statements into chemical equations and then balance the equations :

(a) Hydrogen sulphide gas bums in air to give water and sulphur dioxide.


(b) Phosphorus bums in oxygen to give phosphorus pentoxide.


(c) Carbon disulphide bums in air to give carbon dioxide and sulphur dioxide.


(d) Aluminium metal replaces iron from ferric oxide, Fe203, giving aluminium oxide and iron.


(e) Bi:uiurn chloride reacts with zinc sulphate to give zinc chloride and barium sulphate.
11 Write the balanced chemical equations for the following reactions:

(a) Calcium hydroxide + Carbon dioxide Calcium carbonate + Water


(b) Aluminium + Copper chloride Aluminium chloride + Copper
12 Complete and balance the following equations:

(a) NaOH +....... Na2S04 + H20


(b) Ca(OH)2 +.... CaC03 + H20
13 Correct and balance the following equations:

(i) Ca + H20 CaOH + H


(ii) N + H NH3
14 Write complete balanced equations for the following reactions:

(a) Calcium (solid) +Water (liquid) Calcium hydroxide (solution) +Hydrogen (gas)


(b) Sulphur dioxide (gas)+ Oxygen (gas)Sulphur trioxide (gas)
15 Balance the following equations:

(i) Na + 02 Na20


(ii) H202H20 + 02


(iii) Mg(OH)2 +HCl MgCl2+ H20


(iv) Fe +02Fe203


(v) Al(OH)3Al203 + H20


(vi) NH3 + CuO Cu +N2+ H20


(vii) Al2(S04)3 + NaOH Al(OH)3 + Na2S04


(viii) HN03 +Ca(OH)2Ca(NO3)2 + H2O


(ix) NaOH+H2S04Na2SO4 +H2O


(x) BaCl2+H2S04 BaSO4+ HCl
16 Fill in the following blanks with suitable words:

(a) Chemical equations are balanced to satisfy the law of ........


(b) A solution made in water is known as an ............ solution and indicated by the symbol ..............

Short Answer Type Questions-Pg-19

17 Give one example of a chemical reaction.
17 State two characteristics of the chemical reaction which takes place when dilute sulphuric acid is poured over zinc granules.
17 Give two characteristics of the chemical reaction which occurs on adding potassium iodide solution to lead nitrate solution.
18 What is a chemical equation? Explain with the help of an example.
18 Giving examples, state the difference between balanced and unbalanced chemical equations.
18 Balance the following chemical equations:

(i) NH3 N2 + H2


(ii) C + C02 CO
19 When hydrogen is passed over copper oxide, copper and steam are formed. Write a balanced equation for this reaction and state which of the chemicals are:

(i) elements


(ii) compounds


(iii) reactants


(iv) products


(v) metals


(vi) non-metals
20 What are the various ways in which a chemical equation can be made more informative? Give examples to illustrate your answer.
20 (b) Write balanced chemical equation from the following information:

An aqueous calcium hydroxide solution (lime water) reacts with carbon dioxide gas to produce a solid calcium carbonate precipitate and water.
21 What is a balanced chemical equation? Why should chemical equations be balanced?
21 Aluminium burns in chlorine to form aluminium chloride (AlCl3). Write a balanced chemical equation for this reaction.
21 Potassium metal reacts with water to give potassium hydroxide and hydrogen gas. Write a ba lanced chemical equation for this reaction.
22 Explain, with example, how the physical states of the reactants and products can be shown in a chemical equation.
22 Balance the following equation and add state symbols:

Zn + HCl ZnCl2 + H2
22 Convey the following information in the form of a balanced chemical equation:

"An aqueous solution of ferrous sulphate reacts with an aqueous solution of sodium hydroxide to form a precipitate of ferrous hydroxide and sodium sulphate remains in solution."
23 Write any two observations in an activity which may suggest that a chemical reaction has taken place. Give an example in support of your answer.
24 Aluminium hydroxide reacts with sulphuric acid to form aluminium sulphate and water. Write a balanced equation for this reaction.
24 Balance the following chemical equation :

Mn02 + HCl MnCl2 + Cl2 + H20
25 Write the balanced equations for the following reactions, and add the state symbols :

(a) Magnesium carbonate reacts with hydrochloric acid to produce magnesium chloride, carbon dioxide and water.


(b) Sodium hydroxide reacts with sulphuric acid to produce sodium sulphate and water.
26 Carbon monoxide reacts with hydrogen under certain conditions to form methanol (CH30H). Write a balanced chemical equation for this reaction indicating the physical states of reactants and product as well as the conditions under which this reaction takes place.
27 Potassium chlorate (KC103) on heating forms potassium chloride and oxygen. Write a balanced equation for this reaction and indicate the evolution of gas.
27 (b) Rewrite the following information in the form of a balanced chemical equation : Magnesium burns in carbon dioxide to form magnesium oxide and carbon.
28 Substitute formulae for names and balance the following equation :

Calcium carbonate reacts with hydrochloric acid to produce calcium chloride, water and carbon dioxide gas.
28 (b) Write balanced chemical equation with state symbols for the following reaction:

Sodium hydroxide solution reacts with hydrochloric acid solution to produce sodium chloride solution and water.
29 Ammonia reacts with oxygen to form nitrogen and water. Write a balanced chemical equation for this reaction.

Add the state symbols for all the reactants and products.
30 Write a balanced chemical equation for the process of photosynthesis giving the physical states of all the substances involved and the conditions of the reaction.
31 Translate the following statement into chemical equation and then balance it :

Barium chloride solution reacts with aluminium sulphate solution to form a precipitate of barium sulphate and aluminium chloride solution.
32 When potassium nitrate is heated, it decomposes into potassium nitrite and oxygen. Write a balanced equation for this reaction and add the state symbols of the reactants and products.

Long Answer Type Questions-Pg-20

33 What is meant by a chemical reaction? Explain with the help of an example.
33 Give one example each of a chemical reaction characterised by:

(i) evolution of a gas


(ii) change in colour


(iii) formation of a precipitate


(iv) change in temperature


(v) change in state.
34 State the various characteristics of chemical reactions.
34 State one characteristic each of the chemical reaction which takes place when:

(i) dilute hydrochloric acid is added to sodium carbonate


(ii) lemon juice is added gradually to potassium permanganate solution


(iii) dilute sulphuric acid is added to barium chloride solution


(iv) quicklime is treated with water


(v) wax is burned in the form of a candle
35 What do you understand by exothermic and endothermic reactions?
35 Give one example of an exothermic reaction and one of an endothermic reaction.
35 Which of the following are endothermic reactions and which are exothermic reactions ?

(i) Burning of natural gas


(ii) Photosynthesis


(iii) Electrolysis of water


(iv) Respiration


(v) Decomposition of calcium carbonate

Multiple Choice Questions (MCQs)-Pg-21

36 One of the following does not happen during a chemical reaction. This is:
37 Which of the following does not involve a chemical reaction?
38 You are given the solution of lead nitrate. In order to obtain a yellow precipitate you should mix with it a solution of:
39 An acid which can decolourise purple coloured potassium permanganate solution is:
40 The chemical reaction between two substances is characterised by a change in colour from orange to green.

These two substances are most likely to be:
41 The chemical reaction between quicklime and water is characterised by:
42 One of the following is an endothermic reaction. This is:
43 Which of the following is not an endothermic reaction?
44 One of the following is an exothermic reaction. This is:
45 The chemical equations are balanced to satisfy one of the following laws in chemical reactions. This law is known as:

Questions Based on High Order Thinking Skills (HOTS)-Pg-22

46 When the solution of substance X is added to a solution of potassium iodide, then a yellow solid separates out from the solution.

(a) What do you think substance X is likely to be?


(b) Name the substance which the yellow solid consists of.


(c) Which characteristic of chemical reactions is illustrated by this example ?


(d) Write a balanced chemical equation for the reaction which takes place. Mention the physical states of all the reactants and products involved in the chemical equation.
47 When water is added gradually to a white solid X, a hissing sound is heard and a lot of heat is produced forming a product Y. A suspension of Y in water is applied to the walls of a house during white washing. A clear solution of Y is also used for testing carbon dioxide gas in the laboratory.

(a) What could be solid X? Write its chemical formula.


(b) What could be product Y? Write its chemical formula.


(c) What is the common name of the solution of Y which is used for testing carbon dioxide gas?


(d) Write chemical equation of the reaction which takes place on adding water to solid X.


(e) Which characteristic of chemical reactions is illustrated by this example?
48 When metal X is treated with a dilute acid Y, then a gas Z is evolved which bums readily by making a little explosion.

(a) Name any two metals which can behave like metal X.


(b) Name any two acids which can behave like acid Y.


(c) Name the gas Z.


(d) Is the gas Z lighter than or heavier than air?


(e) Is the reaction between metal X and dilute acid Y exothermic or endothermic?


(f) By taking a specific example of metal X and dilute acid Y, write a balanced chemical equation for the reaction which takes place. Also indicate physical states of all the reactants and products.
49 A solid substance P which is very hard is used in the construction of many buildings, especially flooring. When substance P is heated strongly, it decomposes to form another solid Q and a gas R is given out. Solid Q reacts with water with the release of a lot of heat to form a substance S. When gas R is passed into a clear solution of substance S, then a white precipitate of substance T is formed. The substance T has the same chemical composition as starting substance P.

(a) What is substance P? Write its common name as well as chemical formula.


(b) What is substance Q?


(c) What is gas R?


(d) What is substances? What is its clear solution known as?


(e) What is substance T? Name any two natural forms in which substance T occurs in nature.
50 A silvery-white metal X taken in the form of ribbon, when ignited, burns in air with a dazzling white flame to form a white powder Y. When water is added to powder Y, it dissolves partially to form another substances.

(a) What could metal X be?


(b) What is powder Y?


(c) With which substance metal X combines to form powder Y?


(d) What is substance Z? Name one domestic use of substance Z.


(e) Write a balanced chemical equation of the reaction which takes place when metal X burns in air to form powder Y.
51 A metal X forms a salt XS04. The salt XS04 forms a clear solution in water which reacts with sodium hydroxide solution to form a blue precipitate Y. Metal X is used in making electric wires and alloys like brass.

(a) What do you think metal X could be?


(b) Write the name, formula and colour of salt X S04


(c) What is the blue precipitate Y?


(d) Write a chemical equation of the reaction which takes place when salt XS04 reacts with sodium hydroxide solution. Give the state symbols of all the reactants and products which occur in the above equation.
52 The metal M reacts vigorously with water to form a solution S and a gas G. The solution S turns red litmus to blue whereas gas G, which is lighter than air, burns with a pop sound. Metal M has a low melting point and it is used as a coolant in nuclear reactors.

(a) What is metal M?


(b) What is solution S? Is it acidic or alkaline?


(c) What is gas G?


(d) Write a balanced chemical equation for the reaction which takes place when metal M reacts with water.


(e) Is this reaction exothermic or endothermic?
53 When a mixture of gases X and Y is compressed to 300 atm. pressure and then passed over a catalyst consisting of a mixture of zinc oxide and chromium oxide (heated to a temperature of 300 �C), then an organic compound Z having the molecular formula CH40 is formed. X is a highly poisonous gas which is formed in appreciable amounts when a fuel burns in a limited supply of air; Y is a gas which can be made by the action of a dilute acid on an active metal; and Z is a liquid organic compound which can react with sodium metal to produce hydrogen gas.

(a) What are X, Y and Z?


(b) Write a balanced chemical equation of the reaction which takes place when X and Y combine to form Z. Indicate the conditions under which the reaction occurs.
54 The white solid compound A decomposes quite rapidly on heating in the presence of a black substance X to form a solid compound B and a gas C. When an aqueous solution of compound B is reacted with silver nitrate solution, then a white precipitate of silver chloride is obtained along with potassium nitrate solution. Gas C does not burn itself but helps burn other things.

(a) What is compound A?


(b) What is compound B?


(c) What is gas C?


(d) What do you think is the black substance X? What is its function?


(e) What is the general name of substances like X?
55 Gas A, which is the major cause of global warming, combines with hydrogen oxide B in nature in the presence of an environmental factor C and a green material D to form a six carbon organic compound E and a gas F. The gas F is necessary for breathing.

(a) What is gas A?


(b) What is the common name of B?


(c) What do you think could be C?


(d) What is material D? Where is it found?


(e) Name the organic compound E.


(f) What is gas F? Name the natural process during which it is released?

Very Short Answer Type Questions-Pg-45

1 What type of reaction is represented by the digestion of food in our body?
2 Name the various types of chemical reactions.
3 Why does the colour of copper sulphate solution change when an iron nail is kept immersed in it ?
4 Write the balanced chemical equation for the following reaction :

Zinc + Silver nitrate Zinc nitrate + Silver
5 Which term is used to indicate the development of unpleasant smell and taste in fat and oil containing foods due to aerial oxidation (when they are kept exposed for a considerable time)?
6 What is the general name of the chemicals which are added to fat and oil containing foods to prevent the development of rancidity?
7 State an important use of decomposition reactions.
8 What are anti-oxidants? Why are they added to fat and oil containing foods?
9 Explain why, food products containing fats and oils (like potato chips) are packaged in nitrogen.
10 Give one example of a decomposition reaction which is carried out:

(a) with electricity


(b) by applying heat
11 What type of chemical reaction is used to extract metals from their naturally occurring compounds like oxides or chlorides?
12 Name two anti-oxidants which are usually added to fat and oil containing foods to prevent rancidity.
13 Write one equation each for the decomposition reactions where energy is supplied in the form of (a) heat, (b) light, and(c) electricity.
14 In the refining of silver, the recovery of silver from silver nitrate solution involved displacement by copper metal. Write down the chemical equation of the reaction involved.
16 What type of reactions are represented by the following equations ?

(i) CaC03CaO + CO2


(ii) CaO + H2OCa(OH)2


(iii) 2FeSO4Fe2O3 + SO2 + SO3


(iv) NH4CINH3 + HCl


(v) 2Ca + O22CaO
16 What type of chemical reactions take place when:

(a) a magnesium wire is burnt in air?


(b) lime-stone is heated?


(c) silver bromide is exposed to sunlight


(d) electricity is passed through water?


(e)ammonia and hydrogen chloride are mixed?
17 What type of chemical reactions are represented by the following equations?

(i) A + BCAC + B


(ii) A + B C


(iii) X Y + Z


(iv) PQ + RS PS + RQ


(v) A203 + 2B B203 + 2A
18 Balance the following chemical equations:

(a)


(b)

19 Which of the following is a combination and which is a displacement reaction?

(a)


(b)

20 What type of reactions are represented by the following equations?

(a)


(b)


(c)


(d)


(e)

21 In the following reaction between lead sulphide and hydrogen peroxide :


(a) Which substance is reduced?


(b) Which substance is oxidised?
22 Identify the component oxidised in the following reaction:
23 When S02 gas is passed through saturated solution of H2S, the following reaction occurs :


In this reaction, which substance is oxidized and which one is reduced?
24 Fill in the following blanks with suitable words:

(a) The addition of oxygen to a substance is called ......... whereas removal of oxygen is called.........


(b) The addition of hydrogen to a substance is called ......... whereas removal of hydrogen is called.........


(c) Anti-oxidants are often added to fat containing foods to prevent ..........due to oxidation.

Short Answer Type Questions-Pg-46

25 What is an oxidation reaction? Identify in the following reaction

(i) the substance oxidised, and


(ii) the substance reduced:
26 (a) What is a redox reaction? Explain with an example.

(b) When a magnesium ribbon burns in air with a dazzling flame and forms a white ash, is magnesium oxidized or reduced? Why?


(c) In the reaction represented by the equation:



(i) name the substance oxidised.


(ii) name the oxidising agent.


(iii) name the substance reduced.


(iv) name the reducing agent.
27 (a) Define a combination reaction.

(b) Give one example of a combination reaction which is also exothermic.


(c) Give one example of a combination reaction which is also endothermic.
28 (a) Give an example of an oxidation reaction.

(b) Is oxidation an exothermic or an endothermic reaction?


(c) Explain, by giving an example, how oxidation and reduction proceed side by side.
29 (a) What is the colour of ferrous sulphate crystals? How does this colour change after heating?

(b) Name the product formed on strongly heating ferrous sulphate crystals. What type of chemical reaction occurs in this change?
30 What is a decomposition reaction? Give an example of a decomposition reaction. Describe an activity to illustrate such a reaction by heating.
31 Zinc oxide reacts with carbon, on heating, to form zinc metal and carbon monoxide. Write a balanced chemical equation agent, and

(i) Oxidising agent


(ii) reducing agent, in this reaction.
32 Give one example of a oxidation -reduction reaction which is also:

(a) a combination reaction


(b) a displacement reaction
33 What is the difference between displacement and double displacement reactions ? Write equations for these reactions.
33 What do you mean by a precipitation reaction? Explain giving an example.
34 Explain the following in terms of gain or loss of oxygen with one example each:

(i) oxidation (ii) reduction
34 When copper powder is heated strongly in air, it forms copper oxide. Write a balanced chemical equation for this reaction. Name (i) substance oxidised, and (ii) substance reduced.
35 Define the following in terms of gain or loss of hydrogen with one example each:

(i) oxidation (ii) reduction
35 When a magnesium ribbon is heated, it burns in air to form magnesium oxide. Write a balanced chemical equation for this reaction. Name (i) substance oxidised, and (ii) substance reduced.
36 What is meant by

(a) displacement reaction, and


(b) double displacement reaction? Explain with the help of one example each.
37 Why are decomposition reactions called the opposite of combination reactions? Explain with equations of these reactions.
37 Express the following facts in the form of a balanced chemical equation:

"When a strip of copper metal is placed in a solution of silver nitrate, metallic silver is precipitated and a solution containing copper nitrate is formed".
38 What happens when a piece of iron metal is placed in copper sulphate solution? Name the type of reaction involved.
38 Write balanced chemical equation with state symbols for the following reaction:

Barium chloride solution reacts with sodium sulphate solution to give insoluble barium sulphate and a solution of sodium chloride.
39 In the reaction represented by the following equation:


(a) name the substance oxidized


(b) name the substance reduced


(c) name the oxidizing agent


(d) name the reducing agent
40 What happens when silver nitrate solution is added to sodium chloride solution?

(a) Write the equation for the reaction which takes place.


(b) Name the type of reaction involved.
41 What happens when silver chloride is exposed to sunlight? Write a chemical equation for this reaction. Also give one use of such a reaction.
42 What happens when a zinc strip is dipped into a copper sulphate solution ?

(a) Write the equation for the reaction that takes place.


(b) Name the type of reaction involved.

Long Answer Type Questions-Pg-48

43 Explain the term "corrosion" with an example. Write a chemical equation to show the process of corrosion of iron.
43 What special name is given to the corrosion of iron?
43 What type of chemical reaction is involved in the corrosion of iron?
43 Name any three objects (or structures) which are gradually damaged by the corrosion of iron and steel.
44 Explain the term "rancidity". What damage is caused by rancidity?
44 What type of chemical reaction is responsible for causing rancidity?
44 State and explain the various methods for preventing or retarding rancidity of food.
45 What happens when an aqueous solution of sodium sulphate reacts with an aqueous solution of barium chloride?
45 Write the balanced chemical equation for the reaction which takes place.
45 State the physical conditions of reactants in which the reaction will not take place.
45 Name the type of chemical reaction which occurs.
45 Give one example of another reaction which is of the same type as the above reaction.

Multiple Choice Questions (MCQs)-Pg-48

46 The removal of oxygen from a substance is called:
47 In the context of redox reactions, the removal of hydrogen from a substance is known as:
48 The chemical reaction involved in the corrosion of iron metal is that of :
49 The term used to indicate the development of unpleasant smell and taste in fat and oil containing foods due to aerial oxidation is:
50 In order to prevent the spoilage of potato chips, they are packed in plastic bags in an atmosphere of :
51 A white precipitate can be obtained by adding dilute sulphuric acid to:
52 A white precipitate will be formed if we add common salt solution to:
53 Consider the following equation of the chemical reaction of a metal M:


This equation represents:
54 The process of respiration is:
55 Which of the following can be decomposed by the action of light?
56 Consider the reaction:


This is an example of:
57 You are given the following chemical equation:

Mg (s) + CuO (s) → MgO (s)+ Cu(s)


This equation represents:

Questions Based on High Order Thinking Skills (HOTS)-Pg-49

58 When a green iron salt is heated strongly, its colour finally changes to brown and odor of burning sulphur is given out.

(a) Name the iron salt.


(b) Name the type of reaction that takes place during the heating of iron salt.


(c) Write a chemical equation for reaction involved.
59 A colourless lead salt, when heated, produces a yellow residue and brown fumes.

(a) Name the lead salt.


(b) Name the brown fumes.


(c) Write a chemical equation of the reaction involved.
60 When hydrogen burns in oxygen, water is formed and when water is electrolysed, then hydrogen and oxygen are produced. What type of reaction takes place:

(a) in the first case?


(b) in the second case?
61 A strip of metal X is dipped in a blue coloured salt solution YSO4. After some time, a layer of metal Y form the salt solution is formed on the surface of metal strip X. Metal X is used in galvanization whereas metal Y is used in making electric wires. Metal X and metal Y together form an alloy Z.

(a) What could metal X be?


(b) What could metal Y be?


(c) Name the metal salt YSO4.


(d) What type of chemical reaction takes place when metal X reacts with salt solution YSO4? Write the equation of the chemical reaction involved.


(e) Name the alloy Z.
62 When a black metal compound XO is heated with a colourless gas Y2, then metal X and another compound Y2O are formed. Metal X is red-brown in colour which does not react with dilute acids at all. Gas Y2 can be prepared by the action of a dilute acid on any active metal. The compound Y2O is a liquid at room temperature which can turn anhydrous copper sulphate blue.

(a) What do you think is metal X?


(b) What could be gas Y2?


(c) What is compound XO?


(d) What is compound Y2O?


(e) Write the chemical equation of the reaction which takes place on heating XO with Y2.


(f) What type of chemical equation of the reaction which takes place on heating XO with Y2.
63 A metal X forms a water soluble salt XNO3. When an aqueous solution of XNO3 is added to common salt solution, then a white precipitate of compound Y is formed along with sodium nitrate solution. Metal X is said to be the best conductor of electricity and it does not evolve hydrogen when put in dilute hydrochloric acid.

(a) What is metal X?


(b) What is salt XNO3?


(c) Name the compound Y.


(d) Write the chemical equation of the reaction which takes place on reacting XN03 solution and common salt solution giving the physical states of all the reactants and products.


(e) What type of chemical reaction is illustrated by the above equation?
64 Two metals X and Y form the salts XSO4 and Y2SO4, respectively. The solution of salt XSO4 is blue in colour whereas that of Y2SO4, is colourless. When barium chloride solution is added to XSO4 solution, then a white precipitate Z is formed along with a salt which turns the solution green. And when barium chloride solution is added to Y2SO4, solution, then the same white precipitate Z is formed along with colourless common salt solution.

(a) What could the metals X and Y be?


(b) Write the name and formula of salt XS04.


(c) Write the name and formula of salt Y2S04


(d) What is the name and formula of white precipitate Z?


(e) Write the name and formula of the salt which turns the solution green in the first case.
65 A red-brown metal X forms a salt XSO4. When hydrogen sulphide gas is passed through an aqueous solution of XSO4, then a black precipitate of XS is formed along with sulphuric acid solution.

(a) What could the salt xso4 be?


(b) What is the colour of salt XSO4?


(c) Name the black precipitate XS.


(d) By using the formula of the salt obtained in (a) above, write an equation of the reaction which takes place when hydrogen sulphide gas is passed through its aqueous solution.


(e)What type of chemical reaction takes place in this case?
66 When a strip of red-brown metal X is placed in a colourless salt solution YNO3 then metal Y is set free and a blue coloured salt solution XNO3H is formed. The liberated metal Y forms a shining white deposit on the strip of metal X.

(a) What do you think metal X is?


(b) Name the salt YNO3.


(c) What could be metal Y?


(d) Name the salt X(NO3)2.


(e) What type of reaction takes place between metal X and salt solution YNO3?
67 A metal salt MX when exposed to light splits up to form metal M and a gas X2. Metal M is used in making ornaments whereas gas X2 is used in making bleaching powder. The salt MX is itself used in black and white photography.

(a) What do you think metal M is?


(b) What could be gas X2?


(c) Name the metal salt MX.


(d) Name any two salt solutions which on mixing together can produce a precipitate of salt MX.


(e) What type of chemical reaction takes place when salt MX is exposed to light? Write the equation of the reaction.