Solutions-Class-10-CBSE-NCERT-Science-Chapter-1-Chemical Reactions and Equations

Chemical Reactions and Equations



In-text questions (page 6)

Question 1.

Why should a magnesium ribbon be cleaned before burning in air?

Answer :

Magnesium is very reactive metal. When stored it reacts with oxygen to form a layer magnesium oxide on its surface. This layer of magnesium oxide is quite stable and prevents further reaction of magnesium with oxygen. The magnesium ribbon is cleaned by sand paper to remove this layer so that the underlying metal can be exposed into air.

Question 2.

 Write a balanced equation for the following chemical reactions.

(i) Hydrogen + Chloride —> Hydrogen chloride

(ii) Barium chloride + Aluminium sulphate —> Barium sulphate + Aluminium chloride

(iii) Sodium + Water —> Sodium hydroxide + Hydrogen

Answer :

(i) H+ Cl→ 2HCl

(ii) 3BaCl+ Al2(SO4)→ 3BaSO+ 2AlCl

(iii) 2Na + 2H2O → 2NaOH + H2

Question 3.

 Write a balanced chemical equation with state symbols for the following reactions

(i) Solutions of Barium chloride and Sodium sulphate in water react to give insoluble Barium sulphate and solution of Sodium chloride.

(ii) Sodium hydroxide solution in water reacts with hydrochloric acid solution to produce Sodium chloride solution and water.

Answer :

(i) BaCl+ Na2SO→ BaSO+ 2NaCl

(ii) NaOH + HCl → NaCl + H2O

In-text questions (Page 10)

Question 1.

A solution of a substance ‘X’ is used for whitewashing.

(i) Name the substance ‘X’ and write its formula.

(ii) Write the reaction of the substance ‘X’ named in (i) above with water.

Answer :

(i) The substance ‘X’ which is used in whitewashing is quick lime or Calcium Oxide and its formula is CaO.

(ii) CaO + H2O → Ca(OH)2

Question 2.

Why is the amount of gas collected in one of the test tubes in Activity 1.7 double of the amount collected in the other? Name this gas

Answer :

In activity 1.7, gas collected in one of the test tubes is double of the amount collected in the other because water gets hydrolysed to release H2 and O2 gas. Here, after electrolysis two molecules of Hydrogen and one molecule of oxygen gas is released, hence the amount of Hydrogen collected would be double than that of oxygen.

In-text questions (Page 13)

Question 1.

Why does the colour of copper sulphate solution change when an iron nail is dipped in it?

Answer :

When an iron nail dipped in the copper sulphate solution, iron displaces copper from the copper sulphate because iron is more reactive than copper. Therefore the colour of the copper sulphate solution changes. The reaction is:

Question 2.

Give an example of a double displacement reaction other than the one given in Activity 1.10.

Answer :

Reaction Between silver nitrate (AgNO3) and Sodium chloride (NaCl) is an example of double displacement reaction. During the reaction negative and positive ions trade positions as a result in the formation of white silver chloride precipitate. The chemical reaction is given below.

Ag+ + NO3 + Na+ + Cl– → AgCl + Na+ + NO3

Question 3.

Identify the substances that are oxidized and that are reduced in the following equation.

(i) 4Na(s) + O2(g) → 2Na2O(s)

(ii) CuO(s) + H2(g) → Cu(s) + H2O(l)

Answer :

The Sodium (Na) in the first equation is getting oxidized with the addition of Oxygen (O2) and the Copper (Cu) in the second equation is reduced due to the addition of Hydrogen (H2)

Exercise Questions

Question 1.

Which of the statements about the reaction below are incorrect?

2PbO(s) + C(s) 2Pb(s) + CO2(g)

(a) Lead is getting reduced

(b) Carbon Dioxide is getting oxidised

(c) Carbon is getting oxidised

(d) Lead oxide is getting reduced

(i) (a) and (b)   (ii) (a) and (c)   (iii) (a), (b) and (c)  (iv) all

Answer :

 (i) (a) and (b) is incorrect

[(c) and (d) is correct]

Question 2.

  Fe2O+ 2Al Al2O+ 2Fe

The above reaction is an example of a

(a) Combination reaction.

(b) Double displacement reaction.

(c) Decomposition reaction.

(D) Displacement reaction.

Answer :

Answer is (d) Displacement reaction.

Question 3.

 What happens when dilute hydrochloric acid is added to iron fillings? Tick the correct answer.

(a) Hydrogen gas and Iron chloride are produced.

(b) Chlorine gas and Iron hydroxide are produced.

(c) No reaction takes place.

(D) Iron salt and water are produced.

Answer :

Answer is (a) Hydrogen gas and Iron chloride are produced.

Question 4.

What is a balanced chemical equation? Why should a chemical equation be balanced?

Answer :

A balanced equation is the one in which number of different atoms on both the reactant and product sides are equal. Balancing chemical equation is necessary for the reaction should obey The Law of Conservation of energy. Balancing the chemical equation has no defined method and is purely a trial and error attempt.

Question 5.

Translate the following statements into chemical equations and balance them.

(a) Hydrogen gas combines with nitrogen to form ammonia.

(b) Hydrogen sulphide gas burns in air to give water and sulphur dioxide.

(c) Barium chloride reacts with aluminium sulphate to give Aluminium chloride and a precipitate of barium sulphate.

(d) Potassium metal reacts with water to give potassium hydroxide and Hydrogen gas.

Answer :

 (a) Unbalanced: H+ N→ NH3

       Balanced: 3H+ N→ 2NH3

(b) Unbalanced: H2S + O→ H2O + SO2

      Balanced: 2H2S + 3O→ 2H2O + 2SO2

(c)  Unbalanced: BaCl+ Al2(SO4)→ AlCl+ BaSO4

      Balanced: 3BaCl+ Al2(SO4)→ 2AlCl+ 3BaSO4

(d) Unbalanced: K + H2O → KOH + H2

     Balanced:  2K + 2H2O → 2KOH + H2

Question 6.

 Balance the following chemical equations.

(a) HNO3 + Ca(OH)2  Ca(NO3)2 + H2O

(b) NaOH + H2SO4  Na2SO4 + H2O

(c) NaCl + AgNO3  AgCl + NaNO3

(d) BaCl2 + H2SO4  BaSO4 + HCl

Answer :

(a) 2HNO+ Ca(OH)→ Ca(NO3)+ 2H2O

(b) 2NaOH + H2SO→ Na2SO+ 2H2O

(c) NaCl + AgNO→ AgCl + NaNO3

(d) BaCl+ H2SO→ BaSO+ 2HCl

Question 7.

Write the balanced chemical equation for the following reactions.

Calcium hydroxide + Carbon dioxide —-> Calcium carbonate + Water

Zinc + Silver nitrate —-> Zinc nitrate + Silver

Aluminium + Copper chloride —-> Aluminium chloride + Copper

Barium chloride + Potassium sulphate —-> Barium sulphate + Potassium chloride

Answer :

2Ca(OH)+ 2CO→ 2CaCO+ 2H2O

Zn + 2AgNO→ Zn(NO3)+ 2Ag

2Al + 3CuCl→ 2AlCl+ 3Cu

BaCl+ K2SO→ BaSO+ 2KCl

Question 8.

Write a balanced chemical equation for the following and identify the type of reaction of each case

KBr + BaI KI + BaBr2

ZnCO ZnO + CO2

H+ Cl HCl

Mg + HCl MgCl+ H2

Answer :

2KBr + BaI→ 2KI + BaBr2 (Double Displacement Reaction)

ZnCO→ ZnO + CO2 (Decomposition Reaction)

H2 + Cl → 2HCl (Combination Reaction)

Mg + 2HCl → MgCl+ H2 (Displacement Reaction)

Question 9.

What is meant by exothermic and endothermic reactions? Give examples.

Answer :

An endothermic reaction occurs when energy is absorbed from the surroundings in the form of heat.(Example: Photosynthesis, melting of ice, evaporation). Conversely, an exothermic reaction is one in which energy is released from the system into the surroundings. (Example: Explosions, concrete setting, nuclear fission and fusion).

Question 10.

Why is respiration considered to be an exothermic reaction?

Answer :

The food taken by the living beings is ultimately broken down to glucose by the digestive system. The glucose so formed is slowly oxidised to carbon dioxide and water with the release of heat energy. Thus, respiration is an exothermic reaction.

The reaction taking place is:

C6H12O+ 6O→ 6CO+ 6H2O + Energy

Question 11.

Why are decomposition reactions called the opposite of Combination reactions? Write equations for these reactions.

Answer :

Combination reaction is said to be the reaction between two or more molecules to form a larger molecule; whereas the decomposition reaction is defined as the splitting of larger molecules into two or more smaller molecules. This essentially explains that the decomposition reaction is the opposite of the combination reaction.

(i) 2H2 + O2 → 2H2O (Combination)

2H2O \(\underrightarrow{electrolyte}\)   2H2 + O2 (Decomposition)

(ii) CaCO3 + H2O + CO2 → Ca(HCO3)2 (Combination)

Ca(HCO3)2  \(\underrightarrow{Δ}\)   CaCO3 + H2O + CO2 (Decomposition)

Question 12.

Write one equation each for decomposition reactions in which energy is supplied in the form of heat, light or electricity.

Answer :

(i) Thermal decomposition reaction (Thermolysis)

When heated strongly, potassium chlorate decomposes into potassium chloride and oxygen. This reaction is used for the preparation of oxygen.

2KClO \(\underrightarrow{heat}\)  2KCl + 3O2

(ii) Electrolytic decomposition reaction (Electrolysis)

On passing electricity through molten silver chloride, it decomposes into silver and chlorine.

2AgCl(s) \(\underrightarrow{light}\)  2Ag(s) + Cl2(g)

(iii) Photodecomposition reaction (Photolysis)

In the presence of light, hydrogen peroxide decomposes into water and oxygen.

H2​O2​ (l)  \(\underrightarrow{sunlight}\)     H2​O (l) + O2​ (g)

Question 13.  

What is the difference between displacement and double displacement reactions? Write relevant equations for the above.

Answer :

  • A displacement reaction is the one when a more reactive substance displaces a less reactive one from its salt solution whereas a double displacement reaction is the one where a mutual exchange of ions happens between two compounds.
  • In a displacement reaction, only a single displacement takes place whereas in the double displacement reaction, as the name suggests two displacement takes place between the molecules.


Displacement reaction :

Mg + 2HCl → MgCl+ H2 (Here Mg displaces H from HCL)

Double displacement reaction :

2KBr + BaI2 → 2KI + BaBr2 (Here K and Ba displaces each other)

Question 14.

In the refining of Silver, the recovery of silver from Silver nitrate solution involves displacement reaction by Copper metal. Write down the reaction involved.

Answer :

Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s)

Question 15.

What do you mean by a precipitation reaction? Explain by giving examples.

Answer :

When two solutions containing soluble salts are combined, a double displacement reaction takes place in which the ions are exchanged between the compounds. When one of such compounds formed is in solid form (that is insoluble in aqua) then it settles down at the bottom of the container. This solid is known as the precipitate and the respective reaction is termed as the precipitation reaction.

Examples :

CdSO4(aq) + K2S(aq) → CdS(s) ↓ + K2SO4(aq)

2NaOH(aq) + MgCl2(aq) → 2NaCl(aq) + Mg(OH)2(s) ↓

Question 16.

Explain the following in terms of gain of oxygen with two examples each.

(a) Oxidation

(b) Reduction

Answer :

(a) Oxidation : In a chemical reaction, when the oxygen is added to the element to form its respective oxide it is the element being oxidised.


4Na(s) + O2(g) → 2Na2O(s)

H2S + O→ H2O + SO2

(b) Reduction : In a chemical reaction, when the oxygen is being removed from the compound then it is said to be reduced.


CuO(s) + H2(g) → Cu(s) + H2O(l)

2HgO → 2Hg + O2

Question 17.

A shiny brown coloured element ‘X’ on heating in the air becomes black in colour. Name the element ‘X’ and the black coloured compound formed.

Answer :

The shiny brown coloured element is the Copper metal (Cu). When the metal is heated in air, it reacts with atmospheric oxygen to form copper oxide. Hence, the black coloured compound is the copper oxide.

2Cu(s) + O2(g) → 2CuO(s)

Question 18.

Why do we apply paint on iron articles?

Answer :

Iron articles are painted to prevent them from rusting. When left unpainted, the metal surface comes in contact with the atmospheric oxygen and in the presence of moisture it from Iron(III) oxide. But if painted the surface does not come in contact with moisture and air thus preventing Rusting.

Question 19.

Oil and Fat containing food items are flushed with Nitrogen. Why?

Answer :

The main purpose of flushing Nitrogen into food packets that contain oil and fat items is to prevent Rancidity which occurs when the oil or fat reacts with the oxygen letting out an unpleasant smell and taste. Therefore, by flushing Nitrogen, an unreactive surrounding is created thus preventing rancidity.

Question 20.

Explain the following terms with one example each.

(a) Corrosion

(b) Rancidity

Answer :

Corrosion : Corrosion is a process where a refined metal is oxidised by atmospheric oxygen to form a more stable compound such as oxides. The metal gradually degrades during the corrosion process.

Example : Rusting of iron is a good example of corrosion where the iron is converted to Iron oxide.

Rancidity : Rancidity is the condition produced by the aerial oxidation of the oil and fat present in the food material that produces an unpleasant taste and smell.

Example : Smell in old cooking oil is an example of rancidity.

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