NCERT Solutions for Class 10 Science Chapter 1 Chemical reactions and equations

NCERT Solutions for Class 10 Science Chapter 1 Chemical reactions and equations

NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and equations We have provided class 10 science NCERT Solutions for Chapter 1 Chemical Reactions and Equations

NCERT Solutions for Class 10 Science Chapter 1 Intext Questions

Page Number: 6

Question 1 Why should a magnesium ribbon be cleaned before burning in air ?


Magnesium ribbon should be cleaned before burning in the air because Magnesium gets covered with a layer of magnesium oxide when kept in the air for a long time. This layer hinders the burning of magnesium. Hence, it is to be cleaned before burning.

Question 2 Write the balanced equation for the following chemical reactions.
(i) Hydrogen + Chlorine → Hydrogen chloride
(ii) Barium chloride + Aluminium sulphate → Barium sulphate + Aluminium chloride
(iii) Sodium + Water → Sodium hydroxide + Hydrogen


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


i) BaCl+ Na2SO→ BaSO+ 2NaCl

ii) NaOH + HCl → NaCl + H2O

Page Number: 10

Question 1
A solution of a substance ‘X’ is used for white washing.
(i) Name the substance ‘X’ and write its formula.
(ii) Write the reaction of the substance ‘X’ named in (i) above with water.


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 textbook Activity 1.7 (i.e., electrolysis of water) double of the amount collected in the other? Name this gas. 


In Activity 1.7, water is electrolysed to give H2 gas at one electrode and O2 gas at the other electrode.
2H2O(l) → 2H2(g) + O2(g)
Thus two molecules of water on electrolysis give two molecules of hydrogen gas and one molecule of oxygen gas or in other words, the amount of hydrogen gas collected would be double that of oxygen gas.

Page Number: 13

Question 1
Why does the colour of copper sulphate solution change when an iron nail is dipped in it ?


When an iron nail is 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.

Fe + CuSO4 → FeSO4 + Cu

Question 2
Give an example of a double displacement reaction other than the one given in Activity 1.10


Sodium sulphate and barium chloride undergo double displacement and form barium sulphate and sodium chloride.

Na2SO4 (aq)+ BaCl2(aq) —> BaSO4(white ppt.) + 2NaCl(aq)

Question 3
Identify the substances that are oxidised and the substances which are reduced in the following reactions.
(i) 4Na(s) + O2(g) → 2Na2O(s)
(ii) CuO (s) + H2(g) → Cu (s) + H2O(l) 


(i) The Sodium (Na) is getting oxidized with the addition of Oxygen (O2).
(ii) the Copper (Cu) is reduced due to the addition of Hydrogen (H2).

NCERT Solutions for Class 10 Science Chapter 1 NCERT Questions

Question 1
Which of the statements about the reaction below are incorrect?
2 PbO(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


(i) (a) and (b)

Explanation: (a) Because Oxygen is being removed and (b) Because the removed oxygen from Lead is added to the Carbon.

Question 2
Fe2O3 + 2Al → Al2O3 + 2Fe
The above reaction is an example of a
(a) combination reaction
(b) double displacement reaction
(c) decomposition reaction
(d) displacement reaction


d) Displacement reaction.

Question 3
What happens when dilute hydrochloric acid is added to iron filings? 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.


a) Hydrogen gas and Iron chloride are produced.

Question 4
What is a balanced chemical equation? Why should chemical equations be balanced?


A balanced chemical equation has an equal number of atoms of different elements in the reactants and products. The chemical equations should be balanced to satisfy the law of conservation of mass.

Question 5
Translate the following statements into chemical equations and then 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.


(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


(a) 2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H2O
(b) 2NaOH + H2SO4 → Na2SO4 + 2H2O
(c) NaCl + AgNO3 → AgCl + NaNO3
(d) BaCl2 + H2SO4 → BaSO4 + 2HCl

Question 7
Write the balanced chemical equations for the following reactions :
(a) Calcium hydroxide + Carbon dioxide → Calcium carbonate + Water
(b) Zinc + Silver nitrate → Zinc nitrate + Silver
(c) Aluminium + Copper chloride → Aluminium chloride + Copper
(d) Barium chloride + Potassium sulphate → Barium sulphate + Potassium chloride


(a) Ca (OH)2 + CO2 → CaCO3 + H2O
(b) Zn + 2AgNO3 → Zn(NO3)2 + 2 Ag
(c) 2Al + 3 CuCl2 → 2AlCl3 + 3 Cu
(d) BaCl2 + K2SO4 → BaSO4 + 2KCl

Question 8
Write the balanced chemical equation for the following and identify the type of reaction in each case :
(a) Potassium bromide (aq) + Barium iodide (aq) → Potassium iodide (aq) + Barium
(b) Zinc carbonate(s) → Zinc oxide (s) + Carbon dioxide (g) bromide(s)
(c) Hydrogen (g) + Chloride (g) → Hydrogen chloride (g)
(d) Magnesium (s) + Hydrochloric acid (aq) → Magnesium chloride (aq) + Hydrogen (g)


(a) 2KBr (aq) + Bal2(aq) → 2Kl(aq) + BaBr2(s)
Type: Double displacement reaction

(b) ZnCO3 (s) → ZnO (s) + CO2 (g)
Type: Decomposition reaction

(c) H2 (g) + Cl2 (g) → 2HCl(g)
Type: Combination reaction

(d) Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g)
Type: Displacement reaction

Question 9
What does one mean by exothermic and endothermic reactions? Give examples.


Exothermic reactions: Those reactions in which heat is evolved are known as exothermic reactions.
Example :
(i) C (s) + O2 (g) → CO2 (g) + Heat
(ii) N2 (g) + 3H2 (g) → 2NH3 (g) + Heat

Endothermic reactions: Those reactions in which heat is absorbed are known as endothermic reactions.
Examples :
(i) C (s) + 2S (s) → CS2 (l)
(ii) N2 (g) + O2 (g) → 2NO(g)

Question 10
Why is respiration considered an exothermic reaction? Explain.


Respiration is an exothermic process because during respiration glucose combines with oxygen in the cells of our body to form carbon dioxide and water along with the production of energy.

C6H12O+ 6O→ 6CO+ 6H2O + Energy

Question 11
Why are decomposition reactions called the opposite of combination reactions? Write equations for these reactions.


In a decomposition reaction, a single compound breaks down to produce two or more simpler substances.
For example: CaCO3(s) → CaO(s) + CO2(g)

While, in a combination reaction, two or more substances simply combine to form a new substance.
For example: H2 (g) + Cl2 → 2HCl (g)

Question 12
Write one equation each for the decomposition reactions where energy is supplied in the form of heat, light or electricity.


(a) Thermal decomposition reaction (Thermolysis)

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

2KClO+ Heat → 2KCl + 3O2

(b) Electrolytic decomposition reaction (Electrolysis)

Decomposition of sodium chloride: On passing electricity through molten sodium chloride, it decomposes into sodium and chlorine.

2NaCl + Electricity → 2Na + Cl2

(c) Photodecomposition reaction (Photolysis)

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

2H2O2 + Light → 2H2O

Question 13
What is the difference between displacement and double displacement reactions? Write equations for these reactions.


In displacement reactions, a more reactive metal displaces a less reactive metal from its solution. For example,
Fe(s) + CuSO4(aq) → Cu(s) + FeSO4(aq)
This is a displacement reaction where iron displaces copper from its solution.

In double displacement reactions, two reactants in solution exchange their ions. For example,
AgNO3(aq) + NaCl (aq) → AgCl(s) + NaNO3 (aq)
This is a double displacement reaction where silver nitrate and sodium chloride exchange Cl and NO3 ions between them.

Question 14
In the refining of silver, the recovery of silver from silver nitrate solution involved displacement by copper metal. Write down the reaction involved.


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

Question 15
What do you mean by a precipitation reaction? Explain by giving examples.


A reaction in which an insoluble solid called precipitate is formed that separates from the solution is called a precipitation reaction.

Examples of precipitation reactions are

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 or loss of oxygen with two examples each:
(a) Oxidation and
(b) Reduction.


(a) Oxidation: The addition of oxygen to a substance is called oxidation.
Example :
(i) S(s) + O2(g) → SO2(g) (Addition of oxygen to sulphur)
(ii) 2Mg(s) + O2 (g) → 2MgO(s) (Addition of oxygen to magnesium)

(b) Reduction: The removal of oxygen from a substance is called reduction.
Example :
CuO(s) + H2(g) → Cu(s) + H2O(l)
2HgO → 2Hg + O2

Question 17
A shiny brown coloured element ‘X’ on heating in air becomes black in colour. Name the element ‘X’ and the black-coloured compound formed.


Element ‘X’ is copper (Cu).
The black-coloured compound is copper oxide (CuO). The reaction involved is

2Cu(s) + O2(g) → 2CuO(s)

Question 18
Why do we apply paint on iron articles?


Paint does not allow iron articles to come in contact with air, water and saves iron articles from damage due to rusting.

Question 19
Oil and fat containing food items are flushed with nitrogen. Why ?


To keep food items fresh and save them from getting oxidised, food items are flushed with nitrogen.

Question 20
Explain the following terms with one example each (a) Corrosion, (b) Rancidity.


(a) Corrosion: It is the process in which metals are eaten up gradually by the action of air, moisture or a chemical (such as an acid) on their surface.
Example: When iron is exposed to moist air for a long period of time, its surface acquires a coating of a brown, flaky substance called rust. Rust is mainly hydrated iron (III) oxide [Fe2O3.xH20].

(b) Rancidity: The condition produced by aerial oxidation of fats and oils in foods marked by unpleasant smell and taste is called rancidity.
Rancidity spoils the food materials prepared in fats and oils which have been kept for a considerable time and makes them unfit for eating.

NCERT Solutions for Class 10 Science Chapter 1 Chemical reactions and equations

The topics and subtopics covered in the NCERT Solutions for Class 10 Science Chapter 1 are –
1.1 – Chemical Equations
1.1.1 – Writing a Chemical Equation
1.1.2 – Balanced Chemical Equations
1.2 – Types of Chemical Reactions
1.2.1 – Combination Reaction
1.2.2 – Decomposition Reaction
1.2.3 – Displacement Reaction
1.2.4 – Double Displacement Reaction
1.3 – Have you observed the effects of oxidation reactions in everyday life?
1.3.1 – Corrosion1.3.2 – Rancidity

NCERT Solutions for Class 10 Science

NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations includes all the important topics with a detailed explanation that aims to help students to understand the concepts better. Students can also find NCERT intext, exercises, and back-of-chapter questions. Also working on Class 10 Science Chapter 1 Chemical Reactions and Equations NCERT Solutions will be most helpful to the students to solve their Homework and Assignments.

Class 10 Science Chapter 1 Solutions Students who are preparing for their Class 10 board exams must go through NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations. All Chapter 1 – Chemical Reactions and Equations Exercise Questions with Solutions to help you to revise the complete Syllabus and Score good marks in your board exam.

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Knowledge and good practice will help you score full marks on the questions asked in this chapter.  Learning the fundamentals of Chemistry in CBSE Class 10 is now easy. Class 10 Science Chapter 1 NCERT Solutions NCERT Solutions for Class 10 Science

Chapter 1 of NCERT Solutions for Class 10 Science has good weightage and there will be questions being asked every year from this chapter in this chapter, students learn the basics of chemical reactions, their types and the effects of a chemical oxidation reaction.

Now that we are provided all the necessary information regarding NCERT Solutions for 10 Science Chapter 1 Chemical Reactions and Equations we hope these detailed NCERT Solutions are helpful. Students can also check out NCERT Books, CBSE Syllabus, and CBSE Sample Papers at for free.

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