NCERT Solutions Class 10 Science Chapter 1 Chemical Reactions and Equations

Question

NCERT Solution for Class 10 Science Chapter 1 Chemical Reactions and Equations is one of the most important chapters of class 10. Our solution covers all the important topics related to Chemical Reactions and Equations with a detailed explanation that aims to help students to grasp the concepts with complete clarity.

Students can also find solutions for NCERT intext questions, exercises, and back-of-chapter questions. Our NCERT Solutions Class 10 is based on the latest syllabus proposed by the CBSE and designed by a subject matter expert. Chapter 1 Chemical Reactions And Equations Questions and Answers solutions are very helpful in the preparation for exams and securing good marks. It deals with the overall understanding of chemicals, chemical equations, types of chemical reactions such as combination reaction, decomposition reaction, displacement reaction, double displacement reaction, precipitation reaction, neutralization reaction, oxidation, and reduction reaction.

Our NCERT Solutions Class 10 Science Chapter 1 Chemical Reaction and Equations not only help you to understand the Chemical Reaction and Equations but also give you an in-depth analysis of this topic. A thorough understanding of Chemical Reactions and Equations can give you a significant edge over other students. This chapter is so important that 4-5 questions are asked every year. Good command and ample practice in such topic-related questions provided by our NCERT solutions would be the best way to score full marks in your examination. NCERT in-text questions are also provided which is very helpful in solving the question, revision, completing your homework and assignment on time in the comfort of your home.

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Answer 1

Chapter 1

Chemical Reactions and Equations

Class X

EXERCISE SOLUTION

Question 1:

Which of the statements about the reaction below are incorrect?

(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 1:

(i)(a) and (b)

Question 2:

The above reaction is an example of a

(a) combination reaction.

(b) double displacement reaction.

(c) decomposition reaction.

(d) displacement reaction.

Answer 2:

(d) The given reaction is an example of a 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.

Answer 3:

(a) Hydrogen gas and iron chloride are produced. The reaction is as follows:

Question 4:

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

Answer 4:

A reaction which has an equal number of atoms of all the elements on both sides of the chemical equation is called a balanced chemical equation. The law of conservation of mass states that mass can neither be created nor destroyed. Hence, in a chemical reaction, the total mass of reactants should be equal to the total mass of the products. It means that the total number of atoms of each element should be equal on both sides of a chemical equation. Hence, it is for this reason that chemical equations should be balanced.

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.

Answer 5:

(a) 3H₂(g) + N₂(g) → 2NH₃(g)

(b) 2H₂S(g) + 3O₂(g) → 2H₂O(l) + 2SO₂(g)

(c) 3BaCl₂(aq) + Al₂(SO₄)₃(aq) → 2AlCl₃(aq) + 3BaSO₄(s)

(d) 2K(s) + 2H₂O(l) → 2KOH(aq) + H₂(g)

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 6:

(a) 2HNO₃ + Ca(OH)₂ → NaSO₄ + 2H₂O

(b) 2HaOH + 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

Answer 7:

(a) Ca(OH)₂ + CO₂ → CaCO₃ + H₂O

(b) Zn + 2AgNO₃ → Zn(NO₃)₂ + 2Ag

(c) 2Al + 3CuCl₂ → 2AlCl₃ + 3Cu

(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 bromide(s)

(b) Zinc carbonate (s) → Zinc oxide (s) + Carbon dioxide (g)

(c) Hydrogen (g) + Chlorine (g) → Hydrogen chloride (g)

(d) Magnesium (s) + Hydrochloric acid (aq) → Magnesium chloride (aq) + Hydrogen (g)

Question 9:

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

Answer 9:

Chemical reactions that release energy in the form of heat, light, or sound are called exothermic reactions.

Example: Mixture of sodium and chlorine to yield table salt

Na(s) + 1/2Cl₂(s) → NaCl(s) + 411 kJ of energy

In other words, combination reactions are exothermic. Reactions that absorb energy or require energy in order to proceed are called endothermic reactions.

For example: In the process of photosynthesis, plants use the energy from the sun to convert carbon dioxide and water to glucose and oxygen.

6CO₂(g) + 6H₂O(l) ^_(sunlight)→ C₆H₁₂O₆(aq) (Glucose) + 6O2(g) 

Question 10:

Why is respiration considered an exothermic reaction? Explain.

Answer 10:

Energy is required to support life. Energy in our body is obtained from the food we eat. During digestion, large molecules of food are broken down into simpler substances such as glucose. Glucose combines with oxygen in the cells and provides energy. The special name of this combustion reaction is respiration. Since energy is released in the whole process, it is an exothermic process.

C₆H₁₂O₆(aq) (Glucose) + 6O₂(g) _(Oxygen) → 6CO₂(g) (Carbon dioxide) + 6H₂O(l) (Water) + Energy 

Question 11:

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

Answer 11:

Decomposition reactions are those in which a compound breaks down to form two or more substances. These reactions require a source of energy to proceed. Thus, they are the exact opposite of combination reactions in which two or more substances combine to give a new substance with the release of energy.

Decomposition reaction: AB + Energy → A + B

2H₂O(l) ^{_{(Electrolysis)}} → 2H₂(g) + O₂(g)

Combination reaction: A+B → AB + Energy

2H₂(g) + O2(g) → 2H₂O(l) + Energy

Question 12:

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

Answer 12:

(a) Thermal decomposition: 2FeSO₄(s) (Ferrous sulphate) \(\overset{\Delta}{\longrightarrow}\) Fe2O₃(s) (Ferric oxide) + SO₂(g) (Sulphur dioxide) + SO₃(g) (Sulphur trioxide)

(b) Decomposition by light: 2AgCl(s) (Silver chloride) \(\overset{light}{\longrightarrow}\) 2Ag_(s) (Silver) + Cl_2(s) (Chlorine)

(c) Decomposition by electricity: 2Al₂O₃(aq) (Aluminium oxide) \(\overset{electricity}{\longrightarrow}\) 4Al(s) (Aluminium) + 3O₂(g) (Oxygen)

Question 13:

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

Answer 13:

In a displacement reaction, a more reactive element replaces a less reactive element from a compound.

A + BX → AX + B; where A is more reactive than B

In a double displacement reaction, two atoms or a group of atoms switch places to form new compounds.

AB + CD → AD + CB

For example:

Displacement reaction: CuSO₄(aq) + Zn(s) → ZnSO₄(aq) + Cu(s)

Double displacement reaction: NaSO₄(aq) + BaCl₂(aq) → BaSO₄(s) + 2NaCl(aq)

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.

Answer 14:

2AgNO₃(aq) (Silver nitrate) + Cu(s) (Copper) → Cu(NO₃)₂(aq) (Copper nitrate) + 2Ag(s) (Silver)

Answer 2

Question 15:

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

Answer 15:

A reaction in which an insoluble solid (called precipitate) is formed is called a precipitation reaction.

For example: Na2CO2(aq) (Sodium carbonate) + CaCl2(aq) (Calcium chloride) → CaCO3(s) (Calcium carbonate) + 2NaCl(aq) (Sodium chloride)

In this reaction, calcium carbonate is obtained as a precipitate. Hence, it is a precipitation reaction.

Another example of precipitation reaction is:

Na₂SO₄(aq) (Sodium sulphate) + BaCl₂(aq) (Barium chloride) → BaSO₄(s) (Barium sulphate) + 2NaCl(aq) (Sodium chloride)

In this reaction, barium sulphate is obtained as a precipitate.

Question 16:

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

(a) Oxidation

(b) Reduction

Answer 16:

(a) Oxidation is the gain of oxygen.

For example: 

In equation (i), H₂ is oxidized to H₂O and in equation (ii), Cu is oxidised to CuO.

(b) Reduction is the loss of oxygen.

For example:

In equation (i), CO₂ is reduced to CO and in equation (ii), CuO is reduced to Cu.

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.

Answer 17:

‘X’ is copper (Cu) and the black-coloured compound formed is copper oxide (CuO). The equation of the reaction involved in heating copper is given below.

2Cu (Shiny brown in colour) + O2 \(\overset{\Delta}{\longrightarrow}\) 2CuO (Black in colour)

Question 18:

Why do we apply paint on iron articles?

Answer 18:

Iron articles are painted because it prevents them from rusting. When painted, the contact of iron articles from moisture and air is cut off. Hence, rusting is prevented their presence is essential for rusting to take place.

Question 19:

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

Answer 19:

Nitrogen is an inert gas and does not easily react with these substances. On the other hand, oxygen reacts with food substances and makes them rancid. Thus, bags used in packing food items are flushed with nitrogen gas to remove oxygen inside the pack. When oxygen is not present inside the pack, the rancidity of oil and fat containing food items is avoided.

Question 20:

Explain the following terms with one example each.

(a) Corrosion

(b) Rancidity

Answer 20:

(a) Corrosion: Corrosion is defined as a process where materials, usually metals, deteriorate as a result of a chemical reaction with air, moisture, chemicals, etc. For example, iron, in the presence of moisture, reacts with oxygen to form hydrated iron oxide.

4Fe + 3O₂ + nH₂O → 2Fe₂O₃·nH₂O (Hydrated iron oxide)

This hydrated iron oxide is rust.

(b) Rancidity: The process of oxidation of fats and oils that can be easily noticed by the change in taste and smell is known as rancidity. For example, the taste and smell of butter changes when kept for long. Rancidity can be avoided by:

1. Storing food in airtight containers
2. Storing food in refrigerators
3. Adding antioxidants
4. Storing food in an environment of nitrogen 

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Page 6

Question 1:

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

Answer 1:

Magnesium is a very reactive metal like (Na, Ca, etc.). When it is exposed to air it reacts with oxygen to form a layer of magnesium oxide (MgO) on its surface.

Mg (magnesium) + O₂ (Oxygen) → 2MgO (Magnesium Oxide)

This layer of magnesium oxide is quite stable and prevents further reaction of magnesium with oxygen. The magnesium ribbon is cleaned with sandpaper to remove this layer so that the underlying metal can be used for the reaction.

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

Answer 2:

1. H₂ (Hydrogen) + Cl₂ (Chlorine) → 2HCl (Hydrogen chloride)
2. 3BaCl₂ (Barium Chloride) + Al2(SO₄)₃ (Aluminium Sulphate) → 3BaSO4 (Barium Sulphate) + 2AlCl₃ (Aluminium Chloride)
3. 2Na (sodium) + 2H₂O (water) → 2NaOH (Sodium Hydroxide) + H₂ (Hydrogen)

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.

Answer 3:

(i). BaCl₂(aq) (Barium chloride) + Na₂SO₄(aq) Sodium Sulphate) → BaSO₄(s) (Barium Sulphate) + 2NaCl(aq) (Sodium chloride)

(ii). NaOH(aq) (Sodium Hydroxide) + HCl(aq) (Hydrochloric Acid) → NaCl(aq) (Sodium Chloride) + H₂O(l) (Water)

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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 1:

(i). The substance ‘X’ is calcium oxide. Its chemical formula is CaO.

(ii). Calcium oxide reacts vigorously with water to form calcium hydroxide (slaked lime)

CaO (Calcium Oxide/Quick Lime) + H₂O (Water) → Ca(OH)₂ (Calcium Hydroxide/Sladed Lime) 

Question 2:

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

Answer 2:

During the Electrolysis of water, hydrogen and oxygen is get separated by the electricity. Water (H₂O) contains two parts hydrogen and one part oxygen. Since hydrogen goes to one test tube and oxygen goes to another, the amount of gas collected in one of the test tubes is double the amount collected in the other.

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Page 13

Question 1:

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

Answer 1:

When an iron nail is dipped in a copper sulphate solution, iron (which is more reactive than copper) displaces copper from copper sulphate solution forming iron sulphate, which is green in colour.

CuSO₄(Copper Suphate/ Blue Colour) + Fe (Iron) → FeSO₄ (Iron Sulphate/ Green colour) + Cu (Copper)

Therefore, the blue colour of the copper sulphate solution fades and green colour appears.

Question 2:

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

Answer 2:

Sodium carbonate reacts with calcium chloride to form calcium carbonate and sodium chloride.

Na₂CO₃ (Sodium Carbonate) + CaCl₂ (Calcium Chloride) → CaCO₃ (Calcium Carbonate) + 2NaCl(Sodium Chloride)

In this reaction, sodium carbonate and calcium chloride exchange ions to form two new compounds. Hence, it is a double displacement reaction.

Question 3:

Identify the substances that are oxidised and the substances that are reduced in the following reactions.

(i) 4Na(s) + O₂(g) → 2Na₂O(s)

(ii) CuO(s) + H₂(g) → Cu(s) + H₂O(l)

Answer 3:

(i). Sodium (Na) is oxidised as it gains oxygen and oxygen gets reduced.

(ii). Copper oxide (CuO) is reduced to copper (Cu) while hydrogen (H₂) gets oxidised to water (H₂O).