NCERT Solutions for Class 10 Science Updated for 2022-23

 

NCERT Solutions for Class 10 Science Chapter 1 – PSEB Term I Download Free PDF

 

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NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations is an outstanding study resource needed for the students studying in CBSE Term I of Class 10. These NCERT Solutions are crafted as per the latest CBSE Syllabus by subject experts at BYJU’S. It is very important for the students to solve and study with the help of the NCERT Solutions to get knowledge of the type of questions asked from the chapter, Chemical reactions and equations.

Chapter 1 of NCERT Solutions for Class 10 Science mainly deals with writing chemical equations, writing and balancing chemical equations. Also, in this chapter, students also learn the basics of chemical reactions, their types and the effects of a chemical oxidation reaction in our daily lives. The NCERT Solutions Class 10 Science Chapter 1 provides an overview of the main concepts in the chapter and helps you to get well versed with important topics such as writing chemical equations and balancing them.

The NCERT Solutions for Class 10 Science Chapter 1 has good weightage and there will be around 4 questions being asked every year from this chapter. The types of questions that appear in this chapter are mostly practice-based questions. Thorough knowledge and good practice will help you score full marks on the questions asked from this chapter.

Access Answers to NCERT Class 10 Science Chapter 1 – Chemical Reactions and Equations

In-text questions set 1 Page number – 6

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

Solution:

Magnesium ribbon should be cleaned before burning in air because Magnesium metal reacts with the atmospheric oxygen and forms Magnesium Oxide (MgO) layer which is a very stable compound. In order to prevent further reactions with Oxygen, it is therefore necessary to clean the ribbon by to remove the layer of MgO.

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

Solution:

i) H₂ + Cl₂ → 2HCl

ii) 3BaCl₂ + Al₂(SO₄)₃ →3BaSO₄ + 2AlCl₃ 

iii) 2Na + 2H₂O → 2NaOH + H₂

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.

Solution:

i) BaCl₂ + Na₂SO₄ → BaSO₄ + 2NaCl

ii) NaOH + HCl → NaCl + H₂O

In-text questions set 2 Page number – 10

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.

Solution:

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

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

Solution:

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 set 3 Page number – 13

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

Solution:

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:

Fe + CuSO₄ → FeSO₄ + Cu

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

 Solution:

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^–

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)

Solution:

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 Page number – 14-16

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

Solution:

(i) (a) and (b)

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

2.  Fe₂O₃ + 2Al → Al₂O₃ + 2Fe

The above reaction is an example of a

1. Combination reaction.
2. Double displacement reaction.
3. Decomposition reaction.
4. Displacement reaction.

Solution:

Answer is 4. Displacement reaction.

Explanation: The Oxygen from the Ferrous oxide is getting displaced to the Aluminium metal to form Aluminium Oxide. In this reaction Aluminum is more reactive metal than Fe. Therefore Al will displace Fe from its oxide. This type of chemical reactions in which one of the elements displace another is called displacement reaction. Here less reactive metal is displaced by more reactive metal. Since one-time displacement is occurring, therefore, it is called a single displacement reaction.

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

1. Hydrogen gas and Iron chloride are produced.
2. Chlorine gas and Iron hydroxide are produced.
3. No reaction takes place.
4. Iron salt and water are produced.

Solution:

1. Hydrogen gas and Iron chloride are produced.

Explanation: The Chlorine from Hydrogen chloride is displaced by the Iron fillings to undergo the following reaction.

2HCl + Fe → FeCl₂ + H₂

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

Solution:

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 mass. Balancing the chemical equation has no defined method and is purely a trial and error attempt.

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.

Solution:

(a) Unbalanced: H₂ + N₂ → NH₃

Balanced: 3H₂ + N₂ → 2NH₃

(b) Unbalanced: H₂S + O₂ → H₂O + SO₂

Balanced: 2H₂S + 3O₂ → 2H₂O + 2SO₂

(c)  Unbalanced:

BaCl₂ + Al₂(SO₄)₃ → AlCl₃ + BaSO₄

Balanced: 3BaCl₂ + Al₂(SO₄)₃ → 2AlCl₃ + 3BaSO₄

(d) Unbalanced: K + H₂O → KOH + H₂

Balanced:  2K + 2H₂O → 2KOH + H₂

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

Solution:

(a) 2HNO₃ + Ca(OH)₂ → Ca(NO₃)₂ + 2H₂O

(b) 2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O

(c) NaCl + AgNO₃ → AgCl + NaNO₃

(d) BaCl₂ + H₂SO₄ → BaSO₄ + 2HCl

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

Solution:

2Ca(OH)₂ + 2CO₂ → 2CaCO₃ + 2H₂O

Zn + 2AgNO₃ → Zn(NO₃)₂ + 2Ag

2Al + 3CuCl₂ → 2AlCl₃ + 3Cu

BaCl₂ + K₂SO₄ → BaSO₄ + 2KCl

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

KBr + BaI₂ → KI + BaBr₂

ZnCO₃ → ZnO + CO₂

H₂ + Cl → HCl

Mg + HCl → MgCl₂ + H₂

Solution:

2KBr + BaI₂ → 2KI + BaBr₂ (Double Displacement Reaction)

ZnCO₃ → ZnO + CO₂ (Decomposition Reaction)

H₂ + Cl → 2HCl (Combination Reaction)

Mg + 2HCl → MgCl₂ + H₂ (Displacement Reaction)

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

Solution:

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).

10. Why is respiration considered to be an exothermic reaction?

Solution:

For the survival of life, we require energy. We obtain this energy from the food we eat. The food molecules, through the process of digestion, is broken down into a simpler molecule like glucose. These substances come in contact with the Oxygen present in our body cells to form Carbon dioxide and water along with a certain amount of energy (Respiration process). Since the energy is in the form of heat (that maintains our body temperature) the respiration is considered to be an exothermic reaction. The reaction taking place is:

C₆H₁₂O₆ + 6O₂ → 6CO₂ + 6H₂O + Energy

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

Solution:

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.

In most of the cases the decomposition reaction is endothermic since heat from the surrounding or induced heat is used to break the bonds of the larger molecule. Few examples of decomposition reactions are:

ZnCO₃ → ZnO + CO₂

CaCO₃ + Energy → CaO + CO₂

2HgO → 2Hg + O₂

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

Solution:

(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.

2KClO₃ + 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.

(c) Photodecomposition reaction (Photolysis)

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

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

Solution:

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.

Example:

Displacement reaction

Mg + 2HCl → MgCl₂ + H₂

Double displacement reaction

2KBr + BaI₂ → 2KI + BaBr₂

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.

Solution:

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

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

Solution:

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. Few examples of precipitation reactions are:

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

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

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

(a) Oxidation

(b) Reduction

Solution:

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

4Na(s) + O₂(g) → 2Na₂O(s)

H₂S + O₂ → H₂O + SO₂

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

CuO(s) + H₂(g) → Cu(s) + H₂O(l)

2HgO → 2Hg + O₂

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.

Solution:

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)

18) Why do we apply paint on iron articles?

Solution:

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.

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

Solution:

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.

20) Explain the following terms with one example each.

(a) Corrosion

(b) Rancidity

Solution:

(a) 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. Rusting of iron is a good example of corrosion where the iron is converted to Iron oxide. Millions of dollars are spent annually in preventing rusting from bridges and other monuments.

(b) The condition produced by the aerial oxidation of the oil and fat present in the food material that produces an unpleasant taste and smell. The rancidity is retarded when the food is kept inside the refrigerator since the low temperature does not promote the oxidation reaction.