NCERT Solutions of Chapter 1 Chemical Reactions and Equations Class 10 Science

NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations

In Text Questions

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

Solution

A magnesium ribbon should be cleaned before burning in air to remove the layer of magnesium oxide formed due to reaction of magnesium with oxygen present in the air. The layer of magnesium oxide is usually removed by rubbing the ribbon with sand paper.

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

Solution

The balanced equations for the chemical reactions are:

(I) H2 (g) + Cl2 (g) → 2HCl (g)

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

(III) Na(s) + 2H2O (l) → 2NaOH (aq) + H2 (g)

3. Write the 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.

Solution

(I) BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2NaCl(aq)

(II) NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)

4. 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 is quick lime (calcium oxide) which is used for white washing. Its chemical formula is CaO.

(II) Calcium oxide on reaction with water gives calcium hydroxide.
CaO(s) + H2O(l) → Ca(OH)2(aq)

5. Why is the amount of a gas collected in one of the test tubes in ‘Electrolysis of water’ activity double of the amount collected in the other? Name this gas.

Solution

Water is formed when hydrogen and oxygen combine in the ratio of 2: 1 by volume. So, the volume of hydrogen gas is double of oxygen gas. Thus, on decomposition of water during electrolysis, the volume of hydrogen formed is twice than that of oxygen gas.

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

Solution

Copper sulphate solution is initially blue in colour. When an iron nail is dipped in it, the blue colour changes to green. This happens due to a displacement reaction where iron being more reactive than Cu, displaces Cu to form a green coloured iron sulphate solution while copper metal gets precipitated. Hence the colour changes from blue to green. 

Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s)
CuSO4(aq): blue
FeSO4(aq): green

7. Give an example of a double displacement reaction?

Solution

Pb(NO3)2 (aq) + 2HCl (aq) → PbCl2(s) + 2HNO3(aq)

Pb(NO3)2 : Lead nitrate
PbCl2 : Lead chloride
HNO3 : Nitric acid

8. Identify the substances that are oxidized 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)

Solution

Oxidation is addition of oxygen and reduction is removal of oxygen. Therefore: 

In reaction (i), Sodium metal is oxidized to Na2O as oxygen is added to it. Oxygen is reduced to Na2O as oxygen atoms per molecule becomes less (from 2 to 1). Hence, sodium gets oxidized and Oxygen gets reduced.

In reaction (ii) Copper oxide is reduced to copper (loss of oxygen) and hydrogen is oxidized to H2O (gain of oxygen).

NCERT Exercises

1. Which of the statements about the reaction below are incorrect? 

2PbO(s) + C(s) → 2Pb(s) + CO2(g)
(i) Lead is getting reduced. 

(ii) Carbon dioxide is getting oxidised. 

(iii) Carbon is getting oxidised. 

(iv) Lead oxide is getting reduced. 

(A) (i) and (ii) 

(B) (i) and (iii) 

(C) (i), (ii) and (iii) 

(D) All statements are incorrect

Solution

(A)

In the above reaction, lead oxide is getting converted to lead and carbon is getting converted to carbon dioxide. Lead oxide is losing oxygen whereas carbon is gaining oxygen. Loss of oxygen is known as reduction while gaining oxygen is called oxidation. Hence, Lead oxide is getting reduced and carbon is getting reduced. Thus statements (iii) and (iv) are correct whereas statements (i) and (ii) are incorrect.

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.

Solution

(D)

In the given reaction, Ferric oxide is getting converted to Iron while aluminium is getting oxidized to aluminium oxide. Thus, iron is going from combined state to free state whereas aluminium is going from free state to combined state. Such a reaction is called displacement reaction as in displacement reactions, the more reactive metal (Al in this case) displaces the less reactive metal (Fe in this case) from its compound.

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.

Solution

(A)

When metal react with acids, H2 gas is evolved along with the formation of the respective metals salt

Fe(s) + 2HCl(aq) → FeCl2(s) + H2(g) ↑

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

Solution

A chemical reaction in which the number of atoms of each element is equal on both, the reactant’s side and product’s side, is called a balanced chemical equation.
An example of a balanced chemical reaction is given below: 

N2(g) + 3H2(g) → 2NH3(g)
As we can see, there are 2 atoms of N and 6 atoms of H on both the sides and hence, this reaction is called a balanced chemical equation. 

A reaction should always be written in the balanced form as an unbalanced reaction violates the fundamental principle of law of conservation of mass. According to the law of conservation of mass, the total mass of reactants should be equal to the total mass of the products.
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 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.

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.

Solution

(a) 3H2(g) + N2(g) → 2NH3(g)

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

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

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

6. Balance the following chemical equations. 

(A) HNO3 + Ca(OH)2 → Ca(NO3)2 + H2

(B) NaOH + H2SO4 → Na2SO4 + H2

(C) NaCl + AgNO3 → AgCl + NaNO

(D) BaCl2 + H2SO4 → BaSO4 + HCl

Solution

(a) 2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H2O

(b) 2NaOH + H2SO4 → Na2SO4 + 2H2O

(c) NaCl + AgNO3 → AgCl + NaNO

(d) BaCl2 + H2SO4 → BaSO4 + 2HCl

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

Solution

(A) Ca(OH)2 + CO2 → CaCO3 + H2O

(B) Zn + 2AgNO3 → Zn(NO3)2 + 2Ag

(C) 2Al + 3CuCl2 → 2AlCl3 + 3Cu

(D) BaCl2 + K2SO4 → BaSO4 + 2KCl

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)

Solution

(a) 2KBr(aq) + BaI2 (aq) → 2KI(aq) + BaBr2 (s)
In this reaction, there is an exchange of  ions between  the reactant so it is double displacement reaction.

(b) ZnCO3(s)  → ZnO(s) + CO2(g)

In this reaction, a single reactant breaks down to  give simpler products; so it is decomposition reaction.

(c) H2(g) + Cl2(g) → 2HCl(g)
In this reaction, the single product is formed from two reactants; so it is combination reaction.

(d) Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
In this reaction reaction magnesium displaced Clion from HCl. So, it is displacement reaction.

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

Solution

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

Example 1Mixture of sodium and chlorine to yield table salt

2Na(s) + Cl2(g) → 2NaCl(s) + energy
Example 2: Combustion reaction or burning of nature gas:

CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)
Example 3: Respiration reaction:

C6H12O6(aq) + 6O2(aq) → 6CO2(aq) + 6H2O(l) + energy

C6H12O6 :(Glucose)

Endothermic reaction: Reactions that absorb energy or require energy in order to proceed are called endothermic reactors.

Example: White silver chloride turns grey in sunlight. This is due to the decomposition of silver chloride in presence of sunlight and silver and chlorine formed. The energy is required (Sunlight) so it is endothermic reaction.

2AgCl(s) sunlight → 2Ag(s) + Cl2(g)

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

Solution

The carbohydrates are broken down to form glucose. This glucose combines with oxygen in the cell of our body and provides energy so it is a exothermic reaction. 

C6H12O6(aq) + 6O2(aq) → 6CO2(aq) + 6H2O(l) + energy

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

Solution

Decomposition reactions are those in which a compound breaks down to form two or more substances. While in the combination reaction single product is formed from two or more reactants. Thus decomposition reaction is exact opposite of combination reactions.

Example: 

2H2O(l) → 2H2(g) + O2(g) 2H2(g) + O2(g) → 2H2O(l) + energy

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

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

Solution

Displacement reaction: A more reactive element replaces a less reactive element from a compound.

Example of displacement reaction: 

CuSO4(aq) + Zn(s) → ZnSO4(aq) + Cu(s)
Zinc is more reactive metal as compare to copper so, zinc displace the copper ion in copper.

Double displacement reaction: In the double displacement reaction two compounds react and the positive ion (cation) and the negative ion (anion) of the two reactants switch place forming two new compounds or products.

Example: Na2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2NaCl(aq)

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

Solution

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

Solution

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

Example: 

Na2CO3(aq) → CaCO3(s) + CaCl2(aq) + 2NaCl(aq)
In this reaction, calcium carbonate is obtained as a precipitate. Hence, it is a precipitation reaction.

Na2SO4(aq) + BaCl2(aq)→ BaSO4(s) + 2NaCl(aq)

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

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

(a) Oxidation 

(b) Reduction

Solution

(a) Oxidation is the gain of oxygen

Example: 

(i) CO2 + H2 → CO + H2O
H2 is oxidized to H2O as there is addition of oxygen.

(ii) 2Cu + O2 → 2CuO
Cu is oxidised to CuO.

(b) Reduction is the loss of oxygen.

Example: 

(i) CO2 + H2 → CO + H2O
CO2 is reduced to CO as there is removal of oxygen.

(ii) CuO + H2 → Cu + H2O
CuO is reduced to Cu.

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.

Solution

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

2Cu + O2 → 2CuO

18. Why do we apply paint on iron articles?

Solution

Iron, in the presence of moisture, reacts with oxygen to form hydrated iron oxide.

4Fe + 3O2 + nH2O → 2Fe2O3. nH2O
nH2O : Hydrated iron oxide. This hydrated iron oxide is rust

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

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

Solution

Nitrogen is an inert gas and does not easily 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, rancidity of oil and fat containing food items is avoided.

20. Explain the following terms with one example each. 

(a) Corrosion 

(b) Rancidity

Solution

(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

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 air tight containers
  2. Storing food in refrigerators
  3. Adding antioxidants
  4. Storing food in an environment of nitrogen.

We have discussed the concepts of physical and chemical changes in earlier classes. Chemical reactions signify chemical change. Chemical reactions are various processes which involves change in chemical composition of some substance and forming new one. Many chemical reactions keep taking place in our surroundings. Examples are burning of candle, milk turning sour, rusting of iron. Chemical reaction taking place has many indicators such as change in color and temperature. After that chemical equation has been taught as representation of chemical reaction. It is discussed how to balance a chemical equation to represent law of conservation of mass. After that, it is discussed how to show other important aspects of chemical reaction for example, physical states of chemical reactions. Other factors like temperature can also be mentioned on arrow. Next various types of reactions are discussed with suitable examples. Analytical questions are asked on reactions mentioned in the chapter. Questions based on writing and balancing a chemical equation based on chemical reaction is also asked. So, in this first chapter of NCERT Textbook of chemistry for class 10 CBSE students, we will learn the basics of chemical reactions and its different types. By learning this chapter, students are meant to get proficient with balancing of chemical equations, reactions of different metals and non-metals with acids and bases.