CBSE Class 10 Science Chapter-1 Chemical Reactions and Equations Notes & NCERT Solution

Here are key points for CBSE Class 10 Science Chapter 1: “Chemical Reactions and Equations”:

Key Points:

1. Chemical Equation:

• A representation of a chemical reaction using symbols and formulae of the substances involved is called a chemical equation.

1. Balancing Equations:

• The number of atoms of each element on the reactant side must be equal to the number of atoms of the same element on the product side. This is achieved by balancing the chemical equation.

1. Types of Chemical Reactions:

• Combination Reaction:
  • Two or more substances combine to form a new substance.
• Decomposition Reaction:
  • A single substance breaks down into two or more simpler substances.
• Displacement Reaction:
  • A more reactive element displaces a less reactive element from its compound.
• Double Displacement Reaction:
  • Exchange of ions between two compounds.

1. Oxidation and Reduction:

• Oxidation: The addition of oxygen or loss of hydrogen or electrons.
• Reduction: The addition of hydrogen or loss of oxygen or gain of electrons.

1. Redox Reactions:

• Reactions in which both oxidation and reduction occur simultaneously.

1. Effect of Temperature on Reaction Rate:

• Generally, the rate of a reaction increases with an increase in temperature.

1. Effect of Concentration on Reaction Rate:

• An increase in the concentration of reactants often leads to an increase in the rate of reaction.

1. Catalyst:

• A substance that alters the rate of a chemical reaction without being consumed in the process.

NCERT Solutions:

• Exercise 1:
• Q1. Balancing of Chemical Equations
• Exercise 2:
• Q1. Questions based on Types of Chemical Reactions
• Exercise 3:
• Q1. Questions based on Oxidation and Reduction
• Exercise 4:
• Q1. Questions on Effect of Temperature and Concentration on Reaction Rate
• Exercise 5:
• Q1. Questions related to Catalyst and Chemical Equations

These key points cover the fundamental concepts in CBSE Class 10 Science Chapter 1. If you have specific questions or need further clarification on any topic, feel free to ask!

Chemical Reaction: The process by which a chemical substance transforms into another chemical substance is known as a chemical reaction. Examples include the rusting of iron, the setting of milk into curd, digestion of food, and respiration.

In a chemical reaction, a new substance is formed, which is completely different in properties from the original substance. Therefore, a chemical change occurs during a chemical reaction, involving only a rearrangement of atoms.

Reactants are the substances that take part in a chemical reaction, while the new substances produced as a result are called products. For instance, the burning of magnesium in the air produces magnesium oxide, represented by the chemical equation: 2Mg(s) + O2(g) → 2MgO(s).

Characteristics of Chemical Reactions:

1. Evolution of gas: For example, the reaction between zinc and dilute sulphuric acid: Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) ↑
2. Change in color: Seen in reactions like citric acid with potassium permanganate, resulting in a change from purple to colorless.
3. Change in the state of a substance: Illustrated by the combustion of candle wax, which changes from solid to liquid and gas.
4. Change in temperature: Seen in reactions like the combustion of quick lime and the reaction between zinc granules and dilute sulphuric acid.
5. Formation of precipitate: Exemplified by the reaction between sulphuric acid and barium chloride solution: BaCl2(aq) + H2SO4(aq) → BaSO4(s) (ppt) + 2HCl(aq)

Chemical Equation: A representation of a chemical reaction using symbols and formulae of the substances involved. For example, A + B → C + D, where A and B are reactants, and C and D are products.

Balanced Chemical Equation: An equation where the number of atoms of each element is equal on both sides. This ensures compliance with the Law of Conservation of Mass.

Unbalanced Chemical Equation: An equation where the number of atoms of each element is not equal on both sides.

Balancing a Chemical Equation: The process of adjusting coefficients to make the number of atoms of each element equal on both sides.

Types of Chemical Reactions:

1. Combination Reaction: A + B → AB
2. Decomposition Reaction: AB → A + B
3. Displacement Reaction: A + BC → AC + B
4. Double Displacement Reaction: AB + CD → AC + BD
5. Oxidation and Reduction Reactions (Redox): Simultaneous processes of oxidation and reduction.
6. Exothermic Reaction: Releases energy, like the combustion of carbon.
7. Endothermic Reaction: Absorbs heat, such as the decomposition of calcium carbonate.

Effects of Oxidation Reactions in Everyday Life:

1. Corrosion: Slow conversion of metals into undesirable compounds, illustrated by the rusting of iron.
2. Rancidity: Change in taste and odor of food materials containing fat and oil due to oxidation. Preventive methods include adding antioxidants, vacuum packing, replacing air with nitrogen, and refrigeration.

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 the air?
Answer:
A magnesium ribbon should be cleaned before burning in the air because it gets covered with a layer of magnesium oxide when exposed to air for a long time. This layer hinders the burning of magnesium. Cleaning the ribbon removes this layer, allowing for efficient 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
Answer:
(i) ( H_2 + Cl_2 \rightarrow 2HCl )
(ii) ( 3BaCl_2 + Al_2(SO_4)_3 \rightarrow BaSO_4 + 2AlCl_3 )
(iii) ( 2Na + 2H_2O \rightarrow 2NaOH + H_2 \uparrow )

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:
(i) ( BaCl_2 (aq) + Na_2SO_4 (aq) \rightarrow BaSO_4 (s) + 2NaCl (aq) )
(ii) ( NaOH (aq) + HCl (aq) \rightarrow NaCl (aq) + H_2O (l) )

Page Number: 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 used for whitewashing is calcium oxide (quicklime), and its formula is (CaO).
(ii) The reaction of calcium oxide with water is (CaO + H_2O \rightarrow 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 that of the amount collected in the other? Name this gas.
Answer:
In electrolysis of water, two molecules of hydrogen gas (H₂) are produced for every molecule of oxygen gas (O₂). Hence, the amount of hydrogen gas collected is double that of oxygen gas. The gas collected is hydrogen.

Page Number: 13

Question 1
Why does the color of copper sulphate solution change when an iron nail is dipped in it?
OR
An iron nail is dipped in the solution of copper sulphate for about 30 minutes. State the change in color observed. Give the reason for the change.
Answer:
When an iron nail is dipped in copper sulphate solution, a displacement reaction occurs. The color of copper sulphate solution changes from blue to light green due to the formation of iron sulphate.

Question 2
Give an example of a double displacement reaction other than the one given in Activity 1.10 (NCERT Text Book).
Answer:
Sodium hydroxide and hydrochloric acid react to form sodium chloride and water, which is an example of a double displacement reaction.

Question 3
Identify the substances that are oxidized and the substances which are reduced in the following reactions.
(i) (4Na(s) + O_2(g) \rightarrow 2Na_2O(s))
(ii) (CuO (s) + H_2(g) \rightarrow Cu (s) + H_2O(l))
Answer:
(i) Substances oxidized: (4Na) (sodium), Substances reduced: (O_2) (oxygen).
(ii) Substances reduced: (CuO) (copper oxide), Substances oxidized: (H_2) (hydrogen).

NCERT Solutions for Class 10 Science Chapter 1 Textbook Chapter End 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
Answer:
(i) (a) and (b)

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
Answer:
(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.
Answer:
(a) Hydrogen gas and iron chloride are produced.

Question 4
What is a balanced chemical equation ? Why should chemical equations be balanced ?
Answer:
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.
Answer:
(a) 3H2 (g) + N2 (g) → 2NH3 (g)
(b) H2S (g) + 3O2 (g) → SO2 (g) + 2H2O(l)
(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:
(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
Answer:
(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)
Answer:
(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.
Answer:
Exothermic reactions : Those reactions in which heat is evolved are known as exothermic reactions. An exothermic reaction is indicated by writing “+ Heat”on the products side of an equation.
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. An endothermic reaction is usually indicated by writing “Heat” on the product side of a chemical equation.
Examples :
(i) C (s) + 2S (s) → CS2 (l) – Heat
(ii) N2 (g) + O2 (g) → 2NO(g) – Heat

Question 10
Why is respiration considered an exothermic reaction ? Explain.
Answer:
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.
NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations Chapter End Questions Q10

Question 11
Why are decomposition reactions called the opposite of combination reactions? Write equations for these reactions.
Answer:
In a decomposition reaction, a single compound breaks down to produce two or more simpler substances.
For example:
NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations Chapter End Questions Q11

While, in a combination reaction, two or more substances simply combine to form a new substance.
For example:
NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations Chapter End Questions Q11.1

Question 12
Write one equation each for the decomposition reactions where energy is supplied in the form of heat, light or electricity.
OR
Decomposition reactions require energy either in the form of heat or light or electricity for breaking down the reactants. Write one equation each for decomposition reactions where energy is supplied in the form of heat, light and electricity. [CBSE 2015 (Delhi)]
Answer:
NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations Chapter End Questions Q12

Question 13
What is the difference between displacement and double displacement reactions? Write equations for these reactions.
Answer:
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.
Answer:
NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations Chapter End Questions Q14

Question 15
What do you mean by a precipitation reaction ? Explain by giving examples.
Answer:
A reaction in which an insoluble solid called precipitate is formed that separates from the solution is called a precipitation reaction.
Example : When a solution of iron (III) chloride and ammonium hydroxide are mixed, a brown precipitate of iron (III) hydroxide is formed.
NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations Chapter End Questions Q15

Question 16
Explain the following in terms of gain or loss of oxygen with two examples each:
(a) Oxidation and
(b) Reduction.
Answer:
(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: (i) CuO + H2 Heat−→−− Cu + H2O
Here, copper oxide is being reduced to copper because oxygen gets removed from copper oxide.

(ii) ZnO + C → Zn + CO
Here, zinc oxide is being reduced to zinc because oxygen gets removed from zinc oxide.

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:
Element ‘X’ is copper (Cu).
The black coloured compound is copper oxide (CuO). The reaction involved is
NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations Chapter End Questions Q17

Question 18
Why do we apply paint on iron articles ?
Answer:
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 ?
Answer:
To keep food items fresh and save from getting oxidised, food items are flushed with nitrogen.

Question 20
Explain the following terms with one example each (a) Corrosion, (b) Rancidity.
Answer:
(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].
NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations Chapter End Questions Q20

(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.
Rancidity can be prevented by adding anti-oxidants to foods containing fats and oils. It can also be prevented by flushing fat and oil containing foods with nitrogen before sealing.

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

NCERT Solutions for Class 10 Science (Chemistry) Chapter 1 Chemical Reactions and Equations are part of NCERT Solutions for Class 10 Science. Here we have given Class 10 Science NCERT Solutions Chapter 1.

Question 1
Which of the given 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
Solution:
(i) (a) and (b)

Question 2

The above reaction is an example of a
(i). Combination reaction
(ii). Double displacement reaction
(iii). Decomposition reaction
(iv). Displacement reaction
Solution:
(iv) 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
Solution:
Hydrogen gas and iron chloride are produced

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

Question 4
What is a balanced chemical equation? Why should chemical equations be balanced?
Solution:
An equation for a chemical reaction is an equation in which the number of atoms for each element in the reaction and the total charge is the same for both the reactants and the products. In other words, the mass and the charge are balanced on both sides of the reaction.

Question 5
Translate the following statements into chemical equations and then balance them.
a. Hydrogen gas combines with nitrogen to form ammonia
b. Hydrogen sulfide gas burns in air to give water and sulfur dioxide
c. Barium chloride reacts with Aluminium sulfate to give Aluminium chloride and a precipitate of barium sulphate
d. Potassium metal reacts with water to give a potassium hydroxide and hydrogen gas
Solution:
a. 3H₂ + N₂ → 2NH₃
b. 2H₂S + 3O₂ → 2H₂O + 2SO₂
c. 3BaCl₂ + Al₂(SO₄)₃ → 2AlCl₃ + 3BaSO₄
d. 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
Solution:
a. 2HNO₃ + 2Ca(OH)₂ → Ca(NO₃)₂ + 2H₂O
b. 6NaOH + 3H₂SO₄ → 3Na₂SO₄ + 6H₂O
C. NaCl + AgNO₃ → AgCI + 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 chlorideAnswer:(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 of each case.

Solution:
a. 2KBr + BaI₂ → 2KI + BaBr₂ — Double Displacement reaction
b. ZnCO₃ → ZnO + CO₂ — Decomposition reaction
c. H₂ + Cl₂ → 2HCl — Combination reaction
d. Mg + 2HCl → MgCl₂ + H₂ — Displacement reaction

Question 9
What is meant by exothermic and endothermic reactions? Give examples.
Solution:
An exothermic reaction is one that releases heat.
If 1 mole of N₂ molecule reacts with 1 mole of O₂ molecule, the heat of 184 KJ has to be supplied to initiate the reaction to give 1 mole of NO molecule. This means that the bonds between N – N and O – O are so strong that they do not break easily. N₂ has triple covalent bond between the two N atoms. O₂ has a double covalent bond. Thus energy has to be put into the reaction to break the strong bonds. Thus the above reaction is a good example of an endothermic reaction.

Question 10
Why is respiration considered an exothermic reaction?
Solution:
During respiration, glucose combines with oxygen in the cells of our body to form carbon dioxide and water along with the production of energy.
Glucose + oxygen → carbon dioxide + water + energy
It is an exothermic reaction, because energy is produced during this process.

Question 11
Why are decomposition reactions called the opposite of combination reactions? Write equations for decomposition reactions.
Solution:
Essentially, decomposition reactions are the opposite of combination reactions. A compound decomposes (i.e., “splits-up”) into two or more compounds and/or elements. For example, mercury (II) oxide will, decompose into mercury metal and oxygen, upon heating:
2HgO →  2Hg + O₂
Since heat had to be added to make this reaction occur, it is an endothermic reaction. Most decomposition reactions are endothermic. Another example of decomposition reaction is the heating of calcium carbonate (sea shells, chalk):

Question 12
Write one equation each for decomposition reactions in which energy is supplied in the form of heat, light or electricity?
Solution:
When calcium carbonate is heated, it decomposes to give calcium oxide and carbon dioxide:

Question 13
What is the difference between displacement and double displacement reactions? Write relevant equations for the above?
Solution:
The difference between the displacement and double displacement reactions is that in a displacement reaction one element displaces another by virtue of it being more reactive whereas in a double displacement two anions and two cations switch places between two compounds respectively.
For example:
CuSO₄ (aq) + Zn(s) → ZnSO₄ + Cu(s)
Blue copper sulphate solution reacting with solid zinc will give rise to colourless zinc sulphate solution and solid copper. Thus Zn displaces Cu in the salt form. Zn is more reactive than Cu.
An example of double displacement reaction is the reaction between sodium carbonate and calcium chloride, both in aqueous
Solution:
Na₂CO₃ (aq) + CaCl₂ (aq) → CaCO₃ (ppt) + 2NaCl(aq)

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

Question 15
What do you mean by a precipitation reaction? Explain by giving examples:
Solution:
A precipitation reaction is a reaction in which soluble ions in separate solutions are mixed together to form an insoluble compound that settles out of solution as a solid. This insoluble compound is called a precipitate.

An example of a precipitation reaction
Aqueous silver nitrate (AgNO3), when added to a solution containing potassium chloride (KCl), precipitates a white solid, and silver chloride is observed.
AgNO_3 (aq) + KCl_(aq) → AgCl_(s) + KNO_3(aq)
The silver chloride (AgCl) has formed a solid, which is observed as a precipitate.

Question 16
A shiny brown colored element ‘X’ on heating in the air becomes black in color. Name the element ‘X’ and the black coloured compound formed.
Solution:
The shiny brown colored element X is copper metal (Cu). When copper metal is heated in air, it forms a black colored compound copper oxide. So, the black colored compound is the copper oxide or copper (II) oxide, CuO.

Question 17
Why do we apply paint on iron articles?
Solution:
Rust is a soft and porous substance, which gradually falls from the surface of an iron object, and then the iron below starts rusting. Thus, rusting of iron (or corrosion of iron) is a continuous process which, if not prevented in time, eats up the whole iron object. So, when we apply paint on iron articles it reduces the rusting of iron.

Question 18
Oil and fat containing food items are flushed with nitrogen. Why?
Solution:
Packaging fat and oil containing foods in nitrogen gas can prevent rancidity. When the fat and oil present in food materials gets oxidised (in air), their oxidation products have an unpleasant smell and taste. When it is surrounded by unreactive gas, nitrogen, there is no oxygen (of air) to cause its oxidation and make it rancid.

Question 19
Explain the following terms with one example each.
a. Corrosion
b. Rancidity
Solution:
a. Corrosion is the process in which metals are eaten up gradually by the action of air, moisture or a chemical on their surface. Corrosion is caused mainly by the oxidation of metals by the oxygen of air.
Example: Rusting of iron is the most common form of corrosion. When an iron object is left in damp air for a considerable period of time, it gets covered with a red-brown flaky substance called ‘rust’. This is called rusting of iron.
b. The condition produced by aerial oxidation of fat and oil in food which is marked by an unpleasant smell and taste is called rancidity.
Example: Rancidity can be retarded by keeping food in a refrigerator.
The refrigerator has a low temperature inside it. When the food is kept in a refrigerator, the oxidation of fat and oil in it is slowed down due to low temperature. So, the development of rancidity due to oxidation is retarded.

Question 20
Why should a magnesium ribbon be cleaned before burning in air?
Solution:
To remove the oxide layer and facilitates rapid burning.

Question 21
Write the 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

Question 22
Write a balanced chemical equation and state symbols for the following reactions.
a. Solutions of barium chloride and sodium sulphate in water react to give insoluble barium sulphate and the solution of sodium chloride
b. Sodium hydroxide solution (in water) reacts with hydrochloric acid solution (in water) to produce sodium chloride solution and water.
Solution:

Question 23
A solution of a substance ‘X’ is used for white washing.
Name the substance ‘X’ and write its formula.
(i) Write the reaction of the substance ‘X; named in (ii) above with water
Solution:

Question 24
Why does the colour of copper sulphate solution change when an iron nail is dipped into it?
Solution:
In this reaction, iron displaces copper from copper sulphate solution. The deep blue colour of copper sulphate solution fades due to the formation of light green solution of iron sulphate. A red-brown coating of copper metal is formed on the surface of the iron metal. This displacement reaction occurs because iron is more reactive than copper.

Question 25
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)
Solution:
i. 4Na(s) + O₂ (g) → 2Na₂O(s)
Here oxygen is added to sodium. The addition of oxygen is Called oxidation. So the substance that is oxidized is sodium Na.
ii. CuO(s) + H₂(g) → Cu(s) + H₂O(l)

In this reaction, copper oxide (CuO) gives the oxygen required for the oxidation of hydrogen; therefore, copper oxide is the oxidizing agent. Hydrogen is responsible for removing oxygen from copper oxide; therefore, hydrogen is the reducing agent here.