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Chapter 1: Chemical Reactions and Equations (Part 2) SSLC | Class 10

Apr 10
3 min read

In continuation of Chapter 1, this part focuses on the Types of Chemical Reactions, which is one of the most important topics in Class 10 Science. Understanding these reactions helps students identify how substances interact and change in different chemical processes.

In this blog, we provide simple and exam-focused notes on different types of chemical reactions, along with examples and important questions. These notes are designed for quick revision and better understanding.


Types of Chemical Reactions

1. Combination Reaction

A chemical reaction in which two are more reactants combined to form a single product is called combination reaction

Example:

X + Y------ XY

Burning of fossil fuel  ---- C + O2 ----- CO2

Formation of water ----- 2 H 2  + O2 ----- 2 H2O

CaO + H₂O → Ca(OH)₂ + Heat

Also called exothermic reaction (heat released)

burning of natural gas:CH 4 + 2 O2------ CO2 + 2 H2O

Respiration : C6H12O6 + 6 O2 ------ 6 CO2 + 6 H2 O + energy

2. Decomposition Reaction

Reaction in which compounds splits up into two are more simple substances are known as decomposition reaction. It is carried out by heat light and electricity

Example:

CaCO₃ → CaO + CO₂

👉 Can occur using:

  • Heat

  • Light

  • Electricity

Electrolysis of water is a best example for decomposition reaction

In this  reaction hydrogen is collected at the cathode side and oxygen is collected at the anode side In the ratio of 2:1

3. Displacement Reaction

A reaction in which a more reactive element displaces a less reactive element.

Example:

Fe + CuSO₄ → FeSO₄ + Cu

4. Double Displacement Reaction

Chemical reaction in which more reactive element in a compound displaces a less reactive element in a compound

Example:

Fe + CuSO4 ------ FeSO4 + Cu

CuSO4 + Zn ------- ZnSO4 + Cu

Pb + CuCl2------ PbCl2 + Cu

In the above examples zinc and lead are more reactive element than copper therefore they displaces copper from its compound

5. Oxidation and Reduction

This is also a precipitation reaction: Any reaction in which an insoluble solid is formed that separate from the solution is called precipitation reaction

  • Oxidation → Gain of oxygen / Loss of hydrogen

  • Reduction → Loss of oxygen / Gain of hydrogen

Ex: BaCl2 + Na2 SO4.-------- BaSO4 + 2 NaCl


Important Questions

  1. What is the uses of slaked lime Slaked lime is used for whitewashing

    Ca ( OH)2 + CO2 ------ CaCO3 + H2O

  2. Difference between exothermic and endothermic reaction? Give example

    Reaction in which heat is liberated is called exothermic reaction

    Ex: Burning of coal, respiration, decomposition

    Reaction in which heat is absorbed is called endothermic reaction

    Ex: Decomposition of calcium carbonate

  3. Write one equation each for decomposition reaction where energy supplied in the form of heat light or electricity

    Heat: 2FeSO4 ------- Fe2O3 + SO2 + SO3

    Electricity : 2 H2O----2 H2 + O2

    Light  : 2 AgCl ----- 2 Ag + Cl2

  4. Draw a neat labelled diagram of electrolysis of water

  1. What are the uses of silver Chloride and Bromide

    The decomposition reaction of Silver Bromide and silver chloride are used in black and white photography

  2. Among iron zinc lead which which is more reactive

    Zinc is more reactive than iron and lead

  3. Bacl2 + Na2 SO4 ------- BaSO4 + 2 NaCl what is precipitation reaction which ions are responsible for this reaction?

    Reaction in which an insoluble solid is formed that separate from the solution is called precipitate reaction

     In the above example barium and sulphate ions are responsible for this reaction

  4. In the below diagram name the type of reaction and what type of fumes  are liberated

    It is an example for thermal decomposition reaction

    Here deliberated fumes are brown in colour  ( NO)2

  5. What type of reaction is this? Write the chemical equation for the below diagram

    It is an example for displacement reaction: Fe+ CuSO4  ----- FeSO4 + Cu

  6. Analyse the activity depicted in the figure sulphate crystal given below in this activity when ferrous sulphate crystals are heated does the colour and crystalline nature of it remain same or not support your answer with reason

    It is a type of decomposition reaction and endothermic reaction, here sulphate crystal loses the water and changes its colour, it changes to sulphur trioxide, ferric oxide and Sulphur  dioxide

    2 FeSO4 ------ Fe2 O3 + SO2 + SO3

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