Class 10 Chemical Reactions and Equations Unit Test PDF Welcome to the ultimate preparation hub for Class 10 Science! Chemical Reactions a...
Class 10 Chemical Reactions and Equations Unit Test PDF
Welcome to the ultimate preparation hub for Class 10 Science! Chemical Reactions and Equations is arguably the most critical chapter in the Chemistry syllabus. It isn't just about memorizing formulas; it's about understanding the fundamental "language" of chemistry—how substances interact, transform, and balance out in the world around us.
Whether you are preparing for your first Unit Test or looking ahead to the Board Exams, practicing with the right set of questions is key to building confidence. To help you streamline your revision, we have curated a comprehensive Unit Test PDF that covers:
Balancing Chemical Equations: Step-by-step practice to master the hit-and-trial method.
Types of Reactions: Clear questions on Combination, Decomposition, Displacement, and Redox reactions.
Observations & Colors: Focusing on the practical-based questions that frequently appear in exams.
Corrosion and Rancidity: Real-world applications and prevention.
Why download this test? > This question paper is designed based on the latest NCERT pattern, featuring a mix of Multiple Choice Questions (MCQs), Short Answer types, and Case-based questions to ensure you are ready for any format.
Class 10
Science
Unit Test: Chemical Reactions and Equations
Maximum Marks: 20 Time
Allowed: 60 Minutes
Section A: Objective Type Questions (1 Mark Each = 6 Marks)
1. What happens when ferrous sulphate crystals are
heated?
(a) A single solid product is formed.
(b) It decomposes to form a solid and two gases.
(c) It turns into a white powder and releases oxygen.
(d) It undergoes a displacement reaction.
2. Which of the following represents the balanced
chemical equation for the reaction of iron with steam?
(a) Fe + H2O ⟶ Fe3O4
+ H2 (b)
3Fe + 4H2O ⟶ Fe3O4
+ 4H2
(c) 3Fe + H2O ⟶ Fe3O4
+ H2 (d) Fe
+ 4H2O ⟶ Fe3O4
+ 4H2
3. When an iron nail is immersed in a copper sulphate
solution, iron removes copper from the solution. What type of reaction is this?
(a) Combination reaction (b)
Decomposition reaction
(c) Displacement reaction (d)
Double displacement reaction
4. The reaction between sodium sulphate and barium
chloride produces a white precipitate. What is the chemical formula of this
insoluble substance?
(a) NaCl (b)
BaSO4 (c)
Na2SO4 (d)
BaCl2
5. Which of the following processes is considered an
exothermic reaction?
(a) Respiration (b)
Heating of lead nitrate
(c) Electrolysis of water (d)
Decomposition of silver chloride
6. Assertion-Reasoning Question
Directions: In the following question, a statement of
Assertion (A) is followed by a statement of Reason (R). Choose the correct
option.
Assertion (A): The reaction of calcium oxide with
water is a combination reaction. Reason (R): In this reaction, calcium
oxide and water combine to form a single product, calcium hydroxide.
(a) Both A and R are true and R is the correct explanation
of A.
(b) Both A and R are true but R is not the correct explanation of A.
(c) A is true but R is false.
(d) A is false but R is true.
Section B: Short Answer Type I (2 Marks Each = 4 Marks)
7. State any two physical observations that can help
determine whether a chemical reaction has taken place.
8. Identify the substance that is oxidised and the
substance that is reduced in the following reaction:
CuO(s) + H2(g) ⟶ Cu(s)
+ H2O(l)
Section C: Short Answer Type II (3 Marks Each = 6 Marks)
9. Why is respiration considered an exothermic
reaction? Explain the process briefly.
10. A shiny brown coloured element ‘X’ on heating in
air becomes black in colour. Name the element ‘X’ and the black coloured
compound formed. Write the balanced chemical equation for this reaction.
Section D: Case Study Based Question (4 Marks)
11. Read the passage and answer the questions that
follow: Decomposition reactions require energy either in the form of heat,
light or electricity for breaking down the reactants. Reactions in which energy
is absorbed are known as endothermic reactions. For example, white silver
chloride turns grey in sunlight. This is due to the decomposition of silver
chloride into silver and chlorine by light.
(a) Write the balanced chemical equation for the
decomposition of silver bromide in sunlight. (1 Mark)
(b) State one commercial application where the
decomposition reactions of silver chloride and silver bromide are utilised. (1
Mark)
(c) Are the decomposition reactions of silver halides exothermic or endothermic? Justify your answer. (2 Marks)
Scroll down to find the download link for the Class 10 Chemistry Unit Test PDF and start your practice today!
DOWNLOAD NOW
COMMENTS