Case Study Questions for Class 10 Science Chapter 1

Case Study Questions for Class 10 Science Chapter 1 Chemical Reactions and Equations provided below is very helpful to understand the new format of Board Exams. Case Study Questions for class 10 Chemistry is a very trustable source for practice. Class 10 Science Chapter 1 Case Study Questions is provided to you by NCERT HUB.

Solve the given Case Study Questions for Class 10 Science Chapter 1  to enhance your performance in the upcoming Board Exam. Case Study Questions for Class 10 Chemical Reactions and Equations is very important as these types of questions will be asked in the Board Exam.

Case Study Questions for Class 10 Science Chapter 1 Chemical Reactions and Equations

1. Read the following and answer the questions from 1.1 to 1.5 :

Amit took a lime solution and passed a gas ‘X’ through it. The solution becomes turgid. This solution was then divided into two parts. In the first part, more of gas ‘X’ was passed. While in the second part concentrated sulphuric acid was added. A white precipitate was formed in second part.

1.1) The gas mentioned in above passage is :
(a) O₂
(b) H₃S
(c) CO₂
(d) H₂Answer

1.2) Lime water and chlorine reacts to form :
(a) CaCl₂
(b) CaOCl₂
(c) CaO
(d) CaCOAnswer

1.3) A solution of a substance X is used for white washing. Identify X :
(a) CaO
(b) Ca(OH)₂
(c) CaCO₃
(d) CO₂

Answer

1.4) Ca(HCO₃) is :
(a) insoluble in water
(b) soluble in water
(c) partially soluble in water
(d) partially insoluble in waterAnswer

1.5) Lime water turns milky in the reaction due to the :
(a) oxygen gas is evolved
(b) formation of calcium bicarbonate
(c) CO₂ gas is evolved
(d) formation of calcium carbonateAnswer

Please share Case Study Questions for Class 10 Science Chapter 1 with your friends !

2. Read the following and answer the questions from 2.1 to 2.5 :

In decomposition reactions, a single reactant breaks down to form two or more products. Decomposition reaction is opposite to combination reaction. Thermal decomposition reactions use the energy in form of heat for decomposition of reactants. Electrolytic decomposition reactions involve the use of electrical energy for the decomposition of reactant molecules. Photolysis or or photochemical decomposition involves the use of light energy for the purpose of decomposition.

2.1) Which of the following reactions is a decomposition reaction ?
(a) NaOH + HCl → NaCl + H₂O
(b) NH₄CNO → H₂NCONH₂
(c) 2KClO₃ → 2KCl + 3O₂
(d) H₂ + I₂ → 2HIAnswer

2.2)  2Pb(NO3 )2 → 2PbO + nA + O₂. What is nA in the given reaction ?
(a) NO₂
(b) 2PbNO₂
(c) 4NO₂
(d) 4NOAnswer

2.3) Amino acid is formed by the decomposition of which component of our diet ?
(a) Fat
(b) Protein
(c) Starch
(d) CarbohydrateAnswer

2.4) Silver chloride on exposure to sunlight for a long duration turns grey due to (i) the formation of silver by decomposition of silver chloride (ii) Sublimation of silver chloride (iii) decomposition of chlorine gas from silver chloride (iv) Oxidation of silver chloride. The correct statement(s) is / are :

(a) Only (iv)
(b) Only (i) and (iii)
(c) Only (ii) and (iii)
(d) Only (i) and (ii)Answer

2.5) What type of chemical reaction takes place when electricity is passed through water ?
(a) Displacement reaction
(b) Photochemical decomposition
(c) Electrolytic decomposition
(d) Thermal decompositionAnswer

How much do you like Case Study Questions for Class 10 Science Chapter 1 ?

Check Now :

• Class 10 Science MCQs
• Class 10 SST MCQs
• Class 10 Term-1 Sample Paper 2025-22

3. Read the following and answer the questions from 3.1 to 3.5 :

Redox reactions are those reactions in which oxidation and reduction occur simultaneously. A redox reaction is made up of two half reactions. In the first half reaction, Oxidation takes place and in second half reaction, reduction occurs. Oxidation is a process in which a substance loses electrons and in reduction, a substance hydrogen to a substance and removal of oxygen from a substance. 

The substance which gives oxygen to another substance or removes hydrogen from another substance in an oxidation reaction is known as oxidising agent, while the substance which gives hydrogen to another substance or removes oxygen from another substance in a reduction reaction is known as reducing agent. 

3.1) Which of the following is a redox reaction?
(a) CaCO₃ → CaO + CO₂
(b) CaO + 2HCl → CaCl₂ + H₂O
(c) H₂ + Cl₂ → 2HCl
(d) NaOH + HCl → NaCl + H₂OAnswer

3.2) Identify the reaction in which H₂O₂ is acting as a reducing agent.
(a) Cl₂ + H₂O₂ → 2HCl + O₂
(b) 2FeCl₂ + 2HCl + H₂O₂ → 2FeCl₃ + 2H₂O
(c) H₂SO₃ + H₂O₂ → H₂SO₄ + H₂O
(d) 2HI + H₂O₂ → 2H₂O + I₂Answer

3.3) For the following reaction, identify the correct statement.

                ZnO + CO → Zn + CO₂ 

(a) CO₂ is being oxidised.
(b) ZnO is being reduced.
(c) ZnO is being oxidised.
(d) CO is being reduced.Answer

3.4) In the following reaction, which substance is reduced ?

            PbS + 4H₂O₂ → PbSO₄ + 4H₂O
(a) PbSO₄
(b) PbS
(c) H₂O
(d) H₂O₂Answer

3.5) For the following reactions, identify the one in which H₂S acts as a reducing agent .
(a) CuSO₄ + H₂S → CuS + H₂SO₄
(b) Cd(NO₃)₂ + H₂S → CdS + 2HNO₃
(c) 2FeCl₃ + H₂S → 2FeCl₂ + 2HCl + S
(d) None of theseAnswer

Practice Case Study Questions for Class 10 Science Chapter 1 to boost your score in Board Exam.

4. Read the following and answer the questions from 4.1 to 4.5 :

In a chemical reaction, reactants are converted into products. The conversion of reactants into products in a chemical reaction is often accompanied by some features. These features which take place as a result of chemical reaction are known as characteristics of chemical reactions. Some important characteristics of chemical reactions are : evolution of heat, change in colour, change in temperature etc.

4.1) Reaction of magnesium with air is :
(a) exothermic reaction
(b) substitution reaction
(c) endothermic reaction
(d) reversible reactionAnswer

4.2) Which law is satisfied by a balanced chemical equation ?
(a) Law of multiple proportions
(b) Law of constant proportions
(c) Law of conservation of mass
(d) Law of conservation of chemicalAnswer

4.3) Which one of the following processes involve chemical reactions ?
(a) Storing of Oxygen gas under pressure in a gas cylinder
(b) Liquefication of air
(c) Keeping petrol in china dish in the open
(d) Heating copper wire in the presence of air at high temperatureAnswer

4.4) In which of the following reactions, high amount of heat energy will be evolved ?
(a) Electrolysis of water
(b) Burning of LPG
(c) Decomposition of AgBr in the presence of light
(d) Dissolution of NH₄Cl in waterAnswer

4.5) What type of chemical reaction takes place when electricity is passed through water ?
(a) Thermal decomposition
(b) Photochemical decomposition
(c) Water decomposition
(d) Electrolytic decompositionAnswer

5. Read the following and answer the questions from 5.1 to 5.5 :

You must have observed that iron articles are shiny when they are new, but get coated with a reddish brown powder when left for sometime. This process is commonly known as rusting of iron. Some other metals also get tarnished in the same manner. When a metal is attacked by substances around it such as moisture, its said to corrode and this process is called corrosion. The black coating on silver and the green coating on copper are some examples of corrosion.

5.1) Chemically rust is :
(a) hydrated ferrous oxide
(b) hydrated ferric oxide
(c) only ferric oxide
(d) None of theseAnswer

5.2) Rusting of iron involves a chemical reaction which is a combination of :
(a) Oxidation as well as combination reactions
(b) Reduction as well as displacement reactions
(c) Oxidation as well as displacement reactions
(d) Reduction as well as combination reactionsAnswer

5.3) Rusting of iron takes place in :
(a) ordinary water
(b) distilled water
(c) Both (a) and (b)
(d) None of theseAnswer

5.4) Silver articles turns black when kept in the open for a few days due to formation of :
(a) Ag₂S
(b) H₂S
(c) AgS
(d) AgSO₄Answer

5.5) Copper objects lose their shine and form green coating of :
(a) copper oxide
(b) copper carbonate
(c) basic copper carbonate
(d) copper hydroxide and copper oxideAnswer

We hope the given Case Study Questions for Class 10 Science Chapter 1 Chemical Reactions and Equations provided below is very helpful to understand the new format of Board Exams. Case Study Questions for class 10 Chemistry Chapter 1 is a very trustable source for practice. If you have any queries regarding Case Study Questions for Class 10 Science Chapter 1, contact us and we will get back to you soon.

Here are some case study questions based on Chapter 1: “Chemical Reactions and Equations” from Class 10 Science. These questions are designed to help you apply the concepts of chemical reactions and equations in practical scenarios.

Case Study 1: Rusting of Iron

Case Study:
A metal gate in a park is exposed to air and moisture over time. After a few months, the gate begins to show signs of reddish-brown patches on its surface. This reddish-brown substance is commonly referred to as rust. The rusting of iron occurs due to the combination of iron with oxygen from the air and moisture from the surroundings. Rusting is a type of chemical reaction that affects the properties of iron.

Questions:

1. What type of chemical reaction is rusting of iron? Write the balanced chemical equation for the rusting of iron.

2. Why is the rusting of iron considered a redox reaction?

3. Name one method to prevent rusting of iron.

4. What is the role of moisture in the rusting process?

Case Study 2: Decomposition of Calcium Carbonate

Case Study:
In a laboratory, a student is asked to perform a thermal decomposition reaction using calcium carbonate (CaCO₃). When calcium carbonate is heated strongly, it breaks down into calcium oxide (CaO) and carbon dioxide (CO₂) gas. This reaction is commonly observed in the formation of lime (CaO) from limestone.

Questions:

1. Identify the type of chemical reaction taking place during the decomposition of calcium carbonate.

2. Write the chemical equation for the decomposition reaction of calcium carbonate.

3. What is the role of heat in this reaction?

4. What gas is released during this reaction?

5. What is the importance of the decomposition reaction of calcium carbonate in industry?

Case Study 3: Photosynthesis

Case Study:
Plants undergo a process called photosynthesis, where they convert carbon dioxide and water into glucose and oxygen in the presence of sunlight. The energy from sunlight is absorbed by chlorophyll in plant cells. The process is essential for the production of food in plants and also releases oxygen, which is crucial for life on Earth.

Questions:

1. What type of chemical reaction is photosynthesis?

2. Write the balanced chemical equation for the process of photosynthesis.

3. How does chlorophyll assist in this reaction?

4. What is the role of sunlight in this reaction?

5. Why is photosynthesis considered an endothermic reaction?

Case Study 4: Reaction of Hydrochloric Acid with Zinc

Case Study:
A student is performing an experiment where hydrochloric acid (HCl) is added to zinc metal (Zn) in a beaker. The reaction produces a colorless gas that bubbles up and dissolves in water. The student identifies the gas as hydrogen (H₂). The reaction is exothermic, releasing heat as zinc reacts with hydrochloric acid.

Questions:

1. Write the chemical equation for the reaction between zinc and hydrochloric acid.

2. What gas is produced in this reaction?

3. Why is the reaction exothermic?

4. What would you observe if the gas is tested with a lit match?

5. What happens to the zinc after the reaction?

Case Study 5: Balancing Chemical Equations

Case Study:
In a chemistry class, a teacher demonstrates the importance of balancing chemical equations. She writes the unbalanced equation for the reaction between sodium hydroxide (NaOH) and hydrochloric acid (HCl). The reaction produces sodium chloride (NaCl) and water (H₂O). The students are asked to balance the equation.

Questions:

1. Write the unbalanced equation for the reaction between sodium hydroxide and hydrochloric acid.

2. Balance the chemical equation for this reaction.

3. Why is it important to balance chemical equations?

4. What does the Law of Conservation of Mass state regarding chemical reactions?

5. What type of reaction is this?

Case Study 6: Heating of Copper Sulphate

Case Study:
A student heats copper sulphate (CuSO₄) crystals in a test tube. The color of the copper sulphate changes from blue to white. Upon adding a few drops of water to the white powder, the blue color reappears. The student concludes that the reaction is a physical change followed by a chemical change.

Questions:

1. What happens to copper sulphate when it is heated?

2. What is the chemical reaction that occurs when copper sulphate is heated?

3. What does the change in color indicate about the reaction?

4. Why is the change from blue to white and back to blue considered a physical change and not a chemical one?

5. Write the balanced chemical equation for the thermal decomposition of copper sulphate.

Case Study 7: Neutralization Reaction

Case Study:
A student is asked to neutralize an acid solution using a base. The student prepares a solution of sodium hydroxide (NaOH) and adds it slowly to a solution of hydrochloric acid (HCl). The solution turns neutral after adding an appropriate amount of sodium hydroxide. The pH of the resulting solution is 7.

Questions:

1. What type of chemical reaction is occurring when sodium hydroxide reacts with hydrochloric acid?

2. Write the balanced chemical equation for this neutralization reaction.

3. What is the pH of the neutral solution?

4. Why is the reaction between an acid and a base called neutralization?

5. What are the products formed in this reaction?

Case Study 8: Formation of Ammonium Chloride

Case Study:
In a laboratory, a student performs an experiment by reacting ammonia (NH₃) gas with hydrochloric acid (HCl) gas. The result is the formation of ammonium chloride (NH₄Cl), which appears as a white solid.

Questions:

1. What type of chemical reaction is demonstrated in this experiment?

2. Write the balanced chemical equation for the formation of ammonium chloride.

3. What is the physical state of the product formed in this reaction?

4. Why does the reaction produce a white solid?

5. What is the role of ammonia in this reaction?

These case studies help assess your understanding of different types of chemical reactions, their characteristics, and how they apply in real-world scenarios. Make sure to carefully read the case study and apply your knowledge of the chapter to answer the questions accurately.

Let me know if you need further explanations or additional questions!

Case Study Questions for Class 10 Science Chapter 1

SCIENCE- Class X Sample Case Studies