Class 10 Chemistry Sample Paper for CBSE Board Exams
Prepare for your Class 10 Science Board Examination with this challenging NCERT-based Class 10 Chemistry sample paper by The Busy Brains – Tuition Classes. This original practice paper covers Chemical Reactions and Equations, Acids, Bases and Salts, Metals and Non-metals, and Carbon and its Compounds.
Designed for students who want to move beyond routine textbook exercises, this Class 10 Chemistry question paper includes reasoning-based MCQs, assertion–reason questions, unfamiliar chemical situations, identification of substances from experimental observations, balanced chemical equations, electron-dot structures and numerical problems involving chemical reactions.
The questions draw inspiration from challenging school-examination formats while using independently written wording and contexts. Students will need to interpret observations, apply the reactivity series, analyse chemical behaviour, explain scientific principles and connect different NCERT concepts.
Use this CBSE Class 10 Chemistry practice paper for Board and Pre-Board exams under timed conditions. The paper is an independent educational resource and is not an official CBSE sample paper or a guarantee of questions appearing in the examination.
Class 10 Chemistry
Advanced Board Practice Paper
NCERT-Based Questions for CBSE Board & Pre-Board Preparation
Higher-Order Thinking Application-Based 80 Marks- All five sections are compulsory.
- Read each question carefully and observe the marks allotted.
- Write balanced chemical equations wherever required.
- Use appropriate chemical formulae, symbols and state symbols.
- For observation-based questions, state both the observation and the scientific inference when asked.
- Show all essential calculation steps in numerical questions.
- This is an advanced practice paper; some questions require more than one step of reasoning.
Assertion (A): A reaction in which one substance breaks into two or more simpler substances can be classified as a decomposition reaction.
Reason (R): Decomposition reactions may be brought about by heat, light or electricity.
Assertion (A): Aqueous sodium carbonate solution is basic in nature.
Reason (R): Sodium carbonate is a salt formed from a strong base and a weak acid.
(a) Fe + H₂O (steam) → Fe₃O₄ + H₂
(b) Pb(NO₃)₂ → PbO + NO₂ + O₂
(a) CH₃CH₂OH
(b) CH₃COOH
(a) Name the gas released. (1)
(b) Write the balanced equation for the reaction of calcium carbonate with hydrochloric acid. (1)
(c) Explain why the gas turns lime water milky. (1)
(a) Identify the acidic, neutral and basic solutions. (1)
(b) Which solution would be most suitable for neutralising a small quantity of dilute hydrochloric acid, assuming an appropriate amount is used? (1)
(c) Explain why dilution of an acid with water generally raises its pH. (1)
(a) State two visible changes expected during the reaction. (1)
(b) Write the balanced chemical equation. (1)
(c) Explain the change in terms of relative reactivity and electron transfer. (1)
(a) Write the balanced equation for the reaction of aluminium with oxygen. (1)
(b) Explain how the surface layer formed influences the metal's resistance to further corrosion. (1)
(c) Name the general category of this type of protective oxide layer in the context of aluminium oxide's chemical behaviour. (1)
(a) Write the balanced combustion equation for propane, C₃H₈. (1)
(b) Explain why sufficient oxygen is important for complete combustion. (1)
(c) State one environmental or health concern associated with incomplete combustion of carbon-containing fuels. (1)
(a) Identify A and B. (1)
(b) Write the equation for the reaction of A with sodium. (1)
(c) Write the equation for the reaction of B with sodium hydrogencarbonate. (1)
(a) Why are ionic compounds usually brittle? (1)
(b) Why is graphite able to conduct electricity even though it is a form of carbon? (1)
(c) Why do detergents generally perform better than soaps in hard water? (1)
(a) Balance the following equations. (2)
(i) Al + HCl → AlCl₃ + H₂
(ii) KClO₃ → KCl + O₂
(b) When 10.0 g of calcium carbonate reacts completely with excess hydrochloric acid, calculate the theoretical mass of carbon dioxide produced. (2)
Use: Ca = 40, C = 12, O = 16. Assume the sample is pure.
(c) Name the type of reaction in which calcium carbonate decomposes on heating. (1)
(a) A solution of sodium hydroxide is added to a solution containing zinc ions, first dropwise and then in excess. Describe the expected precipitate and explain its behaviour in excess alkali. (2)
(b) Write the balanced equation for the reaction of zinc with dilute sulphuric acid. State the gas evolved and one test for it. (2)
(c) Why is sodium extracted by electrolysis rather than by heating its oxide with carbon? (1)
(a) Draw the structural formulae of ethane and ethene. State the bonding difference between them. (2)
(b) An organic liquid reacts with sodium hydrogencarbonate and produces a gas that turns lime water milky. Identify the likely functional group and write a representative balanced equation. (2)
(c) State one reason why carbon forms such a large number of compounds. (1)
A laboratory contains three unlabelled solutions: dilute hydrochloric acid, sodium hydroxide and sodium carbonate. A student tests small samples using suitable indicators and then adds dilute hydrochloric acid to a fresh portion of each sample. One sample releases a gas that turns lime water milky, while another undergoes neutralisation without gas evolution.
(a) Which solution releases the gas when treated with hydrochloric acid? (1)
(b) Name the gas and write the balanced equation for its formation. (1)
(c) Which solution neutralises hydrochloric acid without producing a gas? Write the balanced equation. (1)
(d) Suggest one suitable indicator to distinguish the acidic solution from the sodium hydroxide solution. (1)
Three metal samples, P, Q and R, are tested. P displaces Q from its salt solution. R does not displace Q from its salt solution. An iron article is then coated with zinc to improve its resistance to corrosion.
(a) What does the first displacement observation tell you about P and Q? (1)
(b) What can be concluded about R relative to Q? (1)
(c) Name the process used to coat iron with zinc. (1)
(d) Explain why a zinc coating can protect iron from corrosion. (1)
Ethanol is oxidised under suitable conditions to form compound X. Compound X reacts with sodium hydrogencarbonate, releasing a gas. Another sample of ethanol is burned in air as a fuel.
(a) Identify compound X. (1)
(b) Name the gas evolved when X reacts with sodium hydrogencarbonate. (1)
(c) Write the balanced equation for this reaction. (1)
(d) Write the balanced equation for complete combustion of ethanol. (1)
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