A chemical reaction occurs when the bonds between reactant molecules are broken and new bonds are formed between product molecules to form a new substance. Chemical reactions can be found all around us, from the metabolism of food in our bodies to the light we receive from the sun.
Download Class 10 Chemistry Worksheet on Chapter 1 Chemical Reactions and Equations Set 1 PDF
CBSE Class 10 Chemistry Chapter 1 Chemical Reactions and Equations – Set 1
Q-1: Write the balanced chemical equations for each of the following reactions.
a) Liquid hydrogen peroxide decomposes to form water and oxygen gas.
b) Acetylene gas burns in oxygen to form carbon dioxide and water along with evolution of heat.
c) When solid mercury(II) oxide is heated, liquid mercury and oxygen gas are produced.
d) Marble dissolves in a hydrochloric acid to give calcium chloride, water and carbon dioxide.
e) Copper sulphate on treatment with potassium iodide precipitates cuprous iodide, liberates iodine gas and also forms potassium sulphate.
Q-2: Fill in the blanks
a) ________ is the magnetic oxide of iron.
b) In reactivity series, manganese lies _____ zinc
c) To the reaction between AgNO3 solution and NaCl solution, the names given to this type of reactions are _______ and _______.
d) Proteins decompose to form ______ in our body.
e) If copper turnings are added to colourless AgNO3 solution, it turns _________ after sometime.
Q-3: Which of the following displacement reactions will not take place?
a) Zn(s) + FeSO4(aq) → ZnSO4(aq) + Fe(s)
b) Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s)
c) Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq)+ 2Ag(s)
d) Cu(s) + FeSO4(aq) → CuSO4(aq) + Fe(s)
Q-4: Which of the following statements is false?
a) Oxidation results in the loss of an electropositive element and the gain of an electronegative element.
b) Reduction results in the loss of an electronegative element and the gain of an electropositive element.
c) A species that gains electrons is referred to as a reducing agent.
d) An oxidising agent is a type of specie that absorbs hydrogen atoms.
Q-5: Why are certain chemicals and medications kept in coloured bottles?
Q-6: Sakshi desired that her home be white washed. She went to the market and bought 20 kg of quick lime, which she dissolved in 60 litres of water. When she added lime to water, she noticed that the water began to boil even though it was not heated. Give an explanation for her observation. Name the product and write the corresponding chemical equation and word equation.
Q-7: State True and False. If False, state reasons.
a) In a closed vessel, the reaction between heated iron and steam is reversible.
b) Aluminium is highly corrosion resistant.
c) Strong heating of green FeSO4 crystals results in a FeO residue.
d) A chemical reaction is always accompanied by a temperature increase.
e) Respiration is the process by which glucose in the body is oxidised.
Q-8: Examples of decomposition reactions are provided below
2AgBr(s) → 2Ag(s) + Br2(g)
2H2O(l) → 2H2(g) + O2(g)
These reactions represent respectively
a) thermal decomposition, thermal decomposition
b) thermal decomposition, electrolytic decomposition
c) photolytic decomposition, electrolytic decomposition
d) photolytic decomposition, thermal decomposition
Q-9: Which of the following substances does not produce CO2 when exposed to dilute acid?
a) Lime
b) Limestone
c) Baking soda
d) Marble
Q-10: Match the applications in Column I with the chemical substances in Column II.
| Column I | Column II |
|---|---|
| A) Antacid | 1) Washing soda |
| B) Decolourisation | 2) Sodium chloride |
| C) Production of H2 and Cl2 | 3) Bleaching powder |
| D) Preparation of glass | 4) Baking soda |
Q-11: Classify the following reactions as decomposition, combination, displacement, or double displacement.
a) Cl2(g) +2NaBr(aq) → Br2 + 2NaCl (aq)
b) CaO(s) + H2O(l) → Ca(OH)2(aq)
c) Ni(NO3)2(aq) +2NaOH(aq) → Ni(OH)2↓ + 2NaNO3(aq)
d) 2CuO(s)→ 2Cu(s) + O2 (g)
e) 3MnO2 + 4Al → 3Mn + Al2O3
Q-12: What is rancidity? List two methods for preventing rancidity.
Q-13: What data can be extracted from the balanced chemical equations?
Statement for linked answer questions 14-17
It is common to notice that iron articles rust faster in wet weather than in dry weather. Silver articles, on the other hand, turn black in air in any season, and aluminium articles, when exposed to moist air, lose their lustre and their surface becomes dull after a while, and copper vessels become coated with a green layer. Iron sheets coated with zinc are frequently used to protect iron from rusting, such as in buckets and iron water pipes.
Q-14: Why is it rusting faster in the rainy season?
Q-15: Why do silver articles turn black in the air?
Q-16: Why does copper get coated with a green layer?
Q-17: Aluminium oxide is formed as a result of the attack of moist air on aluminium. How is this attack beneficial?
Q-18: The reactions that produce heat are known as
a) Endothermic reaction
b) Exothermic reaction
c) Thermal reactions
d) photochemical reactions
Q-19: Which of the following does not involve a chemical change?
a) Fermentation of grapes
b) Respiration
c) Condensation of water
d) Turning brown of a freshly cut apple in the air
Q-20: When white lead(II) nitrate powder is heated in a boiling tube, lead oxide, oxygen gas, and a brown gas(Y) are formed.
a) For the same, write a balanced chemical reaction.
b) Identify the brown gas Y evolved.
c) What is the pH range of Y’s aqueous solution?
d) Is lead oxide basic, acidic or amphoteric?
e) Identify the type of reaction.
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