Chemical Reactions & Equations Quiz
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Questions and Answers

Which compound is produced when magnesium carbonate reacts with water?

  • Magnesium sulphate
  • Magnesium hydroxide (correct)
  • Magnesium chloride
  • Magnesium oxide

What is the correct volume ratio of hydrogen to oxygen in water?

  • 1:1
  • 1:8
  • 2:1 (correct)
  • 1:2

What type of electrodes are used in the described electrolysis activity?

  • Aluminum
  • Graphite (correct)
  • Coke
  • Copper

Where is hydrogen gas specifically collected during the electrolysis of water?

<p>Cathode (A)</p> Signup and view all the answers

Which of the following processes is classified as endothermic?

<p>Electrolysis (C)</p> Signup and view all the answers

What occurs when hydrogen gas is passed over heated copper oxide?

<p>A reduction reaction occurs. (C)</p> Signup and view all the answers

What is a common effect of oxidation in metals?

<p>Formation of rust or oxides. (B)</p> Signup and view all the answers

Which of the following is a prevention method for rancidity?

<p>Storing food in airtight containers. (A)</p> Signup and view all the answers

What type of reaction is respiration classified as?

<p>Exothermic reaction (C)</p> Signup and view all the answers

What is the process of corrosion primarily caused by?

<p>Chemical reactions with environmental substances. (D)</p> Signup and view all the answers

Which statement best describes rancidity?

<p>The spoilage of fats and oils due to oxidation. (C)</p> Signup and view all the answers

In the process of oxidation, what happens to the compound?

<p>It loses electrons (D)</p> Signup and view all the answers

Why does oxidation impact the shelf life of food products?

<p>It results in unpleasant tastes and smells. (B)</p> Signup and view all the answers

Which of the following equations represents an oxidation reaction?

<p>4Na + O₂ → 2Na₂O (A), H₂S + O₂ → H₂O + SO₂ (C)</p> Signup and view all the answers

What type of reaction is respiration considered to be?

<p>Exothermic reaction. (C)</p> Signup and view all the answers

What is the black-colored compound formed when copper is heated in air?

<p>Copper oxide (D)</p> Signup and view all the answers

What is produced when potassium chlorate is heated?

<p>Oxygen and potassium chloride (B)</p> Signup and view all the answers

Why is silver chloride stored in dark-colored bottles?

<p>To block exposure to light (D)</p> Signup and view all the answers

What can be a direct result of corrosion in metals?

<p>Weakened metal structure. (D)</p> Signup and view all the answers

When electricity is passed through molten sodium chloride, what are the products formed?

<p>Sodium and chlorine (D)</p> Signup and view all the answers

Which of the following best describes the thermal decomposition of potassium chlorate?

<p>It decomposes into potassium chloride and oxygen (A)</p> Signup and view all the answers

In which reaction does a compound lose oxygen?

<p>CuO + H₂ → Cu + H₂O (B)</p> Signup and view all the answers

Which of the following statements is true about a displacement reaction?

<p>A more reactive substance replaces a less reactive substance. (C)</p> Signup and view all the answers

What is the primary product of respiration besides ATP?

<p>Water (A)</p> Signup and view all the answers

What distinguishes a double displacement reaction from a displacement reaction?

<p>Two displacements occur between two compounds (B)</p> Signup and view all the answers

Why does zinc liberate hydrogen gas when reacted with dilute hydrochloric acid, but copper does not?

<p>Zinc is more reactive than copper. (A)</p> Signup and view all the answers

What is the purpose of rubbing a magnesium ribbon before burning it?

<p>To remove oxide coating. (D)</p> Signup and view all the answers

What is the chemical name of the powder produced when magnesium burns?

<p>Magnesium oxide (D)</p> Signup and view all the answers

What is the color of a fresh magnesium ribbon?

<p>White (B)</p> Signup and view all the answers

What is produced when calcium oxide reacts with water?

<p>Calcium hydroxide (A)</p> Signup and view all the answers

What type of reaction is represented by the equation 2H2 + O2 → 2H2O?

<p>Combination Reaction (D)</p> Signup and view all the answers

Which of the following describes an exothermic reaction?

<p>One that releases heat (C)</p> Signup and view all the answers

In the decomposition of calcium carbonate (CaCO3), what are the products formed?

<p>Calcium oxide and carbon dioxide (B)</p> Signup and view all the answers

When calcium hydroxide reacts with carbon dioxide, which product is formed?

<p>Calcium carbonate (B)</p> Signup and view all the answers

Which of the following is an example of a decomposition reaction?

<p>2FeSO4 → Fe2O3 + SO2 + SO3 (A)</p> Signup and view all the answers

Which reaction involves the combination of two or more reactants to form a single product?

<p>2H2 + O2 → 2H2O (A)</p> Signup and view all the answers

What is the primary characteristic of a combination reaction?

<p>Forms a single product from multiple reactants (D)</p> Signup and view all the answers

What must be true for an equation to be considered balanced?

<p>The number of atoms of each element must be equal on both sides. (A)</p> Signup and view all the answers

What does the Law of Conservation of Mass state?

<p>The mass of reactants equals the mass of products. (D)</p> Signup and view all the answers

Which step should be taken first when balancing a chemical equation?

<p>List the number of atoms of elements in the unbalanced equation. (C)</p> Signup and view all the answers

In the experiment involving zinc granules and sulfuric acid, what observable evidence indicates the formation of hydrogen gas?

<p>Bubbles are produced and burn with a popping sound. (C)</p> Signup and view all the answers

What is the initial color change observed when potassium iodide is added to lead nitrate solution?

<p>Colorless to yellow (D)</p> Signup and view all the answers

What does the reaction between zinc and dilute sulfuric acid primarily produce?

<p>Hydrogen gas (A)</p> Signup and view all the answers

When balancing an equation, which compound should be balanced first?

<p>The compound with the maximum number of atoms. (A)</p> Signup and view all the answers

What happens to the temperature of the flask in the zinc and sulfuric acid experiment?

<p>It increases, indicating an exothermic reaction. (D)</p> Signup and view all the answers

Flashcards

Combination Reaction

A chemical reaction where two or more reactants combine to form a single product. Example: 2H2 + O2 → 2H2O

Decomposition Reaction

A chemical reaction where a single reactant breaks down into two or more products. Example: CaCO3 (s) → CaO(S) + CO2

Exothermic Reaction

Chemical reactions that release heat energy into the surroundings. Example: CaO + H2O → Ca(OH)2

Endothermic Reaction

Chemical reactions that absorb heat energy from the surroundings.

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Balanced Chemical Equation

A chemical equation where the number of atoms of each element on the reactant side is equal to the number of atoms of that element on the product side.

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Oxidation

A chemical reaction where a substance gains oxygen or loses hydrogen.

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Law of Conservation of Mass

The principle stating that the total mass of the reactants in a chemical reaction is equal to the total mass of the products.

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Reduction

A chemical reaction where a substance loses oxygen or gains hydrogen.

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Corrosion

The gradual destruction of metals by chemical reactions with substances like moisture and acids, often forming an oxide on the surface.

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Rancidity

The spoilage of fats and oils in food, resulting in unpleasant taste and smell due to oxidation.

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Reactant

The substance being changed in a chemical reaction.

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Product

The substance formed in a chemical reaction.

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Respiration

The process of breaking down food molecules in living organisms to release energy.

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Stoichiometric Coefficient

A coefficient in a balanced chemical equation indicating the relative number of molecules or formula units involved in the reaction.

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Balancing Chemical Equations

The process of adjusting the stoichiometric coefficients in a chemical equation to ensure an equal number of atoms of every element on both sides of the equation.

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Photolytic decomposition

The decomposition of a substance due to exposure to light.

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Thermal decomposition

A reaction where a substance breaks down into simpler substances by supplying heat.

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Photosensitive compound

A compound that absorbs light energy.

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What compound is formed when magnesium carbonate reacts with water?

Magnesium hydroxide is formed when magnesium carbonate reacts with water.

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Displacement Reaction

A chemical reaction where a more reactive element replaces a less reactive element in a compound.

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Double Displacement Reaction

A chemical reaction where two reactants exchange ions to form two new products.

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What is the volume ratio of hydrogen to oxygen in water?

The volume ratio of hydrogen to oxygen in water is 2:1. This means that for every two volumes of hydrogen, there is one volume of oxygen.

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Which electrodes are used in the electrolysis of water?

Graphite electrodes are used in the electrolysis of water. Graphite is a good conductor of electricity and is resistant to corrosion.

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Where is hydrogen gas collected in electrolysis of water?

Hydrogen gas is collected at the cathode during the electrolysis of water. The cathode is the negative electrode where reduction takes place.

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Photodecomposition (Photolysis)

A decomposition reaction that occurs when light is applied.

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Which process is endothermic: electrolysis or condensation?

Electrolysis is an endothermic process which requires energy to break the bonds in water molecules. It is not a spontaneous reaction.

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Electrolytic Decomposition (Electrolysis)

This reaction involves the breakdown of a compound using electricity.

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Reactivity of Metals

The tendency of a metal to lose electrons and form positive ions.

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Activity Series of Metals

A series of metals arranged in order of their decreasing reactivity.

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Study Notes

Chemical Reactions & Equations

  • Chemical reactions involve the transformation of one or more substances into different substances.
  • Examples include rusting of iron, setting of milk, digestion, and respiration.
  • Chemical reactions are indicated by chemical changes.
  • Chemical equations represent chemical reactions using symbols and formulae of reactants and products.
  • Characteristics of chemical reactions include: formation of new substances, change in colour, evolution/absorption of heat, formation of precipitate, change in state of matter, and change in energy.

Balancing Chemical Equations

  • A balanced chemical equation has an equal number of atoms of each element on both sides of the equation.
  • The law of conservation of mass states that mass of reactants equals mass of products.
  • To balance an equation, adjust coefficients in front of chemical formulas to balance the number of atoms of each element.

Types of Chemical Reactions

  • Combination reactions: Two or more reactants combine to form a single product.
    • Example: Formation of water (2Hâ‚‚ + Oâ‚‚ → 2Hâ‚‚O)
  • Decomposition reactions: A single reactant decomposes into two or more products.
    • Example: Decomposition of calcium carbonate (CaCO₃ → CaO + COâ‚‚)
  • Displacement reactions: A more reactive element displaces a less reactive element from its compound.
    • Example: Zinc displacing copper from copper sulfate (Zn + CuSOâ‚„ → ZnSOâ‚„ + Cu)
  • Double displacement reactions: Two ionic compounds react by exchanging ions to form two new compounds.
    • Example: Sodium sulfate and barium chloride reacting to form barium sulfate and sodium chloride (Naâ‚‚SOâ‚„ + BaClâ‚‚ → BaSOâ‚„ + 2NaCl)

Effects of Oxidation Reactions

  • Corrosion: Gradual destruction of metals due to chemical reaction with their environment (e.g., rusting of iron).
  • Rancidity: Spoilage of fats and oils in food due to oxidation.
  • Prevention methods for corrosion and rancidity involve coating, proper storage conditions etc

Oxidation and Reduction

  • Oxidation: Gain of oxygen or loss of hydrogen.
  • Reduction: Loss of oxygen or gain of hydrogen.
  • Redox reactions involve both oxidation and reduction.
  • Examples include reactions involving oxygen and hydrogen.

Experiments and Activities

  • Several activities and experiments are described showcasing chemical reactions and their observations. These illustrate different types of reactions.

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Chemical Reactions & Equations Class 10 Notes PDF

Description

Test your understanding of chemical reactions and equations. This quiz covers the types of chemical reactions, balancing equations, and the characteristics of chemical changes. Dive into topics like the law of conservation of mass and various examples of chemical transformations.

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