Chemistry Activity 1.7 Quiz

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Questions and Answers

What is the chemical formula for the gas emitted when lead nitrate is heated?

  • N2
  • NO2 (correct)
  • N2O
  • NO

What is the name of the process used in Activity 1.7 to decompose water?

  • Filtration
  • Sublimation
  • Distillation
  • Electrolysis (correct)

Which of the following is NOT a product of the decomposition of lead nitrate?

  • Lead oxide (PbO)
  • Nitric acid (HNO3) (correct)
  • Nitrogen dioxide (NO2)
  • Oxygen (O2)

What is the purpose of the carbon electrodes in Activity 1.7?

<p>To provide a pathway for the flow of electricity (A)</p> Signup and view all the answers

Why is it important to add dilute sulphuric acid to the water in Activity 1.7?

<p>To increase the conductivity of the water (C)</p> Signup and view all the answers

What observation would indicate that a burning candle is being extinguished by the gas collected in one of the test tubes in Activity 1.7?

<p>The candle flame goes out (B)</p> Signup and view all the answers

Which of the following statements accurately describes the volume of gas collected in each test tube in Activity 1.7?

<p>The volume of gas collected in one test tube is twice the volume collected in the other (D)</p> Signup and view all the answers

What is the purpose of the rubber stoppers in the holes of the plastic mug in Activity 1.7?

<p>To hold the electrodes in place (D)</p> Signup and view all the answers

What happens to the magnesium ribbon when it is burned?

<p>It transforms into magnesium oxide. (A)</p> Signup and view all the answers

Which of the following scenarios is an example of a chemical change?

<p>Cooking food. (D)</p> Signup and view all the answers

What is produced when magnesium reacts with oxygen?

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

Which activity illustrates a change in the identity of a substance due to a chemical reaction?

<p>Fermenting grapes. (D)</p> Signup and view all the answers

In which condition do chemical reactions typically occur?

<p>Under various temperatures and pressures. (D)</p> Signup and view all the answers

What could be an observation of magnesium ribbon burning in air?

<p>It burns with a dazzling white flame. (D)</p> Signup and view all the answers

Which statement best describes a physical change?

<p>It involves a change of state without altering composition. (D)</p> Signup and view all the answers

Which of the following is a common indicator of a chemical reaction?

<p>Formation of a gas. (B)</p> Signup and view all the answers

What is the final balanced equation after all steps?

<p>3 Fe + 4 H2O → Fe3O4 + 4 H2 (A)</p> Signup and view all the answers

Which element was the last to be balanced in the equation?

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

What does the hit-and-trial method involve when balancing equations?

<p>Balancing only one element at a time (A)</p> Signup and view all the answers

What notation indicates a substance in a gaseous state in a chemical equation?

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

Why is it important to include physical states in a balanced equation?

<p>To communicate the properties of reactants and products (B)</p> Signup and view all the answers

In the balanced equation 3Fe(s) + 4H2O(g) → Fe3O4(s) + 4H2(g), what does the (g) next to H2O signify?

<p>Water is present as steam (C)</p> Signup and view all the answers

How many hydrogen atoms are present in the reactants of the balanced equation?

<p>8 (A)</p> Signup and view all the answers

What will be the number of iron atoms on the left-hand side of the equation after balancing?

<p>3 (A)</p> Signup and view all the answers

Why are physical states usually not included in chemical equations?

<p>They are only needed when specified (A)</p> Signup and view all the answers

What color change occurs to the copper sulphate solution after the iron nails are immersed?

<p>It loses its blue color (A)</p> Signup and view all the answers

What are the coefficients used for balancing the equation?

<p>3 for Fe and 4 for H2O (C)</p> Signup and view all the answers

What represents an aqueous state of a substance in chemical reactions?

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

What happens to the iron nail when placed in copper sulphate solution?

<p>It becomes brownish (C)</p> Signup and view all the answers

In a chemical equation, what does the notation above and below the arrow typically indicate?

<p>Reaction conditions like temperature and pressure (C)</p> Signup and view all the answers

What is the main outcome of balancing a chemical equation?

<p>To create equal numbers of atoms of each element on both sides (C)</p> Signup and view all the answers

Which of the following reactions shows the formation of an insoluble product?

<p>Barium chloride + Aluminium sulphate → Barium sulphate + Aluminium chloride (B)</p> Signup and view all the answers

In the reaction between iron and copper sulphate, which substance is displaced?

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

What is the state symbol for liquid water in a chemical equation?

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

What type of reaction occurs when iron displaces copper from copper sulphate solution?

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

Which of the following elements is more reactive than copper and can displace it?

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

What is produced when sodium reacts with water?

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

What is the formula for iron sulphate produced in the reaction?

<p>FeSO4 (B)</p> Signup and view all the answers

After the reaction, what happens to the copper in the solution?

<p>It precipitates out as solid copper (B)</p> Signup and view all the answers

In the reaction Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s), which substances are reactants?

<p>Fe and CuSO4 (C)</p> Signup and view all the answers

What gases are produced when potassium metal reacts with water?

<p>Potassium hydroxide and hydrogen (B)</p> Signup and view all the answers

What type of reaction occurs when barium chloride reacts with potassium sulfate?

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

Which equation represents a decomposition reaction?

<p>Zinc carbonate(s) → Zinc oxide(s) + Carbon dioxide(g) (D)</p> Signup and view all the answers

What defines an exothermic reaction?

<p>It releases thermal energy. (D)</p> Signup and view all the answers

What type of reaction is represented by the equation: Hydrogen(g) + Chlorine(g) → Hydrogen chloride(g)?

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

Which reaction is an example of a double displacement reaction?

<p>Barium chloride + Potassium sulfate → Barium sulfate + Potassium chloride (B)</p> Signup and view all the answers

In which scenario does reduction occur?

<p>Gain of hydrogen (A)</p> Signup and view all the answers

What products are formed when hydrogen sulfide gas burns in air?

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

Flashcards

Chemical Reaction

A process where substances undergo a transformation to form new substances.

Physical Change

A change that affects one or more physical properties but doesn't alter the substance's identity.

Chemical Change

A change that produces one or more new substances, altering the identity of the original.

Magnesium Oxide

A white powder formed from the reaction of magnesium and oxygen.

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Burning of Magnesium

A reaction that produces a dazzling flame and magnesium oxide.

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Lead Nitrate

A chemical compound used in reactions to demonstrate chemical changes.

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Zinc Granules

Small pieces of zinc used in experiments with acids.

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Acids in Reactions

Substances that can react with metals, producing gases and other products.

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State notations

Symbols (g), (l), (aq), (s) represent states of matter in reactions.

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Aqueous solution

A solution where a substance is dissolved in water, indicated by (aq).

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Balanced chemical equation

Equation where the number of each type of atom is equal on both sides.

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Physical states in equations

Physical states of reactants/products are often noted in chemical equations.

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Reaction conditions

Conditions such as temperature, pressure, or catalyst shown above/below the arrow.

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Example of water as steam

H2O(g) indicates water vapor in the reaction environment.

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Catalysts in reactions

Substances that speed up a reaction without being consumed.

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Insoluble product

A substance that cannot dissolve in water, often forms during reactions.

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Displacement Reaction

A reaction where one element replaces another in a compound.

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Copper Sulphate Solution

A blue solution containing copper ions in water.

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Iron Nail Reaction

Iron nails turn brownish after reacting with copper sulphate.

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Color Change in Solution

The blue color of copper sulphate fades as iron displaces copper.

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Iron Displacing Copper

In the reaction, iron replaces copper in copper sulphate.

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Chemical Equation (1.24)

Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s); iron reacts with copper sulphate.

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Reactivity Series

Zinc and lead are more reactive than copper and can displace it.

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Test Tube Experiment

Test tubes A and B are used to observe reactions of iron with copper sulphate.

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Decomposition Reaction

A type of chemical reaction where a single compound breaks down into two or more products.

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Nitrogen Dioxide (NO2)

A brown gas released during the decomposition of lead nitrate when heated.

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Reaction Equation

The chemical equation showing the breakdown of lead nitrate into lead oxide, nitrogen dioxide, and oxygen.

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Electrolysis of Water

A process that uses electricity to separate water into hydrogen and oxygen gases.

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Carbon Electrodes

Conductive materials used in electrolysis to facilitate the conduction of electricity.

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Candle Test for Gases

A method to identify gases by observing the effect of a flame.

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Sulphuric Acid in Electrolysis

A strong acid used to improve conductivity in the electrolysis setup.

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Hydrogen Sulphide Reaction

Burns in air to produce water and sulfur dioxide.

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Barium Chloride Reaction

Barium chloride reacts with aluminum sulfate to form aluminum chloride and barium sulfate precipitate.

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Potassium and Water Reaction

Potassium reacts with water to give potassium hydroxide and hydrogen gas.

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Exothermic Reaction

Releases heat during the reaction process.

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Endothermic Reaction

Absorbs heat from the surroundings.

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Double Displacement Reaction

Two compounds exchange parts to form two new compounds.

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Precipitation Reaction

Involves the formation of an insoluble solid from a solution.

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Partly Balanced Equation

An unbalanced chemical equation where some elements' atoms are not equal on both sides.

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Balancing Hydrogen

Adjusting the number of hydrogen molecules to have equal hydrogen atoms on both sides of the equation.

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Final Balanced Equation

The complete equation where the number of atoms for each element is the same on both sides.

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Iron Balancing Step

Adjusting the quantity of iron to match both sides of the equation during balancing.

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Hit-and-Trial Method

A balancing method involving trials to find the smallest whole number coefficients for the equation.

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Counting Atoms

The process of ensuring equal numbers of each type of atom on both sides of a chemical equation.

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Water Molecule Contribution

The contribution of water (H2O) to the number of hydrogen atoms in the equation.

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Study Notes

Chemical Reactions and Equations

  • Chemical reactions involve changes in the nature and identity of substances.
  • Chemical reactions involve changes in state, color, formation of gas, and changes in temperature.
  • A chemical reaction occurs when chemical bonds are broken and new chemical bonds are formed.
  • A chemical reaction is represented by a chemical equation.
  • Chemical equations represent reactions concisely, using chemical formulas instead of words.
  • In a chemical equation, reactants appear on the left side and products on the right side, separated by an arrow.
  • Chemical equations must be balanced, meaning the same number of atoms of each element are on both sides of the equation. This follows the law of conservation of mass.
  • Different types of chemical reactions include combination, decomposition, displacement, and double displacement reactions.

Activity 1.1: Magnesium in Air

  • This activity demonstrates a chemical reaction: magnesium burning in air.
  • A magnesium ribbon is cleaned using sandpaper, then held with tongs and burned with a spirit lamp or burner.
  • Ash is collected in a watch glass.
  • Observation: magnesium ribbon burns with a dazzling white flame and forms a white powder (magnesium oxide).

Activity 1.2: Lead Nitrate and Potassium Iodide

  • This activity demonstrates a reaction resulting in a precipitate (a solid that forms from a solution).
  • Lead nitrate solution is added to potassium iodide solution.
  • Observation: a yellow precipitate forms.

Activity 1.3: Zinc and Hydrochloric Acid

  • This activity demonstrates a chemical reaction producing a gas.
  • Zinc granules are added to hydrochloric or sulfuric acid.
  • Observation: bubbles form, and the test tube or flask warms up.

1.1 Chemical Equations

  • Chemical equations concisely represent chemical changes.
  • Reactants are the starting substances; products are the resulting substances.
  • Word equations show the reaction using words.
  • Chemical equations show the change in formulas.

1.1.1 Writing a Chemical Equation

  • Chemical equations use chemical formulas instead of words.
  • The number of atoms of each element must be balanced.

1.1.2 Balanced Chemical Equations

  • The law of conservation of mass dictates that the total mass of reactants equals the total mass of products.
  • Balanced equations have equal numbers of atoms of each element on both sides.

Activity 1.4: Calcium Oxide and Water

  • Calcium oxide (quicklime) reacts vigorously with water to produce calcium hydroxide (slaked lime).
  • The reaction releases significant heat, making it an exothermic process.

1.2 Types of Chemical Reactions

  • Combination Reactions: Two or more reactants form a single product.
  • Decomposition Reactions: A single reactant breaks down into two or more products.
  • Displacement Reactions: More reactive element displaces a less reactive element from a compound.
  • Double Displacement Reactions: A reaction where ions exchange places between two compounds. This often results in the formation of a precipitate.

Activity 1.5: Ferrous Sulphate Decomposition

  • Ferrous sulphate crystals decompose into ferric oxide, sulphur dioxide, sulphur trioxide, and gaseous water when heated.
  • Observation: color change and odour production.

Activity 1.6: Lead Nitrate Decomposition

  • Lead nitrate decomposes into lead oxide, nitrogen dioxide, and oxygen when heated.
  • Observation: emission of brown fumes, color change.

Activity 1.7: Electrolysis of Water

  • Electrolysis is a technique of using a direct electric current to drive a non-spontaneous chemical reaction.
  • Water is split into hydrogen and oxygen using an electric current.

Activity 1.8: Silver Chloride in Sunlight

  • Silver chloride decomposes into silver and chlorine in sunlight.
  • Observation: silver chloride turns gray.

Activity 1.9: Iron and Copper Sulphate

  • Iron displaces copper from copper sulphate solution.
  • Observation: the color of copper sulphate solution changes, and iron nails become coated with copper.

Activity 1.10: Double Displacement

  • Sodium sulphate and barium chloride solutions react, forming insoluble barium sulphate precipitate.

1.2.5 Oxidation and Reduction

  • Oxidation: gain of oxygen or loss of hydrogen.
  • Reduction: loss of oxygen or gain of hydrogen
  • Reactions involving simultaneous oxidation and reduction are called redox reactions.

Questions

  • Various questions pertaining to the concepts covered in the notes are provided.

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