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Questions and Answers
Adding distilled water to the test tube in Activity 1.7 before immersing the electrodes is a part of the procedure.
True
In Activity 1.6, holding the boiling tube with bare hands to observe the change is part of the steps.
False
The burning of a magnesium ribbon in Activity 1.5 is a recommended activity to observe the characteristics of thermal decomposition.
True
In Activity 1.8, the silver chloride remains unchanged when exposed to sunlight.
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Electrolysis of water was demonstrated in Activity 1.7.
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Mixing sodium sulphate and barium chloride results in the formation of a precipitate.
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Sodium chloride is insoluble in water.
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In a double displacement reaction, the anions and cations of two different molecules switch places.
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Barium sulphate is a soluble compound formed in the reaction between sodium sulphate and barium chloride.
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A reaction that produces a precipitate is always called a double displacement reaction.
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The reaction between barium hydroxide and ammonium chloride is an endothermic reaction.
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Ammonium chloride dissolves in water to form a basic solution.
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During a displacement reaction, a more reactive metal can displace a less reactive metal from its compound.
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Iron nails dipped in copper sulphate solution will show no observable reaction.
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The decomposition reactions used in black and white photography are typically endothermic.
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Corrosion only affects metals that come in contact with oxygen and moisture.
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Rancidity is prevented by adding acids to foods containing fats and oils.
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Keeping food in air-tight containers helps slow down oxidation.
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Rusting of iron is an example of a reduction reaction.
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Magnesium ribbon burns with a dazzling flame in air and forms magnesium oxide.
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The green color of ferrous sulfate crystals changes to red when heated.
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In a decomposition reaction, a single reactant breaks down into simpler products.
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Ferric oxide is produced as a gaseous product in the decomposition of ferrous sulfate.
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Calcium carbonate decomposes to form calcium oxide and carbon dioxide when heated.
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The brown fumes observed when heating lead nitrate are nitrogen dioxide (NO2).
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Adding dilute sulfuric acid to the solution in Activity 1.7 generates a greater volume of gas.
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The white color of silver chloride remains unchanged when exposed to sunlight.
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Thermal decomposition reactions are those that require heat to proceed.
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Sulfur trioxide (SO3) is a solid produced in the thermal decomposition reaction of ferrous sulfate.
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The gas collected at the electrodes in Activity 1.7 can be identified using a lighted match.
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A substance that gains oxygen during a reaction is said to be oxidised.
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When hydrogen gas is passed over heated copper (II) oxide, the black coating on the surface remains black.
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In the reaction ZnO + C → Zn + CO, carbon undergoes reduction.
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In the reaction CuO + H₂ → Cu + H₂O, hydrogen acts as a reducing agent.
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The reaction MnO₂ + 4HCl → MnCl₂ + 2H₂O + Cl₂ is an example of a redox reaction.
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Copper (II) oxide undergoes oxidation when hydrogen is passed over it.
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Study Notes
Decomposition Reaction
- A decomposition reaction is a type of reaction where a single reactant breaks down to give simpler products.
- Example: Ferrous sulphate (FeSO4) decomposes to ferric oxide (Fe2O3), sulphur dioxide (SO2), and sulphur trioxide (SO3) when heated.
- During decomposition, ferrous sulphate crystals (FeSO4·7H2O) lose water and change color.
- Another important decomposition reaction is the thermal decomposition of calcium carbonate to calcium oxide and carbon dioxide, which is used in various industries.
Activity 1.6
- Lead nitrate powder (Pb(NO3)2) decomposes to lead oxide, nitrogen dioxide (NO2), and oxygen when heated.
- The decomposition produces brown fumes of nitrogen dioxide.
Activity 1.7
- Electrolysis of water using carbon electrodes and a battery produces hydrogen and oxygen gases.
- Hydrogen gas is highly flammable and can be identified by the "pop" sound it produces when a lighted match is brought near it.
Activity 1.8
- Silver chloride (AgCl) decomposes to silver and chlorine when exposed to sunlight.
- The decomposition of silver chloride is an example of a photochemical decomposition reaction.
Double Displacement Reaction
- A double displacement reaction is a type of reaction where two compounds exchange partners, resulting in the formation of two new compounds.
- Example: Sodium sulphate (Na2SO4) and barium chloride (BaCl2) react to form barium sulphate (BaSO4) and sodium chloride (NaCl).
- The reaction produces a precipitate, which is an insoluble substance formed during a reaction.
Oxidation and Reduction
- Oxidation is the process of adding oxygen to a substance, while reduction is the process of removing oxygen from a substance.
- Example: Copper (Cu) is oxidized to copper oxide (CuO) when heated in the presence of oxygen, and reduced back to copper when hydrogen gas is passed over it.
- Oxidation and reduction reactions occur simultaneously and are known as redox reactions.
- A reducing agent undergoes oxidation, while an oxidizing agent undergoes reduction.
- Examples of redox reactions include ZnO + C → Zn + CO and MnO₂ + 4HCl → MnCl₂ + 2H₂O + Cl₂.
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Description
Observe the decomposition reaction of ferrous sulfate crystals through heating and note the changes in color and odor. Identify the reaction that takes place.
