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Adding distilled water to the test tube in Activity 1.7 before immersing the electrodes is a part of the procedure.
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.
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.
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.
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.
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.
Mixing sodium sulphate and barium chloride results in the formation of a precipitate.
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Sodium chloride is insoluble in water.
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.
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.
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.
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.
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.
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.
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.
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.
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.
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.
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.
Keeping food in air-tight containers helps slow down oxidation.
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Rusting of iron is an example of a reduction reaction.
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.
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.
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.
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.
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.
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).
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.
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.
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.
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.
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.
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.
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.
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.
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.
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.
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.
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.
