Podcast Beta
Questions and Answers
Which iron compound has oxidation that is difficult under normal conditions?
When heated in air, which iron compound forms iron III oxide upon thermal decomposition?
Which process can be used to differentiate between iron II oxide and iron III oxide?
Which sulfate salt of iron can be produced by reacting iron III oxide with concentrated sulfuric acid?
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What is the magnetic moment comparison between the compounds formed from heating iron II oxalate and the subsequent reaction with concentrated hot sulfuric acid?
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What is the solid substance produced from the reduction of Fe2O3 at 880°C?
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What products are formed when hot concentrated H2SO4 reacts with the solid produced from the reduction of Fe2O3?
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Which statement is incorrect concerning the salts produced from the reaction of iron with dilute hydrochloric acid and dilute sulfuric acid?
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What is the correct sequence of processes to obtain iron II sulfide from iron II sulfate?
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Which oxide is described as a black oxide that cannot react with dilute acids?
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Which acid will react with iron the fastest when equal volumes are used?
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The products of reacting diluted sulphuric acid with a mixture of iron (II) oxide and iron (III) oxide will include which of the following?
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Which product is unique to the reaction of concentrated sulfuric acid with iron compared to iron oxides?
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Heating iron oxide in air until redness primarily results in a reaction with which acid?
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Which method is appropriate for obtaining red iron oxide?
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Study Notes
Iron Compounds
- Iron (II) oxide (FeO) is difficult to oxidize under normal conditions.
- Iron (III) oxide (Fe2O3) can be reduced thermally in the absence of air to form iron (II) oxide and two other oxides
- Iron (III) oxide is produced from iron (II) oxide by reacting with concentrated sulfuric acid.
- Iron (III) oxide cannot be further oxidized under normal conditions.
Identifying Iron Oxides
- To differentiate between iron (II) oxide and iron (III) oxide, a strong alkaline solution can be used.
- Iron fillings can be used to differentiate between concentrated sulphuric acid and concentrated nitric acid.
Reactions of Iron and Iron Compounds
- Dilute hydrochloric acid reacts with iron faster than other acids mentioned.
- When dilute sulphuric acid is added to a mixture of iron (II) oxide and iron (III) oxide, the reaction produces iron (II) sulphate, iron (III) oxide, and water.
- Concentrated H2SO4 reacts with iron to produce SO2, which is not produced when reacting with mixed oxide.
- Heating iron in air to redness produces iron (III) oxide.
- Heating iron (III) hydroxide and reducing the product at temperatures higher than 700°C results in the formation of iron.
- The solid substance produced by reducing Fe2O3 at 880°C reacts with hot concentrated H2SO4 to produce FeSO4, Fe2(SO4)3, SO2, and water vapor.
- Iron (II) salts are paramagnetic and their solutions have the same color.
- The correct order of processes needed to obtain iron (II) sulfide from iron (II) sulfate is thermal decomposition, reduction, and reaction with sulfur.
Iron Oxides X, Y, and Z
- X is a black oxide that cannot react with dilute acids.
- Y is a black oxide that can react with both concentrated and dilute acids.
- Z is a red oxide that cannot be oxidized under normal conditions.
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Description
This quiz covers the properties and reactions of various iron compounds, focusing on iron (II) oxide and iron (III) oxide. It explores their behavior in different chemical environments and how to distinguish between them. Test your knowledge on the reactions involving these iron oxides and acids.
