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4Fe+3O(2) rarr 2Fe(2)O(3) (reference to ...

`4Fe+3O_(2) rarr 2Fe_(2)O_(3)` (reference to iron )

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To analyze the reaction \(4Fe + 3O_2 \rightarrow 2Fe_2O_3\) with reference to iron, we will follow these steps: ### Step 1: Identify the oxidation states of the elements in the reaction. - In the reactants, elemental iron (Fe) has an oxidation state of 0 because it is in its elemental form. - Oxygen (O) in \(O_2\) also has an oxidation state of 0 because it is in its elemental form. ### Step 2: Determine the oxidation state of iron in the product \(Fe_2O_3\). - In \(Fe_2O_3\), let the oxidation state of iron be \(X\). - The oxidation state of oxygen is -2. - The formula for the compound is \(2X + 3(-2) = 0\) (since the overall charge of a neutral compound is zero). - This simplifies to \(2X - 6 = 0\). - Solving for \(X\), we get \(2X = 6\) which gives \(X = +3\). ### Step 3: Analyze the change in oxidation states. - The oxidation state of iron changes from 0 (in elemental form) to +3 (in \(Fe_2O_3\)). - This increase in oxidation state indicates that iron is being oxidized. ### Step 4: Determine the change in oxidation state of oxygen. - The oxidation state of oxygen changes from 0 (in \(O_2\)) to -2 (in \(Fe_2O_3\)). - This decrease in oxidation state indicates that oxygen is being reduced. ### Step 5: Conclude the analysis with reference to iron. - Since we are analyzing the reaction with reference to iron, we can conclude that the oxidation of iron occurs as it goes from \(Fe\) to \(Fe_2O_3\). - Therefore, the reaction can be summarized as the oxidation of iron from \(Fe\) to \(Fe_2O_3\). ### Final Answer: Thus, with reference to iron, the oxidation of iron occurs from \(Fe\) to \(Fe_2O_3\). ---
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