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In the reaction 3MnO(2) + 4A1 to 3Mn + 2...

In the reaction `3MnO_(2) + 4A1 to 3Mn + 2A1_(2) O_(3)` the oxidizing agent is

A

`MnO_(2)`

B

A1

C

`A1_(2)_(3)`

D

Mn

Text Solution

AI Generated Solution

The correct Answer is:
To determine the oxidizing agent in the reaction \(3MnO_2 + 4Al \rightarrow 3Mn + 2Al_2O_3\), we can follow these steps: ### Step 1: Identify the oxidation states of the elements involved. - In \(MnO_2\), manganese (Mn) has an oxidation state of +4. - In elemental manganese (Mn), the oxidation state is 0. - In elemental aluminum (Al), the oxidation state is 0. - In \(Al_2O_3\), aluminum (Al) has an oxidation state of +3. ### Step 2: Determine the changes in oxidation states. - Manganese changes from +4 in \(MnO_2\) to 0 in \(Mn\). This indicates that manganese is being reduced (gaining electrons). - Aluminum changes from 0 in \(Al\) to +3 in \(Al_2O_3\). This indicates that aluminum is being oxidized (losing electrons). ### Step 3: Identify the oxidizing and reducing agents. - The substance that gets reduced is the oxidizing agent. Since manganese in \(MnO_2\) is reduced from +4 to 0, \(MnO_2\) is the oxidizing agent. - The substance that gets oxidized is the reducing agent. In this case, aluminum is oxidized from 0 to +3. ### Conclusion: The oxidizing agent in the reaction is \(MnO_2\). ---
To determine the oxidizing agent in the reaction \(3MnO_2 + 4Al \rightarrow 3Mn + 2Al_2O_3\), we can follow these steps: ### Step 1: Identify the oxidation states of the elements involved. - In \(MnO_2\), manganese (Mn) has an oxidation state of +4. - In elemental manganese (Mn), the oxidation state is 0. - In elemental aluminum (Al), the oxidation state is 0. - In \(Al_2O_3\), aluminum (Al) has an oxidation state of +3. ...
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