For the following reaction, identify the substances oxidized, reduced and the oxidizing and reducing agents?
2SO2 + O2 --> 2SO3
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To identify the substances oxidized, reduced, and the oxidizing and reducing agents in a reaction, we need to determine the changes in oxidation numbers.
Let's start by assigning oxidation numbers to each element in the reactants and products:
For the reactants:
- The oxidation number of sulfur (S) in SO2 is +4.
- The oxidation number of oxygen (O) in O2 is 0.
- The oxidation number of sulfur (S) in SO3 is +6.
- The oxidation number of oxygen (O) in SO3 is -2.
Based on the changes in oxidation numbers, we can determine the following:
The substance being oxidized: In this reaction, sulfur (S) is being oxidized from an oxidation state of +4 in SO2 to +6 in SO3. Therefore, sulfur is being oxidized.
The substance being reduced: In this reaction, oxygen (O) is being reduced from an oxidation state of 0 in O2 to -2 in SO3. Therefore, oxygen is being reduced.
The oxidizing agent: The oxidizing agent is the substance that causes another substance to be oxidized. In this reaction, O2 is the oxidizing agent because it facilitates the oxidation of sulfur.
The reducing agent: The reducing agent is the substance that causes another substance to be reduced. In this reaction, SO2 is the reducing agent because it facilitates the reduction of oxygen.
To summarize:
- Substance oxidized: Sulfur (S)
- Substance reduced: Oxygen (O)
- Oxidizing agent: O2
- Reducing agent: SO2