Assign oxidation numbers to each individual element in the following reaction and identify the oxidizing and reducing agents.
2 Zn S + 3 O2 -> 2 S O2 + 2 Zn O
Ox#: Zn=+2 S=-2 O=-2 -> S=+2 O=-2 Zn=+2 O=2
Is that correct?
I'm not sure how to identify the oxidizing and reducing agents.
Your oxidation numbers for each element in the reaction are correct. To identify the oxidizing and reducing agents, you need to look at the change in oxidation numbers of each element in the reaction.
In this reaction:
2 ZnS + 3 O2 -> 2 SO2 + 2 ZnO
Zinc (Zn) goes from an oxidation state of 0 to +2 in ZnO, which means it lost electrons and was oxidized. Therefore, Zinc (Zn) is the reducing agent.
Oxygen (O) goes from an oxidation state of 0 to -2 in SO2, which means it gained electrons and was reduced. Therefore, Oxygen (O) is the oxidizing agent.
Your oxidation number assignments are correct. Now, let's determine the oxidizing and reducing agents in this reaction.
To identify the oxidizing and reducing agents, you need to compare the changes in oxidation numbers of the elements involved in the reaction.
In this reaction:
2 ZnS + 3 O2 -> 2 SO2 + 2 ZnO
Zinc (Zn) is oxidized from an oxidation state of 0 in ZnS to +2 in ZnO. The oxidation number of zinc increased from 0 to +2, indicating that zinc lost electrons and was oxidized.
Oxygen (O) is reduced from an oxidation state of 0 in O2 to -2 in SO2. The oxidation number of oxygen decreased from 0 to -2, indicating that oxygen gained electrons and was reduced.
Therefore, zinc (Zn) is the reducing agent because it lost electrons and was oxidized. Oxygen (O) is the oxidizing agent because it gained electrons and was reduced.
To summarize:
- Reducing Agent: Zn
- Oxidizing Agent: O2