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Sagot :
Alright, let's analyze the chemical reaction step-by-step to identify the atoms that are oxidized and reduced, as well as the oxidizing and reducing agents.
The given chemical equation is:
[tex]\[ C_2H_4(g) + 3O_2(g) \rightarrow 2CO_2(g) + 2H_2O(g) \][/tex]
1. Oxidation States of Reactants and Products:
- Carbon in [tex]\(C_2H_4\)[/tex]: Each hydrogen has an oxidation state of +1. To balance the overall charge of the molecule (which is neutral), the oxidation state of each carbon must be -2.
[tex]\[ \text{Oxidation state of C in } C_2H_4 = -2 \][/tex]
- Oxygen in [tex]\( O_2 \)[/tex]: Since [tex]\( O_2 \)[/tex] is in its elemental form, the oxidation state is 0.
[tex]\[ \text{Oxidation state of O in } O_2 = 0 \][/tex]
- Carbon in [tex]\( CO_2 \)[/tex]: Each oxygen has an oxidation state of -2. To balance the molecule, the oxidation state of carbon must be +4.
[tex]\[ \text{Oxidation state of C in } CO_2 = +4 \][/tex]
- Oxygen in [tex]\( CO_2 \)[/tex]: Oxygen retains its usual oxidation state of -2.
[tex]\[ \text{Oxidation state of O in } CO_2 = -2 \][/tex]
- Hydrogen in [tex]\( H_2O \)[/tex]: Each hydrogen has an oxidation state of +1.
[tex]\[ \text{Oxidation state of H in } H_2O = +1 \][/tex]
- Oxygen in [tex]\( H_2O \)[/tex]: Oxygen retains its usual oxidation state of -2.
[tex]\[ \text{Oxidation state of O in } H_2O = -2 \][/tex]
2. Identifying Oxidation and Reduction:
- Oxidation (loss of electrons): Carbon is oxidized.
[tex]\[ \text{Change for Carbon: } -2 \rightarrow +4 \][/tex]
- Reduction (gain of electrons): Oxygen is reduced.
[tex]\[ \text{Change for Oxygen: } 0 \rightarrow -2 \][/tex]
3. Oxidizing and Reducing Agents:
- Oxidizing Agent: The substance that gets reduced is the oxidizing agent. In this case, [tex]\( O_2 \)[/tex] is the oxidizing agent.
- Reducing Agent: The substance that gets oxidized is the reducing agent. In this case, [tex]\( C_2H_4 \)[/tex] is the reducing agent.
To summarize the oxidation states and changes:
| Element | Role | Symbol | Oxidation State (Reactant) | Oxidation State (Product) |
|---------|------|--------|----------------------------|---------------------------|
| Carbon | Oxidized | C | -2 | +4 |
| Hydrogen| No Change | H | +1 | +1 |
| Oxygen | Reduced | O | 0 | -2 |
### Conclusion:
- Carbon (C) in [tex]\( C_2H_4 \)[/tex] is oxidized, changing from an oxidation state of -2 to +4.
- Oxygen (O) in [tex]\( O_2 \)[/tex] is reduced, changing from an oxidation state of 0 to -2.
- The oxidizing agent is [tex]\( O_2 \)[/tex].
- The reducing agent is [tex]\( C_2H_4 \)[/tex].
We have successfully identified all the required elements and changes in the chemical reaction.
The given chemical equation is:
[tex]\[ C_2H_4(g) + 3O_2(g) \rightarrow 2CO_2(g) + 2H_2O(g) \][/tex]
1. Oxidation States of Reactants and Products:
- Carbon in [tex]\(C_2H_4\)[/tex]: Each hydrogen has an oxidation state of +1. To balance the overall charge of the molecule (which is neutral), the oxidation state of each carbon must be -2.
[tex]\[ \text{Oxidation state of C in } C_2H_4 = -2 \][/tex]
- Oxygen in [tex]\( O_2 \)[/tex]: Since [tex]\( O_2 \)[/tex] is in its elemental form, the oxidation state is 0.
[tex]\[ \text{Oxidation state of O in } O_2 = 0 \][/tex]
- Carbon in [tex]\( CO_2 \)[/tex]: Each oxygen has an oxidation state of -2. To balance the molecule, the oxidation state of carbon must be +4.
[tex]\[ \text{Oxidation state of C in } CO_2 = +4 \][/tex]
- Oxygen in [tex]\( CO_2 \)[/tex]: Oxygen retains its usual oxidation state of -2.
[tex]\[ \text{Oxidation state of O in } CO_2 = -2 \][/tex]
- Hydrogen in [tex]\( H_2O \)[/tex]: Each hydrogen has an oxidation state of +1.
[tex]\[ \text{Oxidation state of H in } H_2O = +1 \][/tex]
- Oxygen in [tex]\( H_2O \)[/tex]: Oxygen retains its usual oxidation state of -2.
[tex]\[ \text{Oxidation state of O in } H_2O = -2 \][/tex]
2. Identifying Oxidation and Reduction:
- Oxidation (loss of electrons): Carbon is oxidized.
[tex]\[ \text{Change for Carbon: } -2 \rightarrow +4 \][/tex]
- Reduction (gain of electrons): Oxygen is reduced.
[tex]\[ \text{Change for Oxygen: } 0 \rightarrow -2 \][/tex]
3. Oxidizing and Reducing Agents:
- Oxidizing Agent: The substance that gets reduced is the oxidizing agent. In this case, [tex]\( O_2 \)[/tex] is the oxidizing agent.
- Reducing Agent: The substance that gets oxidized is the reducing agent. In this case, [tex]\( C_2H_4 \)[/tex] is the reducing agent.
To summarize the oxidation states and changes:
| Element | Role | Symbol | Oxidation State (Reactant) | Oxidation State (Product) |
|---------|------|--------|----------------------------|---------------------------|
| Carbon | Oxidized | C | -2 | +4 |
| Hydrogen| No Change | H | +1 | +1 |
| Oxygen | Reduced | O | 0 | -2 |
### Conclusion:
- Carbon (C) in [tex]\( C_2H_4 \)[/tex] is oxidized, changing from an oxidation state of -2 to +4.
- Oxygen (O) in [tex]\( O_2 \)[/tex] is reduced, changing from an oxidation state of 0 to -2.
- The oxidizing agent is [tex]\( O_2 \)[/tex].
- The reducing agent is [tex]\( C_2H_4 \)[/tex].
We have successfully identified all the required elements and changes in the chemical reaction.
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