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Sagot :
To determine the oxidizing agent and the reducing agent in the given chemical equation, we need to look at the changes in oxidation states of the elements involved. The chemical reaction given is:
[tex]\[ 3 \text{FeS} + 8 \text{HNO}_3 \rightarrow 3 \text{FeSO}_4 + 8 \text{NO} + 4 \text{H}_2\text{O} \][/tex]
Follow these steps to identify the oxidizing and reducing agents:
1. Assign oxidation states to all elements in the reactants and products:
- For [tex]\(\text{FeS}\)[/tex]:
- [tex]\( \text{Fe}\)[/tex] (in [tex]\(\text{FeS}\)[/tex]): Normally, Fe in [tex]\(\text{FeS}\)[/tex] can be considered to have an oxidation state of +2.
- [tex]\( \text{S} \)[/tex] (in [tex]\(\text{FeS}\)[/tex]): Given that Fe is +2, and the compound is neutral, S must have an oxidation state of -2.
- For [tex]\(\text{HNO}_3\)[/tex]:
- [tex]\( \text{H}\)[/tex]: +1.
- [tex]\( \text{N}\)[/tex]: +5, since nitrogen typically has this oxidation state in nitric acid.
- [tex]\( \text{O}\)[/tex]: -2 for each oxygen atom.
- For [tex]\(\text{FeSO}_4\)[/tex]:
- [tex]\( \text{Fe}\)[/tex] (in [tex]\(\text{FeSO}_4\)[/tex]): +2 (same as in [tex]\(\text{FeS}\)[/tex]).
- [tex]\( \text{S}\)[/tex] (in [tex]\(\text{SO}_4^{2-}\)[/tex]): +6 (since the sulfate ion has a -2 charge and each oxygen is -2).
- [tex]\( \text{O}\)[/tex]: -2.
- For [tex]\(\text{NO}\)[/tex]:
- [tex]\( \text{N}\)[/tex]: +2.
- [tex]\( \text{O}\)[/tex]: -2.
- For [tex]\( \text{H}_2\text{O}\)[/tex]:
- [tex]\( \text{H}\)[/tex]: +1.
- [tex]\( \text{O}\)[/tex]: -2.
2. Identify changes in oxidation states:
- [tex]\( \text{S} \)[/tex] in [tex]\(\text{FeS}\)[/tex] changes from -2 (in [tex]\(\text{FeS}\)[/tex]) to +6 (in [tex]\(\text{FeSO}_4\)[/tex]).
- This indicates that sulfur in [tex]\(\text{FeS}\)[/tex] is oxidized.
- [tex]\( \text{N} \)[/tex] in [tex]\(\text{HNO}_3\)[/tex] changes from +5 (in [tex]\(\text{HNO}_3\)[/tex]) to +2 (in [tex]\(\text{NO}\)[/tex]).
- This indicates that nitrogen in [tex]\(\text{HNO}_3\)[/tex] is reduced.
3. Definition of oxidizing and reducing agents:
- The substance that is oxidized (loses electrons) is the reducing agent.
- The substance that is reduced (gains electrons) is the oxidizing agent.
From the changes we have identified:
- [tex]\(\text{FeS} \)[/tex] is oxidized (S changes from -2 to +6 ), so [tex]\(\text{FeS} \)[/tex] is the reducing agent.
- [tex]\(\text{HNO}_3 \)[/tex] is reduced (N changes from +5 to +2 ), so [tex]\(\text{HNO}_3 \)[/tex] is the oxidizing agent.
Thus, the correct answer is:
C. [tex]\(\text{FeS}\)[/tex] is the reducing agent, and [tex]\(\text{HNO}_3\)[/tex] is the oxidizing agent.
[tex]\[ 3 \text{FeS} + 8 \text{HNO}_3 \rightarrow 3 \text{FeSO}_4 + 8 \text{NO} + 4 \text{H}_2\text{O} \][/tex]
Follow these steps to identify the oxidizing and reducing agents:
1. Assign oxidation states to all elements in the reactants and products:
- For [tex]\(\text{FeS}\)[/tex]:
- [tex]\( \text{Fe}\)[/tex] (in [tex]\(\text{FeS}\)[/tex]): Normally, Fe in [tex]\(\text{FeS}\)[/tex] can be considered to have an oxidation state of +2.
- [tex]\( \text{S} \)[/tex] (in [tex]\(\text{FeS}\)[/tex]): Given that Fe is +2, and the compound is neutral, S must have an oxidation state of -2.
- For [tex]\(\text{HNO}_3\)[/tex]:
- [tex]\( \text{H}\)[/tex]: +1.
- [tex]\( \text{N}\)[/tex]: +5, since nitrogen typically has this oxidation state in nitric acid.
- [tex]\( \text{O}\)[/tex]: -2 for each oxygen atom.
- For [tex]\(\text{FeSO}_4\)[/tex]:
- [tex]\( \text{Fe}\)[/tex] (in [tex]\(\text{FeSO}_4\)[/tex]): +2 (same as in [tex]\(\text{FeS}\)[/tex]).
- [tex]\( \text{S}\)[/tex] (in [tex]\(\text{SO}_4^{2-}\)[/tex]): +6 (since the sulfate ion has a -2 charge and each oxygen is -2).
- [tex]\( \text{O}\)[/tex]: -2.
- For [tex]\(\text{NO}\)[/tex]:
- [tex]\( \text{N}\)[/tex]: +2.
- [tex]\( \text{O}\)[/tex]: -2.
- For [tex]\( \text{H}_2\text{O}\)[/tex]:
- [tex]\( \text{H}\)[/tex]: +1.
- [tex]\( \text{O}\)[/tex]: -2.
2. Identify changes in oxidation states:
- [tex]\( \text{S} \)[/tex] in [tex]\(\text{FeS}\)[/tex] changes from -2 (in [tex]\(\text{FeS}\)[/tex]) to +6 (in [tex]\(\text{FeSO}_4\)[/tex]).
- This indicates that sulfur in [tex]\(\text{FeS}\)[/tex] is oxidized.
- [tex]\( \text{N} \)[/tex] in [tex]\(\text{HNO}_3\)[/tex] changes from +5 (in [tex]\(\text{HNO}_3\)[/tex]) to +2 (in [tex]\(\text{NO}\)[/tex]).
- This indicates that nitrogen in [tex]\(\text{HNO}_3\)[/tex] is reduced.
3. Definition of oxidizing and reducing agents:
- The substance that is oxidized (loses electrons) is the reducing agent.
- The substance that is reduced (gains electrons) is the oxidizing agent.
From the changes we have identified:
- [tex]\(\text{FeS} \)[/tex] is oxidized (S changes from -2 to +6 ), so [tex]\(\text{FeS} \)[/tex] is the reducing agent.
- [tex]\(\text{HNO}_3 \)[/tex] is reduced (N changes from +5 to +2 ), so [tex]\(\text{HNO}_3 \)[/tex] is the oxidizing agent.
Thus, the correct answer is:
C. [tex]\(\text{FeS}\)[/tex] is the reducing agent, and [tex]\(\text{HNO}_3\)[/tex] is the oxidizing agent.
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