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Sagot :
Let’s break down the reaction and analyze the oxidation states of the elements involved.
The balanced reaction given is:
[tex]\[ 2 \text{NO} (g) + 2 \text{CO} (g) \rightarrow \text{N}_2 (g) + 2 \text{CO}_2 (g) \][/tex]
1. Determining the Oxidation States:
- The oxidation state of nitrogen (N) in nitric oxide ([tex]\(\text{NO}\)[/tex]) is +2.
- The oxidation state of carbon (C) in carbon monoxide ([tex]\(\text{CO}\)[/tex]) is +2.
- In the product nitrogen gas ([tex]\(\text{N}_2\)[/tex]), the oxidation state of nitrogen is 0.
- In the product carbon dioxide ([tex]\(\text{CO}_2\)[/tex]), the oxidation state of carbon is +4.
2. Changes in Oxidation States:
- For nitrogen in [tex]\(\text{NO}\)[/tex] to [tex]\(\text{N}_2\)[/tex]:
[tex]\[ \text{NO} \rightarrow \text{N}_2 \][/tex]
The oxidation state of nitrogen changes from +2 (in [tex]\(\text{NO}\)[/tex]) to 0 (in [tex]\(\text{N}_2\)[/tex]). This is a reduction process (gain of electrons).
- For carbon in [tex]\(\text{CO}\)[/tex] to [tex]\(\text{CO}_2\)[/tex]:
[tex]\[ \text{CO} \rightarrow \text{CO}_2 \][/tex]
The oxidation state of carbon changes from +2 (in [tex]\(\text{CO}\)[/tex]) to +4 (in [tex]\(\text{CO}_2\)[/tex]). This is an oxidation process (loss of electrons).
3. Describing Reducing and Oxidizing Processes:
- The compound [tex]\(\text{NO}\)[/tex] is reduced (the oxidation state of nitrogen decreases from +2 to 0), which means it is acting as an oxidizing agent.
- The compound [tex]\(\text{CO}\)[/tex] is oxidized (the oxidation state of carbon increases from +2 to +4), which means it is acting as a reducing agent.
So, the detailed changes in oxidation states during this reaction are:
- The oxidation state of nitrogen in [tex]\(\text{NO}\)[/tex] changes from +2 to 0.
- The oxidation state of carbon in [tex]\(\text{CO}\)[/tex] changes from +2 to +4.
Conclusion:
The correct answer that best describes the reducing and oxidizing processes in this reaction is:
- The oxidation state of nitrogen in NO changes from +2 to 0, and the oxidation state of carbon in CO changes from +2 to +4 as the reaction proceeds.
The balanced reaction given is:
[tex]\[ 2 \text{NO} (g) + 2 \text{CO} (g) \rightarrow \text{N}_2 (g) + 2 \text{CO}_2 (g) \][/tex]
1. Determining the Oxidation States:
- The oxidation state of nitrogen (N) in nitric oxide ([tex]\(\text{NO}\)[/tex]) is +2.
- The oxidation state of carbon (C) in carbon monoxide ([tex]\(\text{CO}\)[/tex]) is +2.
- In the product nitrogen gas ([tex]\(\text{N}_2\)[/tex]), the oxidation state of nitrogen is 0.
- In the product carbon dioxide ([tex]\(\text{CO}_2\)[/tex]), the oxidation state of carbon is +4.
2. Changes in Oxidation States:
- For nitrogen in [tex]\(\text{NO}\)[/tex] to [tex]\(\text{N}_2\)[/tex]:
[tex]\[ \text{NO} \rightarrow \text{N}_2 \][/tex]
The oxidation state of nitrogen changes from +2 (in [tex]\(\text{NO}\)[/tex]) to 0 (in [tex]\(\text{N}_2\)[/tex]). This is a reduction process (gain of electrons).
- For carbon in [tex]\(\text{CO}\)[/tex] to [tex]\(\text{CO}_2\)[/tex]:
[tex]\[ \text{CO} \rightarrow \text{CO}_2 \][/tex]
The oxidation state of carbon changes from +2 (in [tex]\(\text{CO}\)[/tex]) to +4 (in [tex]\(\text{CO}_2\)[/tex]). This is an oxidation process (loss of electrons).
3. Describing Reducing and Oxidizing Processes:
- The compound [tex]\(\text{NO}\)[/tex] is reduced (the oxidation state of nitrogen decreases from +2 to 0), which means it is acting as an oxidizing agent.
- The compound [tex]\(\text{CO}\)[/tex] is oxidized (the oxidation state of carbon increases from +2 to +4), which means it is acting as a reducing agent.
So, the detailed changes in oxidation states during this reaction are:
- The oxidation state of nitrogen in [tex]\(\text{NO}\)[/tex] changes from +2 to 0.
- The oxidation state of carbon in [tex]\(\text{CO}\)[/tex] changes from +2 to +4.
Conclusion:
The correct answer that best describes the reducing and oxidizing processes in this reaction is:
- The oxidation state of nitrogen in NO changes from +2 to 0, and the oxidation state of carbon in CO changes from +2 to +4 as the reaction proceeds.
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