Asked by 31
Use the following reaction to answer the question:
2Al + 3Fe³⁺ → 2Al³⁺ + 3Fe
Which of the following is the correct oxidation half-reaction?
2Al + 3Fe³⁺ → 2Al³⁺ + 3Fe
Which of the following is the correct oxidation half-reaction?
Answers
Answered by
GPT-4o mini
In the given reaction:
\[ 2 \text{Al} + 3 \text{Fe}^{3+} \rightarrow 2 \text{Al}^{3+} + 3 \text{Fe} \]
To identify the oxidation half-reaction, we need to determine which species is oxidized. Oxidation is defined as the loss of electrons.
In this reaction:
- Aluminum (Al) starts in the elemental form (0 oxidation state) and ends up as Al³⁺ (oxidation state of +3).
- Iron (Fe) starts as Fe³⁺ and ends up as elemental Fe (0 oxidation state).
Since aluminum is being oxidized (losing electrons), we can express the oxidation half-reaction as follows:
\[ \text{Oxidation half-reaction:} \]
\[ \text{Al} \rightarrow \text{Al}^{3+} + 3 e^- \]
This shows that one aluminum atom loses three electrons to form Al³⁺. Since there are two aluminum atoms reacting, the full equation for the oxidation process would be:
\[ 2 \text{Al} \rightarrow 2 \text{Al}^{3+} + 6 e^- \]
Thus, the correct oxidation half-reaction for the overall reaction is:
\[ \text{2Al} \rightarrow \text{2Al}^{3+} + 6 e^- \]
\[ 2 \text{Al} + 3 \text{Fe}^{3+} \rightarrow 2 \text{Al}^{3+} + 3 \text{Fe} \]
To identify the oxidation half-reaction, we need to determine which species is oxidized. Oxidation is defined as the loss of electrons.
In this reaction:
- Aluminum (Al) starts in the elemental form (0 oxidation state) and ends up as Al³⁺ (oxidation state of +3).
- Iron (Fe) starts as Fe³⁺ and ends up as elemental Fe (0 oxidation state).
Since aluminum is being oxidized (losing electrons), we can express the oxidation half-reaction as follows:
\[ \text{Oxidation half-reaction:} \]
\[ \text{Al} \rightarrow \text{Al}^{3+} + 3 e^- \]
This shows that one aluminum atom loses three electrons to form Al³⁺. Since there are two aluminum atoms reacting, the full equation for the oxidation process would be:
\[ 2 \text{Al} \rightarrow 2 \text{Al}^{3+} + 6 e^- \]
Thus, the correct oxidation half-reaction for the overall reaction is:
\[ \text{2Al} \rightarrow \text{2Al}^{3+} + 6 e^- \]
Answered by
GPT-4o mini
I apologize if my response was unclear or misleading. Let's clarify the oxidation half-reaction for the reaction you provided.
The reaction given is:
\[ 2 \text{Al} + 3 \text{Fe}^{3+} \rightarrow 2 \text{Al}^{3+} + 3 \text{Fe} \]
In this reaction:
- Aluminum (Al) is being oxidized, as it goes from an oxidation state of 0 in elemental aluminum to +3 in Al³⁺.
- The appropriate oxidation half-reaction is where aluminum loses electrons during this process.
The correct oxidation half-reaction for the oxidation of aluminum can be written as:
\[ 2 \text{Al} \rightarrow 2 \text{Al}^{3+} + 6 e^- \]
Here's a clearer breakdown:
1. **Oxidation of aluminum:**
- Each aluminum atom loses 3 electrons:
- \( \text{Al} \rightarrow \text{Al}^{3+} + 3 e^- \)
- Since there are 2 aluminum atoms, you double this equation:
- \( 2 \text{Al} \rightarrow 2 \text{Al}^{3+} + 6 e^- \)
This correctly describes the oxidation process.
If there was a misunderstanding or if there are specific clarifications you are looking for, please let me know, and I’ll be happy to assist!
The reaction given is:
\[ 2 \text{Al} + 3 \text{Fe}^{3+} \rightarrow 2 \text{Al}^{3+} + 3 \text{Fe} \]
In this reaction:
- Aluminum (Al) is being oxidized, as it goes from an oxidation state of 0 in elemental aluminum to +3 in Al³⁺.
- The appropriate oxidation half-reaction is where aluminum loses electrons during this process.
The correct oxidation half-reaction for the oxidation of aluminum can be written as:
\[ 2 \text{Al} \rightarrow 2 \text{Al}^{3+} + 6 e^- \]
Here's a clearer breakdown:
1. **Oxidation of aluminum:**
- Each aluminum atom loses 3 electrons:
- \( \text{Al} \rightarrow \text{Al}^{3+} + 3 e^- \)
- Since there are 2 aluminum atoms, you double this equation:
- \( 2 \text{Al} \rightarrow 2 \text{Al}^{3+} + 6 e^- \)
This correctly describes the oxidation process.
If there was a misunderstanding or if there are specific clarifications you are looking for, please let me know, and I’ll be happy to assist!
Answered by
GPT-4o mini
I apologize for any confusion or frustration my previous responses may have caused. I aim to provide accurate information.
To clarify the oxidation half-reaction in the given reaction:
\[ 2 \text{Al} + 3 \text{Fe}^{3+} \rightarrow 2 \text{Al}^{3+} + 3 \text{Fe} \]
- **Oxidation** involves the loss of electrons. In this reaction, aluminum (Al) goes from an oxidation state of 0 to +3, indicating that it is being oxidized and is losing electrons.
Thus, the oxidation half-reaction can be correctly expressed as:
\[ \text{2Al} \rightarrow 2 \text{Al}^{3+} + 6 e^- \]
This indicates that two aluminum atoms lose a total of six electrons.
If you have specific details or evidence from your sources that contradict this explanation, I would appreciate hearing them so I can better understand your concerns. My goal is to assist you accurately!
To clarify the oxidation half-reaction in the given reaction:
\[ 2 \text{Al} + 3 \text{Fe}^{3+} \rightarrow 2 \text{Al}^{3+} + 3 \text{Fe} \]
- **Oxidation** involves the loss of electrons. In this reaction, aluminum (Al) goes from an oxidation state of 0 to +3, indicating that it is being oxidized and is losing electrons.
Thus, the oxidation half-reaction can be correctly expressed as:
\[ \text{2Al} \rightarrow 2 \text{Al}^{3+} + 6 e^- \]
This indicates that two aluminum atoms lose a total of six electrons.
If you have specific details or evidence from your sources that contradict this explanation, I would appreciate hearing them so I can better understand your concerns. My goal is to assist you accurately!
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