Answer :
Certainly! Let's walk through the redox reaction given:
[tex]\[ 2 \text{Al (s)} + 3 \text{ZnCl}_2 \text{(g)} \rightarrow 3 \text{Zn (s)} + 2 \text{AlCl}_3 \text{(aq)} \][/tex]
We'll analyze each statement to determine if it applies to this reaction:
1. Aluminum atoms transfer electrons to chlorine atoms.
In this reaction, aluminum starts as a solid metal \(\text{Al}\) in its elemental form, with an oxidation state of 0. Aluminum forms \(\text{AlCl}_3\) in the product, where aluminum has an oxidation state of +3. Hence, aluminum loses electrons (is oxidized) and these electrons are transferred to chlorine atoms.
Therefore, this statement is true.
2. Zinc is reduced.
Zinc starts as \(\text{ZnCl}_2\), where zinc has an oxidation state of +2. In the product, it forms elemental zinc \(\text{Zn}\), which has an oxidation state of 0. Hence, zinc gains electrons (is reduced).
Therefore, this statement is true.
3. Zinc is the reducing agent.
The reducing agent is the substance that donates electrons and gets oxidized in the process. In this reaction, aluminum is the one donating electrons and being oxidized, not zinc.
Therefore, this statement is false.
4. The oxidation number of chlorine does not change.
Chlorine in \(\text{ZnCl}_2\) has an oxidation state of -1 and remains in the oxidation state of -1 in \(\text{AlCl}_3\). Thus, the oxidation number of chlorine remains the same throughout the reaction.
Therefore, this statement is true.
5. Aluminum is oxidized.
As established earlier, aluminum starts in the oxidation state of 0 and ends in an oxidation state of +3 in \(\text{AlCl}_3\), indicating it has lost electrons and thus been oxidized.
Therefore, this statement is true.
### Summary:
The statements that apply to the given redox reaction are:
- Aluminum atoms transfer electrons to chlorine atoms. (True)
- Zinc is reduced. (True)
- Zinc is the reducing agent. (False)
- The oxidation number of chlorine does not change. (True)
- Aluminum is oxidized. (True)
Thus, the full and correct answer is:
[tex]\[ (\text{True}, \text{True}, \text{False}, \text{True}, \text{True}) \][/tex]
[tex]\[ 2 \text{Al (s)} + 3 \text{ZnCl}_2 \text{(g)} \rightarrow 3 \text{Zn (s)} + 2 \text{AlCl}_3 \text{(aq)} \][/tex]
We'll analyze each statement to determine if it applies to this reaction:
1. Aluminum atoms transfer electrons to chlorine atoms.
In this reaction, aluminum starts as a solid metal \(\text{Al}\) in its elemental form, with an oxidation state of 0. Aluminum forms \(\text{AlCl}_3\) in the product, where aluminum has an oxidation state of +3. Hence, aluminum loses electrons (is oxidized) and these electrons are transferred to chlorine atoms.
Therefore, this statement is true.
2. Zinc is reduced.
Zinc starts as \(\text{ZnCl}_2\), where zinc has an oxidation state of +2. In the product, it forms elemental zinc \(\text{Zn}\), which has an oxidation state of 0. Hence, zinc gains electrons (is reduced).
Therefore, this statement is true.
3. Zinc is the reducing agent.
The reducing agent is the substance that donates electrons and gets oxidized in the process. In this reaction, aluminum is the one donating electrons and being oxidized, not zinc.
Therefore, this statement is false.
4. The oxidation number of chlorine does not change.
Chlorine in \(\text{ZnCl}_2\) has an oxidation state of -1 and remains in the oxidation state of -1 in \(\text{AlCl}_3\). Thus, the oxidation number of chlorine remains the same throughout the reaction.
Therefore, this statement is true.
5. Aluminum is oxidized.
As established earlier, aluminum starts in the oxidation state of 0 and ends in an oxidation state of +3 in \(\text{AlCl}_3\), indicating it has lost electrons and thus been oxidized.
Therefore, this statement is true.
### Summary:
The statements that apply to the given redox reaction are:
- Aluminum atoms transfer electrons to chlorine atoms. (True)
- Zinc is reduced. (True)
- Zinc is the reducing agent. (False)
- The oxidation number of chlorine does not change. (True)
- Aluminum is oxidized. (True)
Thus, the full and correct answer is:
[tex]\[ (\text{True}, \text{True}, \text{False}, \text{True}, \text{True}) \][/tex]
