At Westonci.ca, we connect you with the answers you need, thanks to our active and informed community. Connect with a community of experts ready to help you find solutions to your questions quickly and accurately. Connect with a community of professionals ready to help you find accurate solutions to your questions quickly and efficiently.
Sagot :
To identify the reduction half-reaction for the given chemical reaction, we need to understand the concepts of oxidation and reduction. In a redox reaction, oxidation involves the loss of electrons, while reduction involves the gain of electrons. A reduction half-reaction shows the species that is gaining electrons.
The given full reaction is:
[tex]\[ \text{Mg (s)} + \text{ZnCl}_2 (\text{aq}) \rightarrow \text{MgCl}_2 (\text{aq}) + \text{Zn (s)} \][/tex]
We need to determine the species that undergoes reduction.
1. Oxidation States Assignment:
- Magnesium (Mg) in its elemental form (s) has an oxidation state of 0.
- Zinc (Zn) in \(\text{ZnCl}_2\) is in the +2 oxidation state.
- Chlorine (Cl) in \(\text{ZnCl}_2\) and \(\text{MgCl}_2\) is in the -1 oxidation state.
- Magnesium (Mg) in \(\text{MgCl}_2\) is in the +2 oxidation state.
- Zinc (Zn) in its elemental form (s) has an oxidation state of 0.
2. Determine the Species Being Reduced:
- Magnesium (Mg) starts in the 0 oxidation state and ends up in the +2 oxidation state. Hence, magnesium is oxidized (it loses electrons).
- Zinc (Zn) starts in the +2 oxidation state in \(\text{ZnCl}_2\) and ends up in the 0 oxidation state. Hence, zinc is reduced (it gains electrons).
3. Write the Reduction Half-Reaction:
Since zinc is gaining electrons, the reduction half-reaction involves the conversion of zinc ions (\( \text{Zn}^{2+} \)) to elemental zinc (Zn).
Therefore, the reduction half-reaction is:
[tex]\[ \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn (s)} \][/tex]
From the given options:
- A. \( \text{Zn (s)} \rightarrow \text{Zn}^{2+} + 2e^- \) (This is an oxidation reaction)
- B. \( \text{Mg (s)} \rightarrow \text{Mg}^{2+} + 2e^- \) (This is an oxidation reaction)
- C. \( \text{Mg}^{2+} + 2e^- \rightarrow \text{Mg (s)} \) (This is a reduction reaction but not relevant to this problem)
- D. \( \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn (s)} \) (This is the correct reduction reaction)
Thus, the correct answer is:
[tex]\[ \boxed{4} \][/tex]
Which corresponds to option D: [tex]\( \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn (s)} \)[/tex].
The given full reaction is:
[tex]\[ \text{Mg (s)} + \text{ZnCl}_2 (\text{aq}) \rightarrow \text{MgCl}_2 (\text{aq}) + \text{Zn (s)} \][/tex]
We need to determine the species that undergoes reduction.
1. Oxidation States Assignment:
- Magnesium (Mg) in its elemental form (s) has an oxidation state of 0.
- Zinc (Zn) in \(\text{ZnCl}_2\) is in the +2 oxidation state.
- Chlorine (Cl) in \(\text{ZnCl}_2\) and \(\text{MgCl}_2\) is in the -1 oxidation state.
- Magnesium (Mg) in \(\text{MgCl}_2\) is in the +2 oxidation state.
- Zinc (Zn) in its elemental form (s) has an oxidation state of 0.
2. Determine the Species Being Reduced:
- Magnesium (Mg) starts in the 0 oxidation state and ends up in the +2 oxidation state. Hence, magnesium is oxidized (it loses electrons).
- Zinc (Zn) starts in the +2 oxidation state in \(\text{ZnCl}_2\) and ends up in the 0 oxidation state. Hence, zinc is reduced (it gains electrons).
3. Write the Reduction Half-Reaction:
Since zinc is gaining electrons, the reduction half-reaction involves the conversion of zinc ions (\( \text{Zn}^{2+} \)) to elemental zinc (Zn).
Therefore, the reduction half-reaction is:
[tex]\[ \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn (s)} \][/tex]
From the given options:
- A. \( \text{Zn (s)} \rightarrow \text{Zn}^{2+} + 2e^- \) (This is an oxidation reaction)
- B. \( \text{Mg (s)} \rightarrow \text{Mg}^{2+} + 2e^- \) (This is an oxidation reaction)
- C. \( \text{Mg}^{2+} + 2e^- \rightarrow \text{Mg (s)} \) (This is a reduction reaction but not relevant to this problem)
- D. \( \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn (s)} \) (This is the correct reduction reaction)
Thus, the correct answer is:
[tex]\[ \boxed{4} \][/tex]
Which corresponds to option D: [tex]\( \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn (s)} \)[/tex].
We hope our answers were helpful. Return anytime for more information and answers to any other questions you may have. We hope our answers were useful. Return anytime for more information and answers to any other questions you have. Thank you for visiting Westonci.ca, your go-to source for reliable answers. Come back soon for more expert insights.