What is being oxidized and reduced in this reaction? + CuSO FeSO 4(aq) + Cu(s) Fe (s) → 4(aq) A Fe is oxidized and Cu is reduced. B Cu is oxidized and Fe is reduced. C The oxidation states of both Fe and Cu do not change. D Oxygen is oxidized and sulfur is reduced.
What is being oxidized and reduced in this reaction? + CuSO FeSO 4(aq) + Cu(s) Fe (s) → 4(aq) A Fe is oxidized and Cu is reduced. B Cu is oxidized and Fe is reduced. C The oxidation states of both Fe and Cu do not change. D Oxygen is oxidized and sulfur is reduced.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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![### Multiple Choice Question 6
**What is being oxidized and reduced in this reaction?**
Reaction:
\[ \text{Fe}_{(s)} + \text{CuSO}_4{(aq)} \rightarrow \text{FeSO}_4{(aq)} + \text{Cu}_{(s)} \]
Options:
A. Fe is oxidized and Cu is reduced.
B. Cu is oxidized and Fe is reduced.
C. The oxidation states of both Fe and Cu do not change.
D. Oxygen is oxidized and sulfur is reduced.
### Explanation:
To determine what is being oxidized and what is being reduced in the reaction, identify the changes in the oxidation states of the elements involved:
1. **Oxidation**: Refers to the loss of electrons.
2. **Reduction**: Refers to the gain of electrons.
In the given reaction:
- Fe (iron) starts with an oxidation state of 0 (elemental form) and ends with an oxidation state of +2 (in FeSO₄).
- Cu (copper) starts with an oxidation state of +2 (in CuSO₄) and ends with an oxidation state of 0 (elemental form).
Thus, Fe loses electrons (is oxidized) and Cu gains electrons (is reduced).
**Correct Answer:**
A. Fe is oxidized and Cu is reduced.
### Additional Information:
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Transcribed Image Text:### Multiple Choice Question 6
**What is being oxidized and reduced in this reaction?**
Reaction:
\[ \text{Fe}_{(s)} + \text{CuSO}_4{(aq)} \rightarrow \text{FeSO}_4{(aq)} + \text{Cu}_{(s)} \]
Options:
A. Fe is oxidized and Cu is reduced.
B. Cu is oxidized and Fe is reduced.
C. The oxidation states of both Fe and Cu do not change.
D. Oxygen is oxidized and sulfur is reduced.
### Explanation:
To determine what is being oxidized and what is being reduced in the reaction, identify the changes in the oxidation states of the elements involved:
1. **Oxidation**: Refers to the loss of electrons.
2. **Reduction**: Refers to the gain of electrons.
In the given reaction:
- Fe (iron) starts with an oxidation state of 0 (elemental form) and ends with an oxidation state of +2 (in FeSO₄).
- Cu (copper) starts with an oxidation state of +2 (in CuSO₄) and ends with an oxidation state of 0 (elemental form).
Thus, Fe loses electrons (is oxidized) and Cu gains electrons (is reduced).
**Correct Answer:**
A. Fe is oxidized and Cu is reduced.
### Additional Information:
There is a navigation element at the bottom, showing that this is the 6th question out of a total of 14, with 4 questions answered so far. There are options to save changes and continue to the next question.
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