What would you use to prove that copper is reduced in the following reaction? Fe) + CuSO4(q) → FeSO4(q) + Cu() -Fe CuSO4 - FeSO4 Single replacement reaction A B C D a decrease in its oxidation number an increase in its oxidation number a gain of oxygen a loss of electrons Cu
What would you use to prove that copper is reduced in the following reaction? Fe) + CuSO4(q) → FeSO4(q) + Cu() -Fe CuSO4 - FeSO4 Single replacement reaction A B C D a decrease in its oxidation number an increase in its oxidation number a gain of oxygen a loss of electrons Cu
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Title: Identifying Reduction of Copper in a Chemical Reaction**
**Introduction:**
Chemical reactions often involve the exchange of elements between reactants, leading to the formation of new substances. One such reaction is a single replacement reaction, where an element in a compound is replaced by another element.
**Reaction Representation:**
\[ Fe_{(s)} + CuSO_4_{(aq)} \rightarrow FeSO_4_{(aq)} + Cu_{(s)} \]
**Description:**
This is a single replacement reaction where a solid iron (Fe) rod is placed in a solution of copper sulfate (CuSO₄). During the reaction, copper (Cu) will be deposited on the iron rod, and the solution will change from blue to green as FeSO₄ forms.
**Visual Examination:**
- **Left Test Tube:**
- Contains a blue solution of copper sulfate (CuSO₄).
- An iron rod (Fe) is submerged in the solution.
- **Right Test Tube:**
- The solution color has changed to green, indicating the formation of iron(II) sulfate (FeSO₄).
- Copper (Cu) is now deposited on the iron rod.
**Question:**
What would you use to prove that copper is reduced in the following reaction?
**Answer Choices:**
A. A decrease in its oxidation number
B. An increase in its oxidation number
C. A gain of oxygen
D. A loss of electrons
**Explanation:**
To determine whether copper is reduced, we need to analyze the changes in the oxidation states of copper. In its ionic form in copper sulfate (Cu²⁺), copper has an oxidation number of +2. When copper is deposited as a solid (Cu), it has an oxidation number of 0. A reduction in terms of redox reactions involves a decrease in the oxidation number.
**Conclusion:**
The correct answer to the question is:
**A decrease in its oxidation number** (Option A).
This visual illustrates how single replacement reactions involve the transfer of electrons, leading to observable changes in the physical state and coloration of the involved substances.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd2e081c9-4ec3-4168-ae7b-be51eea23efd%2F831edb07-ea69-4adc-a2a0-b6f908253586%2Fczhot9_processed.png&w=3840&q=75)
Transcribed Image Text:**Title: Identifying Reduction of Copper in a Chemical Reaction**
**Introduction:**
Chemical reactions often involve the exchange of elements between reactants, leading to the formation of new substances. One such reaction is a single replacement reaction, where an element in a compound is replaced by another element.
**Reaction Representation:**
\[ Fe_{(s)} + CuSO_4_{(aq)} \rightarrow FeSO_4_{(aq)} + Cu_{(s)} \]
**Description:**
This is a single replacement reaction where a solid iron (Fe) rod is placed in a solution of copper sulfate (CuSO₄). During the reaction, copper (Cu) will be deposited on the iron rod, and the solution will change from blue to green as FeSO₄ forms.
**Visual Examination:**
- **Left Test Tube:**
- Contains a blue solution of copper sulfate (CuSO₄).
- An iron rod (Fe) is submerged in the solution.
- **Right Test Tube:**
- The solution color has changed to green, indicating the formation of iron(II) sulfate (FeSO₄).
- Copper (Cu) is now deposited on the iron rod.
**Question:**
What would you use to prove that copper is reduced in the following reaction?
**Answer Choices:**
A. A decrease in its oxidation number
B. An increase in its oxidation number
C. A gain of oxygen
D. A loss of electrons
**Explanation:**
To determine whether copper is reduced, we need to analyze the changes in the oxidation states of copper. In its ionic form in copper sulfate (Cu²⁺), copper has an oxidation number of +2. When copper is deposited as a solid (Cu), it has an oxidation number of 0. A reduction in terms of redox reactions involves a decrease in the oxidation number.
**Conclusion:**
The correct answer to the question is:
**A decrease in its oxidation number** (Option A).
This visual illustrates how single replacement reactions involve the transfer of electrons, leading to observable changes in the physical state and coloration of the involved substances.
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