4. For each of i. ii. With reference to oxidation numbers, indicate whether choice. Use oxidation numbers to justify your answer. For all redox reactions, identify the oxidizing or reducing agent. Explain using oxidation numbers a. CuO + H₂ → Cu + H₂O If applicable: Oxidizing Agent b. 3 Cu +8 HNO3 → 3 Cu(NO3)2 + 2 NO + 4H₂O If applicable: Oxidizing Agent c. AgNO3 + NaCl → AgCl + NaNO3 If applicable: Oxidizing Agent redox Reducing Agent redox Reducing Agent redox Reducing Agent non redox non redox non redox
4. For each of i. ii. With reference to oxidation numbers, indicate whether choice. Use oxidation numbers to justify your answer. For all redox reactions, identify the oxidizing or reducing agent. Explain using oxidation numbers a. CuO + H₂ → Cu + H₂O If applicable: Oxidizing Agent b. 3 Cu +8 HNO3 → 3 Cu(NO3)2 + 2 NO + 4H₂O If applicable: Oxidizing Agent c. AgNO3 + NaCl → AgCl + NaNO3 If applicable: Oxidizing Agent redox Reducing Agent redox Reducing Agent redox Reducing Agent non redox non redox non redox
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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![**Worksheet: Understanding Redox Reactions**
**Instructions:** For each of the following reactions:
i. With reference to oxidation numbers, indicate whether they are redox reactions. Circle your choice. Use oxidation numbers to justify your answer.
ii. For all redox reactions, identify the oxidizing or reducing agent. Explain using oxidation numbers.
---
**a.** \( \text{CuO} + \text{H}_2 \rightarrow \text{Cu} + \text{H}_2\text{O} \)
\[ \text{redox} \,\,\, \text{non redox} \]
*If applicable:*
- Oxidizing Agent: _______________
- Reducing Agent: _______________
---
**b.** \( 3 \, \text{Cu} + 8 \, \text{HNO}_3 \rightarrow 3 \, \text{Cu(NO}_3\text{)}_2 + 2 \, \text{NO} + 4 \, \text{H}_2\text{O} \)
\[ \text{redox} \,\,\, \text{non redox} \]
*If applicable:*
- Oxidizing Agent: _______________
- Reducing Agent: _______________
---
**c.** \( \text{AgNO}_3 + \text{NaCl} \rightarrow \text{AgCl} + \text{NaNO}_3 \)
\[ \text{redox} \,\,\, \text{non redox} \]
*If applicable:*
- Oxidizing Agent: _______________
- Reducing Agent: _______________
---
Please use this worksheet to practice identifying and analyzing redox reactions. Consider how oxidation numbers change and determine the appropriate agents for each reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fef96925c-0e5d-45af-91ad-057e037999bb%2F0ba6c7e9-c104-4e85-9e90-7cd537b90755%2Fovtql3f_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Worksheet: Understanding Redox Reactions**
**Instructions:** For each of the following reactions:
i. With reference to oxidation numbers, indicate whether they are redox reactions. Circle your choice. Use oxidation numbers to justify your answer.
ii. For all redox reactions, identify the oxidizing or reducing agent. Explain using oxidation numbers.
---
**a.** \( \text{CuO} + \text{H}_2 \rightarrow \text{Cu} + \text{H}_2\text{O} \)
\[ \text{redox} \,\,\, \text{non redox} \]
*If applicable:*
- Oxidizing Agent: _______________
- Reducing Agent: _______________
---
**b.** \( 3 \, \text{Cu} + 8 \, \text{HNO}_3 \rightarrow 3 \, \text{Cu(NO}_3\text{)}_2 + 2 \, \text{NO} + 4 \, \text{H}_2\text{O} \)
\[ \text{redox} \,\,\, \text{non redox} \]
*If applicable:*
- Oxidizing Agent: _______________
- Reducing Agent: _______________
---
**c.** \( \text{AgNO}_3 + \text{NaCl} \rightarrow \text{AgCl} + \text{NaNO}_3 \)
\[ \text{redox} \,\,\, \text{non redox} \]
*If applicable:*
- Oxidizing Agent: _______________
- Reducing Agent: _______________
---
Please use this worksheet to practice identifying and analyzing redox reactions. Consider how oxidation numbers change and determine the appropriate agents for each reaction.
Expert Solution
Step 1
Redox reaction are those in which both oxidation and reduction reaction occurs simultaneously. Oxidation means loss of electrons and reduction means gain of electrons.
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