Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following reaction between hydrochloric acid and oxygen. HC(aq) + O2(g) –H¿O(1) + Cl½(g) species oxidized species reduced oxidizing agent reducing agent
Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following reaction between hydrochloric acid and oxygen. HC(aq) + O2(g) –H¿O(1) + Cl½(g) species oxidized species reduced oxidizing agent reducing agent
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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![**Identifying Redox Species in a Chemical Reaction**
**Objective:**
Identify the species oxidized, the species reduced, the oxidizing agent, and the reducing agent in the following reaction between hydrochloric acid and oxygen.
**Reaction:**
\[ \text{HCl}(aq) + \text{O}_2(g) \rightarrow \text{H}_2\text{O}(l) + \text{Cl}_2(g) \]
**Fill in the following information:**
1. **Species Oxidized:**
- _[Blank Box]_
2. **Species Reduced:**
- _[Blank Box]_
3. **Oxidizing Agent:**
- _[Blank Box]_
4. **Reducing Agent:**
- _[Blank Box]_
**Explanation of the Reaction:**
- In this reaction, hydrochloric acid (HCl) reacts with oxygen (O₂) to produce water (H₂O) and chlorine gas (Cl₂).
- To identify the species oxidized and reduced, we need to analyze the change in oxidation states of the elements involved.
**Educational Guide:**
1. **Oxidation State Changes:**
- **Hydrogen (H)** in HCl has an oxidation state of +1.
- **Chlorine (Cl)** in HCl has an oxidation state of -1.
- **Oxygen (O)** in O₂ has an oxidation state of 0.
During the reaction:
- **H in H₂O** retains an oxidation state of +1.
- **O in H₂O** has an oxidation state of -2.
- **Cl in Cl₂** changes to an oxidation state of 0 from -1 in HCl.
2. **Determine Species Oxidized and Reduced:**
- **Species Oxidized:** Chlorine (Cl) is oxidized from -1 to 0.
- **Species Reduced:** Oxygen (O) is reduced from 0 to -2.
3. **Determine the Oxidizing and Reducing Agents:**
- **Oxidizing Agent:** The substance that is reduced (gains electrons) is O₂, hence it is the oxidizing agent.
- **Reducing Agent:** The substance that is oxidized (loses electrons) is HCl, hence it is the reducing agent.
By filling in the boxes with this](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5c33053e-aa43-49cf-b2bb-78272e2ba689%2Fd53d5a63-cf16-4b99-ae35-edb93d7d8e6e%2Fe7pqcfj.png&w=3840&q=75)
Transcribed Image Text:**Identifying Redox Species in a Chemical Reaction**
**Objective:**
Identify the species oxidized, the species reduced, the oxidizing agent, and the reducing agent in the following reaction between hydrochloric acid and oxygen.
**Reaction:**
\[ \text{HCl}(aq) + \text{O}_2(g) \rightarrow \text{H}_2\text{O}(l) + \text{Cl}_2(g) \]
**Fill in the following information:**
1. **Species Oxidized:**
- _[Blank Box]_
2. **Species Reduced:**
- _[Blank Box]_
3. **Oxidizing Agent:**
- _[Blank Box]_
4. **Reducing Agent:**
- _[Blank Box]_
**Explanation of the Reaction:**
- In this reaction, hydrochloric acid (HCl) reacts with oxygen (O₂) to produce water (H₂O) and chlorine gas (Cl₂).
- To identify the species oxidized and reduced, we need to analyze the change in oxidation states of the elements involved.
**Educational Guide:**
1. **Oxidation State Changes:**
- **Hydrogen (H)** in HCl has an oxidation state of +1.
- **Chlorine (Cl)** in HCl has an oxidation state of -1.
- **Oxygen (O)** in O₂ has an oxidation state of 0.
During the reaction:
- **H in H₂O** retains an oxidation state of +1.
- **O in H₂O** has an oxidation state of -2.
- **Cl in Cl₂** changes to an oxidation state of 0 from -1 in HCl.
2. **Determine Species Oxidized and Reduced:**
- **Species Oxidized:** Chlorine (Cl) is oxidized from -1 to 0.
- **Species Reduced:** Oxygen (O) is reduced from 0 to -2.
3. **Determine the Oxidizing and Reducing Agents:**
- **Oxidizing Agent:** The substance that is reduced (gains electrons) is O₂, hence it is the oxidizing agent.
- **Reducing Agent:** The substance that is oxidized (loses electrons) is HCl, hence it is the reducing agent.
By filling in the boxes with this
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