Given the reactions shown below, identify the reactant that is a. oxidized: b. reduced: c. reducing agent: d. oxidizing agent: Overall reaction: 2 AgNO3 + Cu →2 Ag+ Cu(NO3)2 Look closer at the oxidation half-reaction and the reduction half-reaction shown below: Ag+ + e Ag Cu Cu2+ + 2 e
Given the reactions shown below, identify the reactant that is a. oxidized: b. reduced: c. reducing agent: d. oxidizing agent: Overall reaction: 2 AgNO3 + Cu →2 Ag+ Cu(NO3)2 Look closer at the oxidation half-reaction and the reduction half-reaction shown below: Ag+ + e Ag Cu Cu2+ + 2 e
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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**Redox Reactions in Chemistry**
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Given the reactions shown below, identify the reactant that is:
a. **oxidized:**
b. **reduced:**
c. **reducing agent:**
d. **oxidizing agent:**
**Overall reaction:**
\[ 2 \text{AgNO}_3 + \text{Cu} \rightarrow 2 \text{Ag} + \text{Cu(NO}_3\text{)}_2 \]
**Look closer at the oxidation half-reaction and the reduction half-reaction shown below:**
\[ \text{Ag}^+ + e^- \rightarrow \text{Ag} \]
\[ \text{Cu} \rightarrow \text{Cu}^{2+} + 2 e^- \]
**Explanation:**
- In the overall reaction, silver nitrate (\(\text{AgNO}_3\)) reacts with copper (\(\text{Cu}\)) to produce silver (\(\text{Ag}\)) and copper(II) nitrate (\(\text{Cu(NO}_3\text{)}_2\)).
- The oxidation half-reaction shows silver ions (\(\text{Ag}^+\)) gaining an electron (\(e^-\)) to form silver (\(\text{Ag}\)). This indicates reduction as the silver ion gains an electron.
- The reduction half-reaction shows copper (\(\text{Cu}\)) losing two electrons to form copper ions (\(\text{Cu}^{2+}\)). This indicates oxidation as copper loses electrons.
From the reactions:
- The copper (\(\text{Cu}\)) is **oxidized** (loses electrons).
- The silver ion (\(\text{Ag}^+\)) is **reduced** (gains electrons).
- The substance that gets oxidized, copper (\(\text{Cu}\)), is the **reducing agent**.
- The substance that gets reduced, silver ion (\(\text{Ag}^+\)), is the **oxidizing agent**.
Fill in the blanks accordingly for practice and learning.
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Transcribed Image Text:---
**Redox Reactions in Chemistry**
---
Given the reactions shown below, identify the reactant that is:
a. **oxidized:**
b. **reduced:**
c. **reducing agent:**
d. **oxidizing agent:**
**Overall reaction:**
\[ 2 \text{AgNO}_3 + \text{Cu} \rightarrow 2 \text{Ag} + \text{Cu(NO}_3\text{)}_2 \]
**Look closer at the oxidation half-reaction and the reduction half-reaction shown below:**
\[ \text{Ag}^+ + e^- \rightarrow \text{Ag} \]
\[ \text{Cu} \rightarrow \text{Cu}^{2+} + 2 e^- \]
**Explanation:**
- In the overall reaction, silver nitrate (\(\text{AgNO}_3\)) reacts with copper (\(\text{Cu}\)) to produce silver (\(\text{Ag}\)) and copper(II) nitrate (\(\text{Cu(NO}_3\text{)}_2\)).
- The oxidation half-reaction shows silver ions (\(\text{Ag}^+\)) gaining an electron (\(e^-\)) to form silver (\(\text{Ag}\)). This indicates reduction as the silver ion gains an electron.
- The reduction half-reaction shows copper (\(\text{Cu}\)) losing two electrons to form copper ions (\(\text{Cu}^{2+}\)). This indicates oxidation as copper loses electrons.
From the reactions:
- The copper (\(\text{Cu}\)) is **oxidized** (loses electrons).
- The silver ion (\(\text{Ag}^+\)) is **reduced** (gains electrons).
- The substance that gets oxidized, copper (\(\text{Cu}\)), is the **reducing agent**.
- The substance that gets reduced, silver ion (\(\text{Ag}^+\)), is the **oxidizing agent**.
Fill in the blanks accordingly for practice and learning.
---
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