**Redox Reactions: Identifying Oxidation and Reduction**In the following redox reactions, identify what is oxidized and what is reduced.a. \( \text{Zn(s)} + 2\text{Ag}^+(aq) \rightarrow \text{Zn}^{2+}(aq) + 2\text{Ag(s)} \)b. \( \text{Sn}^{2+}(aq) + 2\text{Ce}^{4+}(aq) \rightarrow \text{Sn}^{4+}(aq) + 2\text{Ce}^{3+}(aq) \)c. \( 2\text{Al(s)} + 3\text{Br}_2(g) \rightarrow 2\text{AlBr}_3(aq) \)d. \( \text{H}_2(g) + \text{Cl}_2(g) \rightarrow 2\text{HCl}(aq) \)e. \( 2\text{CO}(g) + \text{O}_2(g) \rightarrow 2\text{CO}_2(g) \) For each reaction, determine the species that lose electrons (oxidized) and the species that gain electrons (reduced).

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4.4 In the following redox reactions, identify what is oxidized and what is reduced- 3+ a. Zn(s) + 2Ag (aq) b. Sn²+(aq) + 2Ce** (aq) → Sn(aq) + 2Ce³+ (aq) c. 2Au(s) + 6H*(aq) 2Au³+ (aq) + 3H2₂(g) d. 4Co(s) + 302(g) ->> 2C0203(s) e. 2CO(g) + O2(g) 2CO2(g) -> 2+ Zn²+ (aq) + 2Ag(s)

4.4 In the following redox reactions, identify what is oxidized and what is reduced- 3+ a. Zn(s) + 2Ag (aq) b. Sn²+(aq) + 2Ce** (aq) → Sn(aq) + 2Ce³+ (aq) c. 2Au(s) + 6H*(aq) 2Au³+ (aq) + 3H2₂(g) d. 4Co(s) + 302(g) ->> 2C0203(s) e. 2CO(g) + O2(g) 2CO2(g) -> 2+ Zn²+ (aq) + 2Ag(s)

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: Identifying Oxidation and Reduction**

In the following redox reactions, identify what is oxidized and what is reduced.

a. \( \text{Zn(s)} + 2\text{Ag}^+(aq) \rightarrow \text{Zn}^{2+}(aq) + 2\text{Ag(s)} \)

b. \( \text{Sn}^{2+}(aq) + 2\text{Ce}^{4+}(aq) \rightarrow \text{Sn}^{4+}(aq) + 2\text{Ce}^{3+}(aq) \)

c. \( 2\text{Al(s)} + 3\text{Br}_2(g) \rightarrow 2\text{AlBr}_3(aq) \)

d. \( \text{H}_2(g) + \text{Cl}_2(g) \rightarrow 2\text{HCl}(aq) \)

e. \( 2\text{CO}(g) + \text{O}_2(g) \rightarrow 2\text{CO}_2(g) \)

For each reaction, determine the species that lose electrons (oxidized) and the species that gain electrons (reduced).

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