onsider the equation below, which specie is the oxidizing agent? Cr- (aq) + Fe (s)-> (a) Cr(s) (b) Fe 17 Consider the following reactions: (c) a voltmeter (d) an aqueous solution 18. Cr (s) + Fe (c) Craq (aq) (d) Fe (aq) Zn² (aq)-> Zn (s) E = -0.76 V Ag (aq) Ag (s) E° = 0.80V What is the standard potential for the reaction? (a) 1.56 V (b) -1.56 V (c) -0.76 V (d) 0.04 V Which statement is true for an electrochemical cell built from an oxidation-reduction reaction (a) A G is positive, Eº is positive (c)) A Gº is negative, Eº is positive (b)) A Gº is positive, E' is negative (d)) A G is negative, Eº is negative
onsider the equation below, which specie is the oxidizing agent? Cr- (aq) + Fe (s)-> (a) Cr(s) (b) Fe 17 Consider the following reactions: (c) a voltmeter (d) an aqueous solution 18. Cr (s) + Fe (c) Craq (aq) (d) Fe (aq) Zn² (aq)-> Zn (s) E = -0.76 V Ag (aq) Ag (s) E° = 0.80V What is the standard potential for the reaction? (a) 1.56 V (b) -1.56 V (c) -0.76 V (d) 0.04 V Which statement is true for an electrochemical cell built from an oxidation-reduction reaction (a) A G is positive, Eº is positive (c)) A Gº is negative, Eº is positive (b)) A Gº is positive, E' is negative (d)) A G is negative, Eº is negative
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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16,17, & 18
![## Electrochemistry Practice Questions
### 16. Consider the equation below; which species is the oxidizing agent?
\[ \text{Cr}^{3+} \, (aq) + \text{Fe} \, (s) \rightarrow \text{Cr} \, (s) + \text{Fe}^{2+} \, (aq) \]
- (a) Cr (s)
- (b) Fe (s)
- (c) Cr\(^3\) \(aq\)
- (d) Fe\(^{2+}\) \(aq\)
### 17. Consider the following reactions:
Zn\(^{2+}\) \((aq)\) \(\rightarrow\) Zn \((s)\) \quad \(E^\circ = -0.76 \, V\)
Ag\(^+\) \((aq)\) \(\rightarrow\) Ag \((s)\) \quad \(E^\circ = 0.80 \, V\)
What is the standard potential for the reaction?
- (a) 1.56 V
- (b) -1.56 V
- (c) -0.76 V
- (d) 0.04 V
### 18. Which statement is true for an electrochemical cell built from an oxidation-reduction reaction?
- (a) \(\Delta G^\circ\) is positive, \(E^\circ\) is positive
- (b) \(\Delta G^\circ\) is positive, \(E^\circ\) is negative
- (c) \(\Delta G^\circ\) is negative, \(E^\circ\) is positive
- (d) \(\Delta G^\circ\) is negative, \(E^\circ\) is negative
### Explanation
These questions address key concepts in electrochemistry, such as identifying oxidizing and reducing agents, calculating standard electrode potentials, and understanding the relationship between Gibbs free energy change (\(\Delta G^\circ\)) and cell potential (\(E^\circ\)) in electrochemical cells.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6e037f4c-cb65-45a7-9b65-cb6a6aa1e30e%2Fecb97edc-201f-46b0-b845-f3a321c931e6%2F36hmqpj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:## Electrochemistry Practice Questions
### 16. Consider the equation below; which species is the oxidizing agent?
\[ \text{Cr}^{3+} \, (aq) + \text{Fe} \, (s) \rightarrow \text{Cr} \, (s) + \text{Fe}^{2+} \, (aq) \]
- (a) Cr (s)
- (b) Fe (s)
- (c) Cr\(^3\) \(aq\)
- (d) Fe\(^{2+}\) \(aq\)
### 17. Consider the following reactions:
Zn\(^{2+}\) \((aq)\) \(\rightarrow\) Zn \((s)\) \quad \(E^\circ = -0.76 \, V\)
Ag\(^+\) \((aq)\) \(\rightarrow\) Ag \((s)\) \quad \(E^\circ = 0.80 \, V\)
What is the standard potential for the reaction?
- (a) 1.56 V
- (b) -1.56 V
- (c) -0.76 V
- (d) 0.04 V
### 18. Which statement is true for an electrochemical cell built from an oxidation-reduction reaction?
- (a) \(\Delta G^\circ\) is positive, \(E^\circ\) is positive
- (b) \(\Delta G^\circ\) is positive, \(E^\circ\) is negative
- (c) \(\Delta G^\circ\) is negative, \(E^\circ\) is positive
- (d) \(\Delta G^\circ\) is negative, \(E^\circ\) is negative
### Explanation
These questions address key concepts in electrochemistry, such as identifying oxidizing and reducing agents, calculating standard electrode potentials, and understanding the relationship between Gibbs free energy change (\(\Delta G^\circ\)) and cell potential (\(E^\circ\)) in electrochemical cells.
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