The reverse copper disproportion reaction has been proposed to etch solid copper: Cu + Cu²+ (1)→ 2Cut (1) Determine the equilibrium constant of the disproportionation reaction using the following half-cell reactions: Cu² (1) + e→ Cut (1) Cu → Cu*(1) + e E = 0.153 V Eº = -0.521 V
The reverse copper disproportion reaction has been proposed to etch solid copper: Cu + Cu²+ (1)→ 2Cut (1) Determine the equilibrium constant of the disproportionation reaction using the following half-cell reactions: Cu² (1) + e→ Cut (1) Cu → Cu*(1) + e E = 0.153 V Eº = -0.521 V
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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![**Title: Understanding the Copper Disproportionation Reaction**
The reverse copper disproportionation reaction has been proposed to etch solid copper. This reaction can be represented as:
\[ \text{Cu} + \text{Cu}^{2+}(l) \rightarrow 2\text{Cu}^+(l) \]
To determine the equilibrium constant of this disproportionation reaction, we can use the following half-cell reactions:
1. \[ \text{Cu}^{2+}(l) + e^- \rightarrow \text{Cu}^+(l) \]
\[ E^{\circ} = 0.153 \, \text{V} \]
2. \[ \text{Cu} \rightarrow \text{Cu}^+(l) + e^- \]
\[ E^{\circ} = -0.521 \, \text{V} \]
**Explanation of Electrochemical Data:**
- The first reaction involves the reduction of copper(II) ions to copper(I) ions with a standard electrode potential of \(0.153 \, \text{V}\).
- The second reaction involves the oxidation of solid copper to copper(I) ions with a standard electrode potential of \(-0.521 \, \text{V}\).
By understanding these half-reactions, you can calculate the overall cell potential and, subsequently, the equilibrium constant for the reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7447eb07-fceb-4d7b-a8f5-73349ee04b18%2Feb6693fb-cc5e-4b9d-b888-acfebecdd0f0%2Fvsmhfib_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Understanding the Copper Disproportionation Reaction**
The reverse copper disproportionation reaction has been proposed to etch solid copper. This reaction can be represented as:
\[ \text{Cu} + \text{Cu}^{2+}(l) \rightarrow 2\text{Cu}^+(l) \]
To determine the equilibrium constant of this disproportionation reaction, we can use the following half-cell reactions:
1. \[ \text{Cu}^{2+}(l) + e^- \rightarrow \text{Cu}^+(l) \]
\[ E^{\circ} = 0.153 \, \text{V} \]
2. \[ \text{Cu} \rightarrow \text{Cu}^+(l) + e^- \]
\[ E^{\circ} = -0.521 \, \text{V} \]
**Explanation of Electrochemical Data:**
- The first reaction involves the reduction of copper(II) ions to copper(I) ions with a standard electrode potential of \(0.153 \, \text{V}\).
- The second reaction involves the oxidation of solid copper to copper(I) ions with a standard electrode potential of \(-0.521 \, \text{V}\).
By understanding these half-reactions, you can calculate the overall cell potential and, subsequently, the equilibrium constant for the reaction.
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