For the reaction below, which statement best describes what is happening with the sign of AGO? 2 Cu CI O4la q) + N a20la q) - Cu2Os) + 2 Na CI O4la q) (exothermic) O The reaction is spontaneous at all temperatures. The reaction is non-spontaneous at all temperatures. The reaction is non-spontaneous at low temperature and spontaneous at high temperature. O The reaction is spontaneous at low temperature and non-spontaneous at high temperature.

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...
icon
Related questions
icon
Concept explainers
Question

6.

**Question:**

For the reaction below, which statement best describes what is happening with the sign of ΔG°?

\[ 
2 \text{CuClO}_4\text{(aq)} + \text{Na}_2\text{O}_2\text{(aq)} \rightarrow \text{Cu}_2\text{O(s)} + 2 \text{NaClO}_4\text{(aq)}  \, \text{(exothermic)}
\]

**Options:**

- A. The reaction is spontaneous at all temperatures.
- B. The reaction is non-spontaneous at all temperatures.
- C. The reaction is non-spontaneous at low temperature and spontaneous at high temperature.
- D. The reaction is spontaneous at low temperature and non-spontaneous at high temperature.

**Explanation:**

In an exothermic reaction, the sign of ΔH° is negative. For a reaction to be spontaneous, ΔG° must be negative. The relationship between ΔG°, ΔH°, and ΔS° is given by the Gibbs free energy equation:

\[ 
\Delta G° = \Delta H° - T\Delta S° 
\]

Here, since the reaction is exothermic, ΔH° is negative. Depending on the sign and magnitude of ΔS°, the reaction can show different temperature dependencies indicated in the options.
Transcribed Image Text:**Question:** For the reaction below, which statement best describes what is happening with the sign of ΔG°? \[ 2 \text{CuClO}_4\text{(aq)} + \text{Na}_2\text{O}_2\text{(aq)} \rightarrow \text{Cu}_2\text{O(s)} + 2 \text{NaClO}_4\text{(aq)} \, \text{(exothermic)} \] **Options:** - A. The reaction is spontaneous at all temperatures. - B. The reaction is non-spontaneous at all temperatures. - C. The reaction is non-spontaneous at low temperature and spontaneous at high temperature. - D. The reaction is spontaneous at low temperature and non-spontaneous at high temperature. **Explanation:** In an exothermic reaction, the sign of ΔH° is negative. For a reaction to be spontaneous, ΔG° must be negative. The relationship between ΔG°, ΔH°, and ΔS° is given by the Gibbs free energy equation: \[ \Delta G° = \Delta H° - T\Delta S° \] Here, since the reaction is exothermic, ΔH° is negative. Depending on the sign and magnitude of ΔS°, the reaction can show different temperature dependencies indicated in the options.
Expert Solution
Step 1

In this reaction change in entropy is negative beacuse no of particle decreasing 

And ∆H is negative

∆G=∆H-T∆S

So ∆G is negative at low temperature so ran is spontaneous and ∆G is positive at high temperature so reaction is non-spontaneous.

 

 

steps

Step by step

Solved in 2 steps

Blurred answer
Knowledge Booster
Ideal and Real Gases
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY