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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![**Transcription for Educational Website**
---
**Chemical Solubility and Thermodynamics**
**Instructions:** This question has multiple parts. Work all the parts to get the most points.
**Problem Statement:**
A soluble salt, \( \text{MX}_2 \), is added to water in a beaker. The equation for the dissolving of the salt is:
\[ \text{MX}_2 (s) \rightarrow \text{M}^{2+} (aq) + 2\text{X}^{-} (aq); \quad \Delta H < 0 \]
**Discussion:**
- **Equation Breakdown:** The process described involves a solid salt (\( \text{MX}_2 (s) \)) dissolving in water to form aqueous ions (\( \text{M}^{2+} (aq) \) and \( 2\text{X}^{-} (aq) \)).
- **Thermodynamics Insight:** The enthalpy change (\( \Delta H \)) is less than zero, indicating that the dissolution process is exothermic.
**Exploration Question:**
Based on the equation and the thermodynamic data provided (\( \Delta H < 0 \)), will the dissolution make the solution in the beaker warmer or colder?
---](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F788121ef-4805-46b3-9141-6f4b24a2642f%2F3ed6d822-7520-4acd-8645-5e22bbb6aa45%2Fkfz26jg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Transcription for Educational Website**
---
**Chemical Solubility and Thermodynamics**
**Instructions:** This question has multiple parts. Work all the parts to get the most points.
**Problem Statement:**
A soluble salt, \( \text{MX}_2 \), is added to water in a beaker. The equation for the dissolving of the salt is:
\[ \text{MX}_2 (s) \rightarrow \text{M}^{2+} (aq) + 2\text{X}^{-} (aq); \quad \Delta H < 0 \]
**Discussion:**
- **Equation Breakdown:** The process described involves a solid salt (\( \text{MX}_2 (s) \)) dissolving in water to form aqueous ions (\( \text{M}^{2+} (aq) \) and \( 2\text{X}^{-} (aq) \)).
- **Thermodynamics Insight:** The enthalpy change (\( \Delta H \)) is less than zero, indicating that the dissolution process is exothermic.
**Exploration Question:**
Based on the equation and the thermodynamic data provided (\( \Delta H < 0 \)), will the dissolution make the solution in the beaker warmer or colder?
---
![### Question
After the salt dissolves and the solution returns to room temperature, what is the sign of \( q \) for the system?
- \( q < 0 \)
- \( q = 0 \)
- \( q > 0 \)
**[Submit Button]**
This question evaluates the understanding of thermodynamics related to the dissolution of salt in a solvent. The sign of \( q \) indicates whether the process is exothermic (\( q < 0 \)) or endothermic (\( q > 0 \)), or if there is no heat change (\( q = 0 \)).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F788121ef-4805-46b3-9141-6f4b24a2642f%2F3ed6d822-7520-4acd-8645-5e22bbb6aa45%2Fqq6vv08_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Question
After the salt dissolves and the solution returns to room temperature, what is the sign of \( q \) for the system?
- \( q < 0 \)
- \( q = 0 \)
- \( q > 0 \)
**[Submit Button]**
This question evaluates the understanding of thermodynamics related to the dissolution of salt in a solvent. The sign of \( q \) indicates whether the process is exothermic (\( q < 0 \)) or endothermic (\( q > 0 \)), or if there is no heat change (\( q = 0 \)).
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