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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![The chemical reaction under consideration is:
\[ \text{Ca}(s) + 2 \text{H}_2\text{O}(\ell) \rightarrow \text{Ca(OH)}_2(\text{aq}) + \text{H}_2(\text{g}) \]
The table below displays the standard enthalpy of formation (\(\Delta_f H^\circ\)) and the standard entropy (\(S^\circ\)) for each substance involved in the reaction:
| Substance | \(\Delta_f H^\circ\) (kJ/mol) | \(S^\circ\) (J/K·mol) |
|-------------------|---------------------------|-------------------|
| Ca(s) | 0 | 41.59 |
| H\(_2\)O(\(\ell\))| -285.83 | 69.95 |
| Ca(OH)\(_2\)(aq) | -1002.82 | -74.5 |
| H\(_2\)(g) | 0 | 130.7 |](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7a354f1c-cdfd-41e5-a863-9a86a504af1c%2F8af7dd45-69f1-4f26-8409-fdc0f6029d9b%2F6flwi25_processed.png&w=3840&q=75)
Transcribed Image Text:The chemical reaction under consideration is:
\[ \text{Ca}(s) + 2 \text{H}_2\text{O}(\ell) \rightarrow \text{Ca(OH)}_2(\text{aq}) + \text{H}_2(\text{g}) \]
The table below displays the standard enthalpy of formation (\(\Delta_f H^\circ\)) and the standard entropy (\(S^\circ\)) for each substance involved in the reaction:
| Substance | \(\Delta_f H^\circ\) (kJ/mol) | \(S^\circ\) (J/K·mol) |
|-------------------|---------------------------|-------------------|
| Ca(s) | 0 | 41.59 |
| H\(_2\)O(\(\ell\))| -285.83 | 69.95 |
| Ca(OH)\(_2\)(aq) | -1002.82 | -74.5 |
| H\(_2\)(g) | 0 | 130.7 |
![**Spontaneity of a Reaction at 298 K**
The image poses a question regarding the spontaneity of a chemical reaction at 298 Kelvin. It offers two options to select from:
- ○ yes
- ○ no
This question is likely part of a learning module on thermodynamics, focusing on concepts such as Gibbs free energy to determine spontaneity. The spontaneity of a reaction can be calculated using the equation:
\[ \Delta G = \Delta H - T \Delta S \]
Where:
- \( \Delta G \) is the change in Gibbs free energy,
- \( \Delta H \) is the change in enthalpy,
- \( T \) is the temperature in Kelvin,
- \( \Delta S \) is the change in entropy.
A reaction is spontaneous when \( \Delta G < 0 \) (negative). At 298 K, students must evaluate the reaction conditions to determine if option "yes" or "no" is correct based on the provided data or context.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7a354f1c-cdfd-41e5-a863-9a86a504af1c%2F8af7dd45-69f1-4f26-8409-fdc0f6029d9b%2Ffhhizdf_processed.png&w=3840&q=75)
Transcribed Image Text:**Spontaneity of a Reaction at 298 K**
The image poses a question regarding the spontaneity of a chemical reaction at 298 Kelvin. It offers two options to select from:
- ○ yes
- ○ no
This question is likely part of a learning module on thermodynamics, focusing on concepts such as Gibbs free energy to determine spontaneity. The spontaneity of a reaction can be calculated using the equation:
\[ \Delta G = \Delta H - T \Delta S \]
Where:
- \( \Delta G \) is the change in Gibbs free energy,
- \( \Delta H \) is the change in enthalpy,
- \( T \) is the temperature in Kelvin,
- \( \Delta S \) is the change in entropy.
A reaction is spontaneous when \( \Delta G < 0 \) (negative). At 298 K, students must evaluate the reaction conditions to determine if option "yes" or "no" is correct based on the provided data or context.
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