Magnesium oxide forms from magnesium and oxygen: Use data in the table to calculate A.Says, AS surr, and AStotal for this reaction. State and Substance ΔΗ; (kJ/mol) Sᵒ [J/(K-mol)] 311.7 364.5 223.0 26.9 32.7 205.0 PCk (g) PCls (g) 2Mg(s) + O₂(g) → 2MgO(s) Cl₂(g) MgO(s) Mg(s) O₂(g) -287.0 -374.9 0 -601.7 0 0
Magnesium oxide forms from magnesium and oxygen: Use data in the table to calculate A.Says, AS surr, and AStotal for this reaction. State and Substance ΔΗ; (kJ/mol) Sᵒ [J/(K-mol)] 311.7 364.5 223.0 26.9 32.7 205.0 PCk (g) PCls (g) 2Mg(s) + O₂(g) → 2MgO(s) Cl₂(g) MgO(s) Mg(s) O₂(g) -287.0 -374.9 0 -601.7 0 0
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...
Related questions
Question
Estimate the temperature in K at which the reaction will become nonspontaneous.
![### Formation of Magnesium Oxide from Magnesium and Oxygen
The chemical reaction for the formation of magnesium oxide is given by:
\[ 2\text{Mg}(\text{s}) + \text{O}_2(\text{g}) \rightarrow 2\text{MgO}(\text{s}) \]
#### Thermodynamic Data Table
This data is used to calculate the changes in entropy and enthalpy for the surroundings, system, and total reaction.
| State and Substance | \(\Delta H^\circ_f \) (kJ/mol) | \( S^\circ \) [J/(K·mol)] |
|---------------------|-----------------|--------------------|
| \(\text{PCl}_3\)(g) | -287.0 | 311.7 |
| \(\text{PCl}_5\)(g) | -374.9 | 364.5 |
| \(\text{Cl}_2\)(g) | 0 | 223.0 |
| \(\text{MgO}\)(s) | -601.7 | 26.9 |
| \(\text{Mg}\)(s) | 0 | 32.7 |
| \(\text{O}_2\)(g) | 0 | 205.0 |
### Explanation
- **\(\Delta H^\circ_f\)**: Standard enthalpy of formation in kilojoules per mole (kJ/mol).
- **\(S^\circ\)**: Standard molar entropy in joules per Kelvin per mole \([J/(K·mol)]\).
This table includes values for several substances, including \(\text{MgO}\), which is crucial for calculations related to this exothermic reaction. The enthalpy of formation (\(\Delta H^\circ_f\)) and entropy (\(S^\circ\)) for each substance will assist in determining the thermodynamic properties of the reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff85a7368-ad51-49a6-b8f6-6f50d27fc24a%2Fe6947755-0b52-429d-8c19-bcc37eb7a025%2Fs22kyxg_processed.png&w=3840&q=75)
Transcribed Image Text:### Formation of Magnesium Oxide from Magnesium and Oxygen
The chemical reaction for the formation of magnesium oxide is given by:
\[ 2\text{Mg}(\text{s}) + \text{O}_2(\text{g}) \rightarrow 2\text{MgO}(\text{s}) \]
#### Thermodynamic Data Table
This data is used to calculate the changes in entropy and enthalpy for the surroundings, system, and total reaction.
| State and Substance | \(\Delta H^\circ_f \) (kJ/mol) | \( S^\circ \) [J/(K·mol)] |
|---------------------|-----------------|--------------------|
| \(\text{PCl}_3\)(g) | -287.0 | 311.7 |
| \(\text{PCl}_5\)(g) | -374.9 | 364.5 |
| \(\text{Cl}_2\)(g) | 0 | 223.0 |
| \(\text{MgO}\)(s) | -601.7 | 26.9 |
| \(\text{Mg}\)(s) | 0 | 32.7 |
| \(\text{O}_2\)(g) | 0 | 205.0 |
### Explanation
- **\(\Delta H^\circ_f\)**: Standard enthalpy of formation in kilojoules per mole (kJ/mol).
- **\(S^\circ\)**: Standard molar entropy in joules per Kelvin per mole \([J/(K·mol)]\).
This table includes values for several substances, including \(\text{MgO}\), which is crucial for calculations related to this exothermic reaction. The enthalpy of formation (\(\Delta H^\circ_f\)) and entropy (\(S^\circ\)) for each substance will assist in determining the thermodynamic properties of the reaction.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 5 steps with 6 images
Knowledge Booster
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
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY