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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![**Title: Estimating the Enthalpy of Reaction for Sulfur Tetrafluoride Monoxide Formation**
**Introduction:**
Understanding chemical reactions involves estimating the energy changes that occur. This can be done by analyzing bond energies. Here, we will estimate the enthalpy change (\(\Delta H_{\text{rxn}}\)) for the formation of sulfur tetrafluoride monoxide (\(\text{SOF}_4\)).
**Chemical Structure:**
The Lewis structure of sulfur tetrafluoride monoxide (\(\text{SOF}_4\)) shows sulfur (S) centrally connected to an oxygen (O) atom and four fluorine (F) atoms, each with pairs of valence electrons indicating lone pairs around the F and O atoms.
**Bond Energies:**
Use the following bond energies (kJ/mol) to calculate the enthalpy change:
| Bond | Energy (kJ/mol) |
|-------|-----------------|
| S–F | 310 |
| S–O | 265 |
| S=O | 523 |
| O–O | 142 |
| O=O | 498 |
| O–F | 180 |
**Calculation:**
Estimate \(\Delta H_{\text{rxn}}\) using the bond energies provided to determine the overall energy change for breaking and forming bonds in the reaction.
**Enthalpy Change Calculation Box:**
\[ \Delta H_{\text{rxn}} = \text{(Fill in with calculation result)} \, \text{kJ/mol} \]
**Conclusion:**
Accurate knowledge of bond energies allows for the estimation of reaction energetics, crucial for predicting reaction behavior and stability.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc8ab2c5b-9b7e-4f04-bb69-d806282b0355%2F77526a71-f517-4ab1-bfbd-8fb68d12266f%2Fk5yif3n_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Estimating the Enthalpy of Reaction for Sulfur Tetrafluoride Monoxide Formation**
**Introduction:**
Understanding chemical reactions involves estimating the energy changes that occur. This can be done by analyzing bond energies. Here, we will estimate the enthalpy change (\(\Delta H_{\text{rxn}}\)) for the formation of sulfur tetrafluoride monoxide (\(\text{SOF}_4\)).
**Chemical Structure:**
The Lewis structure of sulfur tetrafluoride monoxide (\(\text{SOF}_4\)) shows sulfur (S) centrally connected to an oxygen (O) atom and four fluorine (F) atoms, each with pairs of valence electrons indicating lone pairs around the F and O atoms.
**Bond Energies:**
Use the following bond energies (kJ/mol) to calculate the enthalpy change:
| Bond | Energy (kJ/mol) |
|-------|-----------------|
| S–F | 310 |
| S–O | 265 |
| S=O | 523 |
| O–O | 142 |
| O=O | 498 |
| O–F | 180 |
**Calculation:**
Estimate \(\Delta H_{\text{rxn}}\) using the bond energies provided to determine the overall energy change for breaking and forming bonds in the reaction.
**Enthalpy Change Calculation Box:**
\[ \Delta H_{\text{rxn}} = \text{(Fill in with calculation result)} \, \text{kJ/mol} \]
**Conclusion:**
Accurate knowledge of bond energies allows for the estimation of reaction energetics, crucial for predicting reaction behavior and stability.
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