Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Educational Website Transcription:**
**Free Energy Calculation for Chemical Reactions**
The standard reaction free energy \( \Delta G^\circ = 1100. \, \text{kJ} \) is provided for this specific chemical reaction:
\[ 4 \text{PCl}_3(g) \rightarrow \text{P}_4(g) + 6 \text{Cl}_2(g) \]
Using this information, you will need to complete the table below. Make sure to round each of your answers to the nearest kilojoule (kJ).
| **Reaction** | \( \Delta G^\circ \) |
|--------------|------------------------|
| \( \text{P}_4(g) + 6 \text{Cl}_2(g) \rightarrow 4 \text{PCl}_3(g) \) | [ ] kJ |
| \( \frac{1}{4} \text{P}_4(g) + \frac{3}{2} \text{Cl}_2(g) \rightarrow \text{PCl}_3(g) \) | [ ] kJ |
| \( 8 \text{PCl}_3(g) \rightarrow 2 \text{P}_4(g) + 12 \text{Cl}_2(g) \) | [ ] kJ |
**Explanation for Educators:**
- **Diagram/Equation Explanation**: The chemical equations in the table demonstrate various forms of phosphorus and chlorine transformations to phosphorous trichloride (\(\text{PCl}_3\)) and its reverse reactions.
- **Problem Solving**: Students should utilize the provided standard reaction free energy to calculate the unknown Gibbs free energies based on the stoichiometry of each reaction. Use principles such as reaction inversion and proportional stoichiometry to solve.
- **Learning Outcome**: Students will gain skills in applying thermodynamic principles to predict the directionality and feasibility of chemical reactions.
Use the table and provided information to enhance understanding of reaction spontaneity and energy change calculations in chemical processes.](https://content.bartleby.com/qna-images/question/14977a0d-3296-466e-81da-31d1738097d5/4607495a-45ed-482c-b911-0f8d1de88143/fa7i6ii_processed.png)
Transcribed Image Text:**Educational Website Transcription:**
**Free Energy Calculation for Chemical Reactions**
The standard reaction free energy \( \Delta G^\circ = 1100. \, \text{kJ} \) is provided for this specific chemical reaction:
\[ 4 \text{PCl}_3(g) \rightarrow \text{P}_4(g) + 6 \text{Cl}_2(g) \]
Using this information, you will need to complete the table below. Make sure to round each of your answers to the nearest kilojoule (kJ).
| **Reaction** | \( \Delta G^\circ \) |
|--------------|------------------------|
| \( \text{P}_4(g) + 6 \text{Cl}_2(g) \rightarrow 4 \text{PCl}_3(g) \) | [ ] kJ |
| \( \frac{1}{4} \text{P}_4(g) + \frac{3}{2} \text{Cl}_2(g) \rightarrow \text{PCl}_3(g) \) | [ ] kJ |
| \( 8 \text{PCl}_3(g) \rightarrow 2 \text{P}_4(g) + 12 \text{Cl}_2(g) \) | [ ] kJ |
**Explanation for Educators:**
- **Diagram/Equation Explanation**: The chemical equations in the table demonstrate various forms of phosphorus and chlorine transformations to phosphorous trichloride (\(\text{PCl}_3\)) and its reverse reactions.
- **Problem Solving**: Students should utilize the provided standard reaction free energy to calculate the unknown Gibbs free energies based on the stoichiometry of each reaction. Use principles such as reaction inversion and proportional stoichiometry to solve.
- **Learning Outcome**: Students will gain skills in applying thermodynamic principles to predict the directionality and feasibility of chemical reactions.
Use the table and provided information to enhance understanding of reaction spontaneity and energy change calculations in chemical processes.
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