2. Calculate AS° for the reaction: Substance: S°(J/K mol): SiCl4(g) + 2Mg(s) → 2MgCl₂(s) + Si(s) SiCl4(g) 330.73 Mg(s) 32.68 MgCl₂(s) 89.62 Si(s) 18.83
2. Calculate AS° for the reaction: Substance: S°(J/K mol): SiCl4(g) + 2Mg(s) → 2MgCl₂(s) + Si(s) SiCl4(g) 330.73 Mg(s) 32.68 MgCl₂(s) 89.62 Si(s) 18.83
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 problem asks to calculate the standard entropy change (\( \Delta S^\circ \)) for the reaction:
\[
\text{SiCl}_4(g) + 2\text{Mg}(s) \rightarrow 2\text{MgCl}_2(s) + \text{Si}(s)
\]
**Table of Standard Entropies (\( S^\circ \)) in J/K·mol:**
| Substance | \( \text{SiCl}_4(g) \) | \( \text{Mg}(s) \) | \( \text{MgCl}_2(s) \) | \( \text{Si}(s) \) |
|----------------|------------------------|-------------------|-----------------------|-----------------|
| \( S^\circ \) (J/K·mol) | 330.73 | 32.68 | 89.62 | 18.83 |
**Options for \( \Delta S^\circ \):**
A) –254.96 J/K
B) –198.02 J/K
C) 198.02 J/K
D) 254.96 J/K
To solve this, use the standard entropy change formula:
\[
\Delta S^\circ = \sum S^\circ_{\text{products}} - \sum S^\circ_{\text{reactants}}
\]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F52d8280a-7ac0-487b-875a-b87cea38d519%2F2c5068a4-b5ca-4b2f-9aab-a44c29cf4722%2Fkz94e75_processed.png&w=3840&q=75)
Transcribed Image Text:The problem asks to calculate the standard entropy change (\( \Delta S^\circ \)) for the reaction:
\[
\text{SiCl}_4(g) + 2\text{Mg}(s) \rightarrow 2\text{MgCl}_2(s) + \text{Si}(s)
\]
**Table of Standard Entropies (\( S^\circ \)) in J/K·mol:**
| Substance | \( \text{SiCl}_4(g) \) | \( \text{Mg}(s) \) | \( \text{MgCl}_2(s) \) | \( \text{Si}(s) \) |
|----------------|------------------------|-------------------|-----------------------|-----------------|
| \( S^\circ \) (J/K·mol) | 330.73 | 32.68 | 89.62 | 18.83 |
**Options for \( \Delta S^\circ \):**
A) –254.96 J/K
B) –198.02 J/K
C) 198.02 J/K
D) 254.96 J/K
To solve this, use the standard entropy change formula:
\[
\Delta S^\circ = \sum S^\circ_{\text{products}} - \sum S^\circ_{\text{reactants}}
\]
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