Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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![**Calculating ΔS° for the Reaction at 25°C**
Given the following information, calculate ΔS° for the reaction:
\[ \text{SO}_3(g) + \text{H}_2\text{O}(l) \rightarrow \text{H}_2\text{SO}_4(l) \]
**Hint:** Because ΔS° is a state function (like ΔH°), you can use a table to calculate it in the same way. This means you should add up all the entropy for the products (times the number of each) and subtract all the entropy for the reactants.
**Entropy Values:**
| Species | S° (J/mol·K) |
|-------------|--------------|
| SO₃(g) | 256.2 |
| H₂O(l) | 69.9 |
| H₂SO₄(l) | 156.9 |
**Solution Choices:**
- a) 544.3 J/K
**Explanation:**
To calculate the standard entropy change (ΔS°) for the reaction, use the following equation:
\[ ΔS° = ΣS°_{\text{products}} - ΣS°_{\text{reactants}} \]
1. Calculate the sum of the entropies of the products:
- H₂SO₄(l): 156.9 J/mol·K
2. Calculate the sum of the entropies of the reactants:
- SO₃(g): 256.2 J/mol·K
- H₂O(l): 69.9 J/mol·K
3. Subtract the total entropy of the reactants from the total entropy of the products to find ΔS°.](https://content.bartleby.com/qna-images/question/065e3530-493f-4c36-b85d-4fbc9e0fed20/7d6cb2e7-122e-419a-9a87-43218657582b/7iupqam_processed.jpeg)
Transcribed Image Text:**Calculating ΔS° for the Reaction at 25°C**
Given the following information, calculate ΔS° for the reaction:
\[ \text{SO}_3(g) + \text{H}_2\text{O}(l) \rightarrow \text{H}_2\text{SO}_4(l) \]
**Hint:** Because ΔS° is a state function (like ΔH°), you can use a table to calculate it in the same way. This means you should add up all the entropy for the products (times the number of each) and subtract all the entropy for the reactants.
**Entropy Values:**
| Species | S° (J/mol·K) |
|-------------|--------------|
| SO₃(g) | 256.2 |
| H₂O(l) | 69.9 |
| H₂SO₄(l) | 156.9 |
**Solution Choices:**
- a) 544.3 J/K
**Explanation:**
To calculate the standard entropy change (ΔS°) for the reaction, use the following equation:
\[ ΔS° = ΣS°_{\text{products}} - ΣS°_{\text{reactants}} \]
1. Calculate the sum of the entropies of the products:
- H₂SO₄(l): 156.9 J/mol·K
2. Calculate the sum of the entropies of the reactants:
- SO₃(g): 256.2 J/mol·K
- H₂O(l): 69.9 J/mol·K
3. Subtract the total entropy of the reactants from the total entropy of the products to find ΔS°.
Transcribed Image Text:Below is the transcription of the image content, designed for an educational website:
---
**Species Entropy Values**
| Species | \( S^\circ \) (J/mol·K) |
|-----------|-----------------------|
| SO₃(g) | 256.2 |
| H₂O(l) | 69.9 |
| H₂SO₄(l) | 156.9 |
**Question:**
Calculate the change in entropy (\( \Delta S \)) for a given process using the above species.
**Options:**
a) 544.3 J/K
b) -175.8 J/K
c) -169.2 J/K
d) -64.21 J/K
---
This table provides standard molar entropy values for specific chemical species, and you are required to calculate the entropy change for a reaction involving these species. Select the correct entropy change from the options provided.
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