### Calculating Standard Entropy Change for the Reaction:**Reaction:**\[ \text{H}_2(\text{g}) + \text{Br}_2(\text{l}) \rightarrow 2 \text{HBr}(\text{g}) \]To find the value of standard entropy change, ΔSº, for the reaction, we use the given standard thermodynamic properties of the substances involved.**Given Table:**#### Standard Thermodynamic Properties for Selected Substances| Substance | \(\Delta H_f^\circ\) (kJ mol⁻¹) | \(\Delta G_f^\circ\) (kJ mol⁻¹) | \(S^\circ\) (J K⁻¹ mol⁻¹) ||-----------|---------------------|-----------------------|-------------------------------|| \(\text{Br}_2(\text{l})\) | 0 | 0 | 152.23 || \(\text{Br}_2(\text{g})\) | 30.91 | 3.142 | 245.5 || \(\text{Br}(\text{g})\) | 111.88 | 82.429 | 175.0 || \(\text{Br}^-\) (aq) | -120.9 | -102.82 | 80.71 || \(\text{BrF}_3(\text{g})\) | -255.60 | -229.45 | 292.42 || \(\text{HBr}(\text{g})\) | -36.3 | -53.43 | 198.7 |#### Steps to Calculate \(\Delta S^\circ_{\text{reaction}}\):1. **Identify the standard entropy values (\(S^\circ\)) for each substance:** - \(S^\circ (\text{H}_2(\text{g}))\) = **Assumed Known for Calculation** - \(S^\circ (\text{Br}_2(\text{l}))\) = 152.23 J K⁻¹ mol⁻¹ - \(S^\circ (\text{HBr}(\text{g}))\) = 198.7 J K⁻¹ mol⁻¹2. **Apply the formula for the standard entropy change:** \[ \Delta

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Use the table below to answer the questions that follow. The value of standard entropy change, AS°, for the following reaction, H2(g) + Br2(1) → 2 HBr(g) is J/K.

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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Question

### Calculating Standard Entropy Change for the Reaction:

**Reaction:**
\[ \text{H}_2(\text{g}) + \text{Br}_2(\text{l}) \rightarrow 2 \text{HBr}(\text{g}) \]

To find the value of standard entropy change, ΔSº, for the reaction, we use the given standard thermodynamic properties of the substances involved.

**Given Table:**

#### Standard Thermodynamic Properties for Selected Substances

| Substance | \(\Delta H_f^\circ\) (kJ mol⁻¹) | \(\Delta G_f^\circ\) (kJ mol⁻¹) | \(S^\circ\) (J K⁻¹ mol⁻¹) |
|-----------|---------------------|-----------------------|-------------------------------|
| \(\text{Br}_2(\text{l})\) | 0 | 0 | 152.23 |
| \(\text{Br}_2(\text{g})\) | 30.91 | 3.142 | 245.5 |
| \(\text{Br}(\text{g})\) | 111.88 | 82.429 | 175.0 |
| \(\text{Br}^-\) (aq) | -120.9 | -102.82 | 80.71 |
| \(\text{BrF}_3(\text{g})\) | -255.60 | -229.45 | 292.42 |
| \(\text{HBr}(\text{g})\) | -36.3 | -53.43 | 198.7 |

#### Steps to Calculate \(\Delta S^\circ_{\text{reaction}}\):

1. **Identify the standard entropy values (\(S^\circ\)) for each substance:**
- \(S^\circ (\text{H}_2(\text{g}))\) = **Assumed Known for Calculation**
- \(S^\circ (\text{Br}_2(\text{l}))\) = 152.23 J K⁻¹ mol⁻¹
- \(S^\circ (\text{HBr}(\text{g}))\) = 198.7 J K⁻¹ mol⁻¹

2. **Apply the formula for the standard entropy change:**
\[
\Delta

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