Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Using the values in Table 6.2, give ΔH for each reaction, and classify the reaction as endothermic or exothermic.**
**a.**
\[ \text{H-Br:} \rightarrow \text{H} \cdot + \cdot \text{Br:} \]
\[ \Delta H = \_\_\_\_ \text{kcal/mol} \]
(Select: Endothermic/Exothermic)
---
**b.**
\[ \text{H} \cdot + \cdot \text{Cl:} \rightarrow \text{H-Cl} \]
\[ \Delta H = \_\_\_\_ \text{kcal/mol} \]
(Select: Endothermic/Exothermic)
---
**c.**
\[ \text{H-OH} \rightarrow \text{H} \cdot + \cdot \text{OH} \]
\[ \Delta H = \_\_\_\_ \text{kcal/mol} \]
(Select: Endothermic/Exothermic)
---
**Explanation:**
This exercise involves calculating the enthalpy change (ΔH) for each of the given chemical reactions using data from Table 6.2 (not provided). You will then classify each reaction as either endothermic (absorbing heat) or exothermic (releasing heat).
Each part (a, b, c) represents a chemical reaction with spaces to fill in the ΔH value and to select whether the reaction is endothermic or exothermic. The dot (•) represents an unpaired electron, indicating the species are radicals.](https://content.bartleby.com/qna-images/question/2ecf5b80-2518-4246-9cf0-28fbc9ab655e/8cd3c29c-29d7-4975-8b7c-e70492d2a476/gmgc7ci_processed.jpeg)
Transcribed Image Text:**Using the values in Table 6.2, give ΔH for each reaction, and classify the reaction as endothermic or exothermic.**
**a.**
\[ \text{H-Br:} \rightarrow \text{H} \cdot + \cdot \text{Br:} \]
\[ \Delta H = \_\_\_\_ \text{kcal/mol} \]
(Select: Endothermic/Exothermic)
---
**b.**
\[ \text{H} \cdot + \cdot \text{Cl:} \rightarrow \text{H-Cl} \]
\[ \Delta H = \_\_\_\_ \text{kcal/mol} \]
(Select: Endothermic/Exothermic)
---
**c.**
\[ \text{H-OH} \rightarrow \text{H} \cdot + \cdot \text{OH} \]
\[ \Delta H = \_\_\_\_ \text{kcal/mol} \]
(Select: Endothermic/Exothermic)
---
**Explanation:**
This exercise involves calculating the enthalpy change (ΔH) for each of the given chemical reactions using data from Table 6.2 (not provided). You will then classify each reaction as either endothermic (absorbing heat) or exothermic (releasing heat).
Each part (a, b, c) represents a chemical reaction with spaces to fill in the ΔH value and to select whether the reaction is endothermic or exothermic. The dot (•) represents an unpaired electron, indicating the species are radicals.
Transcribed Image Text:**Table 6.2: Bond Dissociation Energies (ΔH) for Some Common Bonds**
This table presents the bond dissociation energies, which are measures of the strength of chemical bonds. The energy is expressed in kilocalories per mole (kcal/mol) and denotes the energy required to break the bond between atoms A and B, resulting in free radicals A· and ·B.
- **H—H**: +104 kcal/mol
- **F—F**: +38 kcal/mol
- **Cl—Cl**: +58 kcal/mol
- **Br—Br**: +46 kcal/mol
- **I—I**: +36 kcal/mol
- **H—OH**: +119 kcal/mol
- **H—F**: +136 kcal/mol
- **H—Cl**: +103 kcal/mol
- **H—Br**: +88 kcal/mol
- **H—I**: +71 kcal/mol
This information is crucial for understanding the stability and reactivity of molecules in various chemical reactions. Higher ΔH values signify stronger bonds that require more energy to break.
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