**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. **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/molThis 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.

Answer:When during a reaction energy gets released then it is an exothermic reaction and when during…

Using the values in Table 6.2, give AH for each reaction, and classify the reaction as endothermic or exothermic. a. AH = H-Br: (select) b. AH= C. (select) H. + ·ÖK: →→→ H¬CI: - нӧн AH= - H. + Br: (select) kcal/mol kcal/mol → H. + ÖH kcal/mol

Using the values in Table 6.2, give AH for each reaction, and classify the reaction as endothermic or exothermic. a. AH = H-Br: (select) b. AH= C. (select) H. + ·ÖK: →→→ H¬CI: - нӧн AH= - H. + Br: (select) kcal/mol kcal/mol → H. + ÖH kcal/mol

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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