**Estimating the Enthalpy Change of Formation (\( \Delta H_f^\circ \)) for Potassium Bromide**Use the following data to estimate \( \Delta H_f^\circ \) for potassium bromide:\[ \text{K(s)} + \frac{1}{2} \text{Br}_2(g) \rightarrow \text{KBr(s)} \]### Given Data:- **Lattice energy**: \(-671 \, \text{kJ/mol}\)- **Ionization energy for K**: \(419 \, \text{kJ/mol}\)- **Electron affinity of Br**: \(-325 \, \text{kJ/mol}\)- **Bond energy of Br}_2\)**: \(193 \, \text{kJ/mol}\)- **Enthalpy of sublimation for K**: \(90. \, \text{kJ/mol}\)### Objective:Calculate the standard enthalpy change of formation, \( \Delta H_f^\circ \), in kJ/mol.

Interpretation- To determine the ∆Hof of the potassium bromide , KBr (s) by the given information in the question . Concept- To determine the ∆Hof of the potassium bromide , KBr (s) by the given information , here we born haber cycle process of KBr .

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Use the following data to estimate AH; for potassium bromide. 1 K(s) + Br2 (g) KBr(s) Lattice energy -671 kJ/mol Ionization energy for K 419 kJ/mol Electron affinity of Br -325 kJ/mol Bond energy of Br2 193 kJ/mol Enthalpy of sublimation for K 90. kJ/mol AH = kJ/mol %3D

Use the following data to estimate AH; for potassium bromide. 1 K(s) + Br2 (g) KBr(s) Lattice energy -671 kJ/mol Ionization energy for K 419 kJ/mol Electron affinity of Br -325 kJ/mol Bond energy of Br2 193 kJ/mol Enthalpy of sublimation for K 90. kJ/mol AH = kJ/mol %3D

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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

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Question

**Estimating the Enthalpy Change of Formation (\( \Delta H_f^\circ \)) for Potassium Bromide**

Use the following data to estimate \( \Delta H_f^\circ \) for potassium bromide:

\[ \text{K(s)} + \frac{1}{2} \text{Br}_2(g) \rightarrow \text{KBr(s)} \]

### Given Data:
- **Lattice energy**: \(-671 \, \text{kJ/mol}\)
- **Ionization energy for K**: \(419 \, \text{kJ/mol}\)
- **Electron affinity of Br**: \(-325 \, \text{kJ/mol}\)
- **Bond energy of Br}_2\)**: \(193 \, \text{kJ/mol}\)
- **Enthalpy of sublimation for K**: \(90. \, \text{kJ/mol}\)

### Objective:
Calculate the standard enthalpy change of formation, \( \Delta H_f^\circ \), in kJ/mol.

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