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

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

Chemistry
Chemistry
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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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**Estimating the Enthalpy of Formation for Potassium Bromide** To estimate the enthalpy change of formation \(\Delta H_f^\circ\) for potassium bromide (KBr), use the provided thermodynamic data and the balanced chemical equation: \[ \text{K(s)} + \frac{1}{2} \text{Br}_2(g) \rightarrow \text{KBr(s)} \] **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 \(\Delta H_f^\circ\) for KBr(s): \[ \Delta H_f^\circ = \, \_ \, \text{kJ/mol} \] **Explanation:** To find the enthalpy change of formation, consider the steps required to form KBr from its elements. The calculation involves using Hess's Law, which considers formation, sublimation, ionization, electron affinity, and lattice energy to determine the overall enthalpy change.
Transcribed Image Text:**Estimating the Enthalpy of Formation for Potassium Bromide** To estimate the enthalpy change of formation \(\Delta H_f^\circ\) for potassium bromide (KBr), use the provided thermodynamic data and the balanced chemical equation: \[ \text{K(s)} + \frac{1}{2} \text{Br}_2(g) \rightarrow \text{KBr(s)} \] **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 \(\Delta H_f^\circ\) for KBr(s): \[ \Delta H_f^\circ = \, \_ \, \text{kJ/mol} \] **Explanation:** To find the enthalpy change of formation, consider the steps required to form KBr from its elements. The calculation involves using Hess's Law, which considers formation, sublimation, ionization, electron affinity, and lattice energy to determine the overall enthalpy change.
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