Using the values in Table 11.4 and ΔHsolution =-17.7 kJ / mol for KF, calculate the lattice ener

Name: Problem 28, Chapter 11: Chemistry The Science in Context
Uploaded: 2024-06-29T00:08:42-08:00
Channel: Susan Hallstrom
Description: Using the values in Table 11.4 and ΔHsolution =-17.7 kJ / mol for KF, calculate the lattice energy of KF.

step 1 In this problem, we are asked to find the heat of, or the lattice energy. And we are also given

Question

Using the values in Table 11.4 and $\Delta H_{\text {solution }}=-17.7 \mathrm{kJ} / \mathrm{mol}$ for KF, calculate the lattice energy of KF.

   Using the values in Table 11.4 and $\Delta H_{\text {solution }}=-17.7 \mathrm{kJ} / \mathrm{mol}$ for KF, calculate the lattice energy of KF.

Chemistry The Science in Context

Thomas R. Gilbert 5th Edition

Chapter 11, Problem 28

Instant Answer

Solved by Expert Susan Hallstrom

06/29/2024

Step 1

This is given by the sum of the enthalpy of hydration for each of its components. In this case, it is K+ and F-. From Table 11.4, we find that the enthalpy of hydration for K+ is -335 kJ/mol and for F- is -502 kJ/mol. So, the enthalpy of hydration for the solution Show more…

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Using the values in Table 11.4 and $\Delta H_{\text {solution }}=-17.7 \mathrm{kJ} / \mathrm{mol}$ for KF, calculate the lattice energy of KF.

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Key Concepts

Lattice Energy

Lattice energy is the energy required to completely separate one mole of an ionic solid into its gaseous ions. It is a measure of the strength of the bonds in the ionic lattice and is typically determined by the energy released when these ions come together to form the solid from infinite separation.

Enthalpy of Solution

Enthalpy of solution refers to the heat change that occurs when a solute dissolves in a solvent. For ionic compounds, this process involves overcoming the lattice energy to break the ionic solid and then releasing energy through interactions (hydration) between the ions and the solvent molecules.

Born-Haber Cycle

The Born-Haber cycle is a thermochemical cycle that uses Hess’s law to relate the lattice energy of an ionic compound to other measurable energetic quantities such as ionization energy, electron affinity, and the enthalpy of formation. By summing these steps, one can calculate or estimate the lattice energy indirectly.

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