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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Calculate the molar enthalpy of formation, Δf, of solid lithium fluoride from the lattice energy (Table 12.1) and other thermochemical data. The enthalpy of formation of Li(g), Δf [Li(g)] = 159.37 kJ/mol. Other required data can be found in Appendices F and L.

TABLE 12.1

Lattice Energies of Some Ionic Compounds

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Interpretation Introduction

Interpretation:

The molar enthalpy formation of lithium fluoride has to be calculated.

Concept introduction:

The molar enthalpy formation is calculated by using following method,

ΔfHo=ΔsubHo+IE+Do+EA+ΔlatticeU

Explanation

The molar enthalpy formation is calculated by using Hess law, the enthalpy of the formation is given below

ΔfHo=ΔsubHo+IE+Do+EA+ΔlatticeUΔsubHo=+159.37kJ/molIE=+520kJ/molDo=+78

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