The molar enthalpy formation of lithium fluoride has to be calculated. Concept introduction: The molar enthalpy formation is calculated by using following method, Δ f H o = Δ sub H o + IE +D o + EA+ Δ lattice U

Question

16). Using the thermochemical data below calculate the lattice energy for the formation of Na₂O. Na(s) → Na(g) 107.3 kJ/mol Na(g) → Na (g) + 1 e - 495.9 kJ/mol -418 kJ/mol 249.1 kJ/mol -141 kJ/mol -1484.5 kJ/mol 2 Na(s) + O₂(g) →→→ Na₂O(s) 1/2 O₂(g) → 0(g) O(g) + 1 e→O(g) O(g) +1e0²(g)

Answer 1

Question

Chapter 12, Problem 17PS

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+ Δ latticeU

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16). Using the thermochemical data below calculate the lattice energy for the formation of Na₂O. Na(s) → Na(g) 107.3 kJ/mol Na(g) → Na (g) + 1 e - 495.9 kJ/mol -418 kJ/mol 249.1 kJ/mol -141 kJ/mol -1484.5 kJ/mol 2 Na(s) + O₂(g) →→→ Na₂O(s) 1/2 O₂(g) → 0(g) O(g) + 1 e→O(g) O(g) +1e0²(g)

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