1. showing the complete Born-Haber for the lattice energy of KCl(s).
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1. showing the complete Born-Haber for the lattice energy of KCl(s).
Part I. Use a Born-Haber cycle to calculate the lattice energy of KCl from the following data. (5 marks) Ionization energy of K(g) = 444.0 kJ mol-1 Electron Affinity of Cl(g) = -381.0 kJ mol-1 Energy to Sublime K(s) = 152.0 kJ mol-1 Bond energy of Cl2 = 201.0 kJ mol-1 ∆rH for K(s) + 1/2 Cl2(g) ↔ KCl(s) = -480.0 kJ mol-1 art II. Using the lattice energy calculated in part I determine the enthalpy of solution potassium chloride...
Draw the Born-Haber Cycle with these values and calculate
lattice energy.
Problem 1: Label each reaction listed below for the Born-Haber cycle in the formation of Cao lattice and calculate the lattice energy of Cal given the following information. AH KD) Ca(s) + Ca(8) 193 Calg) - Cat (8) + e 590 Cat (8) - Cat (8) + e- 2 O(g) + O2(g) O(8) + e- O (8) -141 O (8) + e- O (8) 878 Ca(s) + O2(g) →...
Discuss the relationship of calculating lattice energy and the Born-Haber cycle. Here are some suggestions of topics on which to elaborate upon in your explanations: Provide an explanation of the Born-Haber cycle. Explain the difference between ionization energy and electron affinity. Explain how the enthaply of formation is related to the Born-Haber cycle.
C) Lattice Energy Determine the standard formation energy of the following ionic compounds using the Born-Haber cycle and 4 the information from the table on the last page. a. NaBr(s) b. MgCl2(s)
What is the Born-Haber cycle? How is it used to determine lattice energy and how is Hess’s law used? Please write it all out, illustrate if necessary.
Construct a Born-Haber cycle and calculate the lattice energy of CaC2 (s). Note that this solid contains the diatomic ion C22–.Useful Information:?H°f (CaC2(s)) ?Hsub (Ca (s)) ?Hsub (C (s)) Bond dissociation energy of C2 (g) = +614 kJ/molFirst ionization energy of Ca (g) = +590 kJ/mol Second ionization energy of Ca (g) = +1143 kJ/mol First electron affinity of C2 (g) = –315 kJ/mol Second electronaffinity of C2 (g) = +410 kJ/mol= –60 kJ/mol = +178 kJ/mol = +717 kJ/mol
1)a. Using the Born Haber cycle, determine the enthalpy for lattice formation of MgO. Mg (s), ΔHsub = +148 kJ/mol bond dissociation energy for O2 = +499 kJ/mol 1st ionization energy for Mg = +738 kJ/mol 1st electron affinity for O = –141 kJ/mol 2nd ionization energy for Mg = +1450 kJ/mol 2nd electron affinity for O = +844 kJ/mol MgO(s), enthalpy of formation = –602 kJ/mol 1)b. Calculate the lattice formation energy of MgO using the Madelung constant....
Given the following information, construct a Born-Haber cycle to calculate the lattice energy of CaC2(s): Net energy change for the formation of CaC2(s)=−60kJ/mol Heat of sublimation for Ca(s)=+178kJ/mol Ei1 for Ca(g)=+590kJ/mol Ei2 for Ca(g)=+1145kJ/mol Heat of sublimation for C(s)=+717kJ/mol Bond dissociation energy for C2(g)=+614kJ/mol Eea1 for C2(g)=−315kJ/mol Eea2 for C2(g)=+410kJ/mol Express your answer using four sig figs
1. Construct a Born-Haber cycle showing all steps in the formation of LiF(s). The overall equation is given below Li(s) 1/2F:(g) LiF(s)
1. Construct a Born-Haber cycle showing all steps in the formation of LiF(s). The overall equation is given below Li(s) 1/2F:(g) LiF(s)
a) Determine the lattice energy of thallium(I) iodide using a Born-Haber cycle with “experimental” thermodynamic data. Then calculate it using the Born-Mayer equation. Determine the % deviation of the calculated value from the “experimental” value. b) Explain the result from part (a), giving consideration to HSAB concept.