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What is the Born-Haber cycle? How is it used to determine lattice energy and how is...
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.
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.
7) For the ionic solid AlzOs a) Determine its lattice energy using the appropriate Born-Haber cycle and the following values. All values in kJ/mol: IEi (A)-557.5:IE2 (A)-1817; IEs (A)-2745; IE(Al) 11580 E (0)-1314; IE2 (0) 3388; IEs (O)-5300 ΔΗ"a (O) =-141 (first electron affinity) ; ΔΗ'EA AH (Al) 330; AHa (O)-249;AH (Al Os)--1669.8 (o)- 798 (second electron affinity) b) Al:O, crystallizes in a corundum structure. How does the above lattice energy compare to the lattice energy determined by an electrostatic...
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) →...
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)
Use the Born-Haber Cycle and information given below to determine the lattice energy of LiF. Li(s) → Li(g) +159.3 kJ Li(g) → Li+(g) + e– +500.9 kJ F2(g) → 2 F(g) +158.8 kJ F(g) + e– → F–(g) –332.6 kJ Li+(g) + F–(g) → LiF(s) ? --------------------------------------------------- Li(s) + ½ F2(g) → LiF(s) – 616.0 kJ Group of answer choices +209.0 kJ –1023 kJ +1023 kJ –209.0 kJ –1102.4 kJ
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....
Use the Born Haber cycle (see equations and enthalpy values below) to determine the lattice energy for BeI2 (s) (∆H LE (BeI2 (s))= ?) Show your work. Box your final answer. A. Be(g)→Be1+ (g) + 1 e–∆H = + 899.5kJ B. Be1+ (g) →Be2+ (g) + 1 e–∆H = +1757 kJ C. Be(s)→Be(g)∆H= +302kJ D. I2(s)→I2(g)∆H= + 62.4kJ E. I(g) + e–→I–(g)∆H= –295kJ F. I2(g)→2I(g)∆H= + 151 kJ G. Be(s) + I2(s) →BeI2(s)∆H= –208 kJ
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...
2. Find the experimental Lattice energy of aluminum oxide using a Born-Haber cycle using the following information: AH (aluminum oxide) = -1676 kJ/mol IE, (aluminum) = 577.6 kJ/mol IE, (aluminum) =1816.7 kJ/mol IE, (aluminum) = 2744.8 kJ/mol AH® (aluminum atom, g) = 329.7 kJ/mol AHⓇEAI (oxygen) = -200.4 kJ/mol AHⓇEAT (oxygen) = 780.0 kJ/mol AH® (oxygen atom, g) = 249.2 kJ/mol Write each of the appropriate balanced chemical equations (with physical state) and assign the appropriate enthalpy to each. Be...