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 is added to water. To solve this problem use ΔhydH(K+) = -326.00 kJ mol-1 and ΔhydH(Cl-) = -348.00 kJ mol-1.
Part I. Use a Born-Haber cycle to calculate the lattice energy of KCl from the following...
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
Born-Fajans-Haber Cycle Suppose a chemist discovers a new metallic element and names it "Xtrinsium" (Xt) Xt exhibits chemical behaviour similar to an alkaline earth Xt(s) + Cl2(g) → XtCl2(s) Lattice energy for XtCl2 First Ionization energy of Xt Second Ionization energy of Xt Electron affinity of Cl Bond energy of Cl2 Enthalpy of sublimation (atomization) of Xt 2260. kJ/mol 430. kJ/mol 731 kJ/mol -348.7 kJ/mol 239 kJ/mol 170. kJ/mol Use the above data to calculate ΔHof for Xtrinsium chloride.
Using the Born Haber cycle in the previous question, and the following energies, calculate the standard energy of formation for Srl2 Enthalpy of sublimation of Sr(s) = 164 kJ/mol 1st ionization energy of Sr(g) = 549 kJ/mol 2nd ionization energy of Sr(g) - 1064 kJ/mol Enthalpy of sublimation of 12(s) = 62 kJ/mol Bond dissociation energy of 12(g) - 153 kJ/mol 1st electron affinity of l(g) = -295 kJ/mol Lattice energy of Srlz(s) = -1960 kJ/mol *Note: Do not include...
Consider the following information. • The lattice energy of KCl is AHlattice = -701 kJ/mol. • The enthalpy of sublimation of K is AHsub = 89.0 kJ/mol. • The first ionization energy of K is IE1 = 419 kJ/mol. • The electron affinity of Cl is AHEA = -349 kJ/mol. • The bond energy of Cl, is BE = 243 kJ/mol. Determine the enthalpy of formation, AHf, for KCl(s). AHư= kJ/mol
1. showing the complete Born-Haber for the lattice energy of KCl(s).
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.
Question 4 4 pts Use the Born-Haber Cycle to calculate the lattice energy for the formation of X2Y. Input your answer in units of kJ/mole with the correct sign. Process Enthalpy (kJ/mol). X(s)--> X(g) 115 X(g) -->X*(8) + le 499 Y2 (8) --> 2Y (8) 264 -295 Y (8) + 1e.-->Y (8) Y (8) + 1e' --> Y2 () 115 2X(s) +% Y2 (8)--> X2Y(s) -549
Using the Born-Haber cycle shown below, calculate the lattice energy for MgCl2 in kJ* mol-1 Mg**g) + 2Cl(g) 2 x-349 AH2nd le(Mg) - 1451 2xAH (01) --698 My*(g) 2013) Mg (g) + 2Cl(g) AHORE (Mg) - 738 Mg(g) + 2Cl(g) 2 x 122 2xAH CIT- +244 Mg(g) + Cl2(g) AHTE (MgCl2) Mg(s) + Clą(9) AHM9) - 148 AH, (MgCl2) --641 MgCl (s)
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...
Physical Chemistry: Use a Born-Haber cycle to find an experimentally based value for the lattice enthalpy of sodium bromide (NaBr(s)). The lattice enthalpy corresponds to the enthalpy change for the process NaBr(s) rightarrow Na^+(g) + Br^-(g) Use the following information in doing this problem. delta H degree_f(Na(g)) = 107.32 kJ/mol delta H degree_IE1(Na(g)) = 495.8 kJ/mol delta H degree_f(Br(g)) = 111.88 kJ/mol delta H degree_EA(Br(g)) = -324.6 kJ/mol delta H degree_f(NaBr(s)) = -361.06 kJ/mol The ionization enthalpy (IE_1) and electron...