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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...
Calculate the enthalpies of formation, ΔHfo, of the following
group 1 fluoride compounds from their elements using the Born–Haber
cycle.
NaF RbF Number Number kJ ol kJ mol AHO, kJ/mol Sublimation of Na(s) 108 86 Sublimation of Rb(s) 158 Dissociation of F2(g Ionization energy of Na(g) 496 ionization energy of Rb(g) 403 Electron affinity of F(g) -322 Lattice enthalpy of NaF(s) 926 Lattice enthalpy of RbF(s) 789
Put the following energies in ordered based on the Born Haber cycle below. Sp2+ (8) + 2e- +218) 6 Sr2+ (g) + 2e + 12(e) 7 Sr2+ + 211- (e) fe) + 214 ce 5 Sri+ (g) + 1e + + 12 (8) 4 Sr(e) SriB) + 12 (6) + 12 (5) 3 8 22 Sris)+ 12 (9) 1 Srl (5
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....
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.
Calculate the lattice energy for LiF(s) given the following: sublimation energy for Li(s) = +166 KJ/mol delta Hf for F(g) = +77 KJ/mol first ionization energy of Li(g) = +520 KJ/mol electron affinity of F(g) = -328 KJ/mol enthalpy of formation of LiF(s) = -617 KJ/mol
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
Rutle (TIO2) (Iv) (8) [25] Question 2 2 (a) () Using a Bom-Haber cycle, calculate the lattice enthalpy of LIO2, given the following data AH°(kJ/mol) +161 Sublimation of Li(s) +520 lonization of LI(g) +498 Dissociation of O2(g) -141 Electron affinity of O(g) +865 Electron affinity of O (g) -598 Enthalpy of formation of LIO2 TURN OVE
Consider the following information. The lattice energy of NaCl is ΔH lattice=−788 kJ/mol The enthalpy of sublimation of Na is ΔHsub=107.5 kJ/mol The first ionization energy of Na is IE1=496 kJ/mol. The electron affinity of Cl is ΔHEA=−349 kJ/mol. The bond energy of Cl2 is BE=243 kJ/mol. Determine the enthalpy of formation, ΔHf, for NaCl(s). ΔHf= kJ/mol
Consider the following information. The lattice energy of LiCl is ΔH lattice = −834 kJ/mol. The enthalpy of sublimation of Li is ΔH sub = 159.3 kJ/mol. The first ionization energy of Li is IE 1 = 520 kJ/mol. The electron affinity of Cl is ΔH EA = -349 kJ/mol. The bond energy of Cl2 is BE = 243 kJ/mol. Determine the enthalpy of formation, ΔHf, for LiCl(s).