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Using the Born Haber cycle in the previous question, and the following energies, calculate the standard...
Sr2+ (8) + 2e +216) 6 Sr2+ (g) + 2e + 12 (g) 7 Sr2+ (g) + 211- (e) 5 Sr1+ (g) + 1e + 12 (8) 4 Srie) + 12 (8) 3 Sre) + 12 (s) 8 2 Sris) + 12 (5) 1 Sr12(s) Using the Born Haber cycle in the previous question, and the 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...
4) Calculate the lattice enthalpy for calcium fluoride using the Born-Haber cycle method, using the provided table. (Show all your work; 2 points) Enthalpies, AH/(kJ mol) +192 Process Sublimation of Ca(s) Ionization of Ca(g) Dissociation of F2(g) Electron gain by F(g) Formation of CaF (s) +1735 to Ca(ag +157 -328 -1220
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
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.
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 data given below, sketch a Born-Haber cycle for the formation of BaC2(s) and insert the various equations and energy values into the individual steps of your cycle Sublimation energy for Ba(s) +180 kJmol1 Electron affinity for Cl(g)-346 kJmol1 First ionization energy for Ba(g)-+514 kJmol1 Bond dissociation energy for Clh(g) +243 kJmol Enthalpy of formation of BaCl2: Ba(s) + Ch(g) BaCh(s)--610 kJmol Lattice energy. Ba2+(g) + 2Cl.(g) → BaCl2(s)--2075 kJmol-1 Calculate the second ionization energy for Ba+(g) → Ba2+(g)...
3. Draw the Bom Haber Cycle and calculate the lattice energies for LiF, MgO, and CaC12 using the data provided in the table below. This can be done on a separate page if you are working off this template. AH (1/2 B.E.) Electon Affinity Ionization Sublimation AH EA Energy Ionic Compoud F 80 kJ/mol 328 kJ/mol Li 520 kJ/mol 155 kJ/mol LiF -594 kJ/mol 0 249.4 kJ/mol 141 kJ/mol (15) . Mg 738 kJ/mol (19) 148 kJ/mol MgO -601 kJ/mol...
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...
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