In question 3, the E.A (electron affinity) value for F, Cl should be in negative, but I have solved accordingly to the data provided in the table.
3. Draw the Bom Haber Cycle and calculate the lattice energies for LiF, MgO, and CaC12...
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....
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...
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
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)
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Using the Born-Haber cycle shown below, calculate the lattice energy for MgCl2 in kJ* mol-1 Mg*g) + 2Cl(g) 2 -349 AH2nd (Mg) - 1451 2xAH (01) --698 Mg*9) 2C119) Mg'ig)2Cl(g) 2x+122 AH. Pot (Mg) - 738 Mg(g) + 2Cl(g) 2xAH LCI - +244 Mgig). Clz (9 Mg(s) : AH (Mg) - 148 Cl2(g) AHTE MgCI) AH. (MgCl) --641 MgCl (s)
2) Write down a Born-Haber cycle for magnesium oxide (Mg0). Using the data provided below, determine the experimental value of the lattice enthalpy Uexp. Now calculate the lattice enthalpy Ucale (unit cell of Mg0 shown below). What do these values tell you about the bonding in Mg0? AHP(Mg0)--602 k]/mol Alto (Mg) = + 148 kJ/mol AH to (02) = +249 kJ/mol bond enthalpy (02)+498 k]/mol 16, (Mg) = +738 kJ/mol IE2 (Mg) +1451 k]/mol EA (O) = +142 kJ/mol EA2(0)...
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
Draw a Born Haber cycle for gallium(I) oxide and calculate the crystal lattice energy for Gallium(I) oxide, given: ΔH°sub (Ga) = 277 kJ/mol E.A.1 (O) = –133 kJ/mol I.E.1(Ga) = 578.84 kJ/mol E.A.2 (O) = 247 kJ/mol I.E.2(Ga) = 1979.4 kJ/mol B.D.E.(O2) = 495 kJ/mol I.E.3(Ga) = 2964.5 kJ/mol ΔHf° (Ga2O) = – 349.8 kJ/mol ANS: -2779 kJ/mol (It was in the Answer Key)
Part A Use the Born-Haber cycle, data from Appendix llBand the following table to calculate the lattice energy of Cao. (AsubH for calcium is 178 kJ/mol: EA 141 kJ/mol, EA 744 kJ/mol: IEC 590 kJ/mol. IE2 1145 kJ/mol. TABLE 9.1 Average Bond Energies Bond Energy Bond Energy Bond Energy Bond kJ mo 1) Bond (kJ mol 1) Bond (kJ mol 237 414 418 218 389 946 193 464 208 H 0 N-0 222 590 565 272 51 200 H-Br 364...