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. MgO packs like
NaCl and has a total radii distance of 212 pm. The constant a is
approximately 3.45 Å−1.
1)c. How does the lattice energy for MgO compare to NaCl?
1)a. Using the Born Haber cycle, determine the enthalpy for lattice formation of MgO. Mg (s),...
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...
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 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
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)...
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...
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
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
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...
The enthalpy of formation of MX is ΔHf° = –527 kJ/mol. The enthalpy of sublimation of M is ΔHsub = 139 kJ/mol. The ionization energy of M is IE = 475 kJ/mol. The electron affinity of X is ΔHEA = –309 kJ/mol. (Refer to the hint). The bond energy of X2 is BE = 223 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