Given the following information, calculate the lattice energy of CaF2 The enthalpy of formation of CaF2...
Knowing the enthalpy of formation of calcium fluoride is -1228 KJ / mol, the enthalpy of the sublimation of calcium is 168kj/mole, the bond enthalpy of fluorine is 155kj/mole, the electron affinity of fluorine is -328 kj/mole, the first ionization enthalpy of calcium is 590kj/mole and the second ionization enthaply is 1145kj/mole, calculate the lattice enthalpy of calcium fluoride.
Consider the following information. The enthalpy of formation of CaO is ΔHf°=-634.9 kJ/mol. The enthalpy of sublimation of Ca is ΔHsab = 177.8 kJ/mol. The first and second ionization energies of Ca are IE1 = 590 kJ/mol and IE2 = 1145 kJ/mol. The first electron affinity of O is ΔHAI=-142 kJ/mol. The bond energy of O2 is BE = 498 kJ/mol. The lattice energy of CaO is ΔHatice = -3414 kJ/mol. Determine the second electron affinity of O.
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
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
Structure with an (8,4) coordination unit cell (0) Given the b. Calcium fluorite (CaF2) has a fluorite structure with an (8,4) coordina Given the following data, use Born-Haber cycle to calculate the lattice enthalpy of CaF2 AH KJ/mol +178 +1228 Sublimation of Ca(s) Decomposition of CaF2(s) Dissociation of F2(g) lonisation of Ca(s) lonisation of Ca (8) Electron gain of F(b) +79 +590 +1145 -328 Given the following data d* = 0.345x10-11m, K=1.20 MJÅ. mol-, e = 1.602x10-19 C, N =...
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
2. Use the following data to calculate the lattice energy (U) of NaCl(s) from sodium me chlorine: Enthalpy of formation (4H) for NaCl(s) - -411 kJ/mol Enthalpy of sublimation (4Hub) of Na 107.3 kJ/mol The first ionization energy of Na (E,)-495.8 kJ/mol The bond dissociation energy (D) of Clh- 243 kJ/mol The electron affinity of Cl (Eea)- 348.6 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).
Write down the chemical equation for the 2nd ionization (IE2) energy for calcium. Follow the instructions below: Calculate IE2 for calcium using the data listed below. For each data item, write down the chemical equation associated with the process (i.e., that defines the process) - making sure to indicate all phases. In order to show your work, demonstrate, using Hess' law, how you came up with the Born-Haber cycle that lead to the net chemical equation for the IE2 of...