Using the thermodynamic quantities shown below: construct a
Born-Haber cycle for the following reaction: Li(s) + 1/2
F2(g)
LiF(s); calculate the lattice energy of LiF.
Vaporization of Li(s): +159
F2 bond enthalpy: +155
Li ionization energy: +520
F- electron affinity: +328
LiF(s) heat of formation: -616
Using the thermodynamic quantities shown below: construct a Born-Haber cycle for the following reaction: Li(s) +...
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 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
1. Construct a Born-Haber cycle showing all steps in the formation of LiF(s). The overall equation is given below Li(s) 1/2F:(g) LiF(s)
1. Construct a Born-Haber cycle showing all steps in the formation of LiF(s). The overall equation is given below Li(s) 1/2F:(g) LiF(s)
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
Discuss the relationship of calculating lattice energy and the Born-Haber cycle. Here are some suggestions of topics on which to elaborate upon in your explanations: Provide an explanation of the Born-Haber cycle. Explain the difference between ionization energy and electron affinity. Explain how the enthaply of formation is related to the Born-Haber cycle.
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)...
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
OADVANCED MATERIAL Interpreting a Born-Haber cycle This thermodynamic cycle describes the formation of an ionic compound M X2 from a metal element M and nonmetal element X in their standard states. Use it to answer the questions in the table below. 2+ 1100 1000 900 2- 800--- 700 600 M (8)+2X) 500. enthalpy 400 (kJ/mol) 300. M (g) + X, (g) 200 ▼ | 700,- 600 M (g) + 2x (g 500 enthalpy 400. 300. м (е) + x, (g)...
7. Use the Born Haber cycle and the given information to determine the net energy change (in kJ/mol) that takes place in the formation of KF(s) from the elements: Ks) + F2@KFS) Heat of sublimation of K = 89.2 kJ/mol Bond dissociation energy for F2 = 158 kJ/mol Lattice Energy of KF = 821 kJ/mol Eca for F = -328 kJ/mol E; for K = 418.8 kJ/mol
Use the Born-Haber Cycle and information given below to determine the lattice energy of LiF. Li(s) → Li(g) +159.3 kJ Li(g) → Li+(g) + e– +500.9 kJ F2(g) → 2 F(g) +158.8 kJ F(g) + e– → F–(g) –332.6 kJ Li+(g) + F–(g) → LiF(s) ? --------------------------------------------------- Li(s) + ½ F2(g) → LiF(s) – 616.0 kJ Group of answer choices +209.0 kJ –1023 kJ +1023 kJ –209.0 kJ –1102.4 kJ