Calculate the overall energy change in kilojoules per mole for the formation of CsF(s) from its elements using the following data:
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- Calculate the lattice energy of potassium fluoride, KF, using the BornHaber cycle. Use thermodynamic data from Appendix C to obtain the enthalpy changes for each step. (Note: You will obtain a slightly different answer if you use values given in Chapter 8 for the ionization energy and electron affinity, which are energy values at 0 K rather than the enthalpy changes at 298 K.)arrow_forwardOf the five elements Sn, Si, Sb, O, Te, which has the most endothermic reaction? (E represents an atom.) What name is given to the energy for the reaction? E(g)E+(g)+earrow_forwardGiven the following enthalpy values for Na and Cl, calculate the lattice energy of NaCl using the Born- Haber cycle. for Na = 107.5 kJ/mole for Na = 495.8 kJ/mole for Cl, = 242.6 kJ/mole AHO sublimation AH ionization energy AHO dissociation energy ΔΗΡ electron affinity TOr Cl, = -348.6 kJ/mole AH formation for NaCl(s) = -4l1.2 kJ/molearrow_forward
- 1) Calculate the lattice energy for NaCl(s) using a Born-Haber cycle and the following information: NaCl(s) → Nat(g) + Cl-(g) Na(s) + 1/2 C12(g) → NaCl(s) Na(s) → Na(g) Na(g) → Na+(g) + e- 1/2 C12(g) → Cl(g) Cl(g) + e- → Cl-(g) ? -411.0 kJ/mol +107.3 kJ/mol +495.8 kJ/mol +121.7 kJ/mol -348.6 kJ/molarrow_forwardConsider an ionic compound, MX3, composed of generic metal M and generic gaseous halogen X. The enthalpy of formation of MX3 is Δ?∘f=−925 kJ/mol. The enthalpy of sublimation of M is Δ?sub=175 kJ/mol. The first, second, and third ionization energies of M are IE1=579 kJ/mol, IE2=1677 kJ/mol, and IE3=2479 kJ/mol. The electron affinity of X is Δ?EA=−369 kJ/mol. (Refer to the hint). The bond energy of X2 is BE=179 kJ/mol. Determine the lattice energy of MX3.arrow_forwardUse the data provided below to calculate the lattice energy of RbCl. Is this value greater or less than thelattice energy of NaCl? Explain.Electron affinity of Cl = –349 kJ/mol1st ionization energy of Rb = 403 kJ/molBond energy of Cl2 = 242 kJ/molSublimation energy of Rb = 86.5 kJ/molΔHf [RbCl (s)] = –430.5 kJ/molarrow_forward
- Consider the following information. • The lattice energy of RbCl is AHjattice = -689 kJ/mol. t • The enthalpy of sublimation of Rb is AHsub = 80.9 kJ/mol. • The first ionization energy of Rb is IE, 403 kJ/mol. • The electron affinity of Cl is AHEA = -349 kJ/mol. • The bond energy of Cl, is BE = 243 kJ/mol. Determine the enthalpy of formation, AHf, for RbCl(s). AHf = kJ/molarrow_forwardConsider an ionic compound, MX, composed of generic metal M and generic, gaseous halogen X. • The enthalpy of formation of MX is AH; -517 kJ/mol. • The enthalpy of sublimation of M is AH sub = 141 kJ/mol. • The ionization energy of M is IE = 449 kJ/mol. • The electron affinity of X is AHEA = -323 kJ/mol. (Refer to the hint). • The bond energy of X, is BE = 217 kJ/mol. Determine the lattice energy of MX. AHjattice kJ/molarrow_forwardWhat is the chemical formula for the compound formed between manganese(IV) and chlorine? chemical formula: What is the chemical formula for the compound formed between manganese(IV) and sulfur? chemical formula:arrow_forward
- The lattice energy of potassium iodide is the energy required for the following reaction. KI(s) → K+(g) + I−(g) ΔHrxn = ΔHlattice Use the Born-Haber cycle to calculate ΔHlattice for KI(s) from the information given below. Equation 1: 2 K(s) + I2(g) → 2 KI(s) ΔH1 = −655 kJ/mol Equation 2: K(s) → K(g) ΔH2 = 89 kJ/mol Equation 3: I2(g) → 2 I(g) ΔH3 = 214 kJ/mol Equation 4: K(g) → K+(g) + e− ΔH4 = 419 kJ/mol Equation 5: I(g) + e− → I−(g) ΔH5 = −294 kJ/molarrow_forwardConsider the following information. • The lattice energy of NaCl is AHjattice = -788 kJ/mol. • The enthalpy of sublimation of Na is AHub = 107.5 kJ/mol. • The first ionization energy of Na is IE1 = 496 kJ/mol. • The electron affinity of Cl is AHEA = -349 kJ/mol. • The bond energy of Cl, is BE = 243 kJ/mol. Determine the enthalpy of formation, AHf, for NaCl(s). AH¡ = kJ/mol * TOOLS x10arrow_forwardConsider an ionic compound, MXMX, composed of generic metal MM and generic, gaseous halogen XX. The enthalpy of formation of MXMX is Δ?∘f=−553ΔHf∘=−553 kJ/mol. The enthalpy of sublimation of MM is Δ?sub=129ΔHsub=129 kJ/mol. The ionization energy of MM is IE=491IE=491 kJ/mol. The electron affinity of XX is Δ?EA=−325ΔHEA=−325 kJ/mol. (Refer to the hint). The bond energy of X2X2 is BE=219BE=219 kJ/mol. Determine the lattice energy of MXMX. Δ?lattice=ΔHlattice= kJ/molarrow_forward
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