9. Given the information below, determine the lattice energy of MgCl2.Mg(s) - Mg(g)DH°f = +147.1 kJ/mol½ Cl2(g) – CI(g)DH2°f =+122 kJ/molMg(g) – Mg*(g) DH3°t = +738 kJ/molMg*(g)Mg* (g)DH4°F = +1450kJ/molCl(g) - Cl (g) DH5°f = -349 kJ/molMg(s) + Cl2(g) – MgCl2(s) DH6°r = -641 kJ/mol

Given: Enthalpy of vaporization of Mg (ΔHvap) = +147.1 kJ/mol First ionization energy of Mg (IE1) =…

Given the information below, determine the lattice energy of MgCl2. Mg(s) → Mg(g) +122 kJ/mol DH°f = +147.1 kJ/mol ½ Cl2(g) → CI(g) DH2°f = Mg(g) - Mg (g) DH3°t = +738 kJ/mol kJ/mol Mg (g) Mg (g) DH4°f = +1450 Cl(g) - CI (g) DHs°f = -349 kJ/mol Mg(s) + Cl2(g) - MgCl2(s) DH6°r = -641 kJ/mol

Given the information below, determine the lattice energy of MgCl2. Mg(s) → Mg(g) +122 kJ/mol DH°f = +147.1 kJ/mol ½ Cl2(g) → CI(g) DH2°f = Mg(g) - Mg (g) DH3°t = +738 kJ/mol kJ/mol Mg (g) Mg (g) DH4°f = +1450 Cl(g) - CI (g) DHs°f = -349 kJ/mol Mg(s) + Cl2(g) - MgCl2(s) DH6°r = -641 kJ/mol

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 128AE: For each of the following, write an equation that corresponds to the energy given. a. lattice energy...

See similar textbooks

Similar questions

A commercial process for preparing ethanol (ethyl alcohol), C2H5OH, consists of passing ethylene gas. C2H4, and steam over an acid catalyst (to speed up the reaction). The gas-phase reaction is Use bond enthalpies (Table 9.5) to estimate the enthalpy change for this reaction when 37.0 g of ethyl alcohol is produced.
hat is the enthalpy change for a process? Is enthalpy a state function? In what experimental apparatus are enthalpy changes measured?
What main factors control the magnitude of lattice energies? Give a specific example of a compound that should have a high lattice energy, and explain why its lattice energy is high.
Arrange the following series of compounds in order of increasing lattice energies. (a) NaBr, NaCl, KBr (b) MgO, CaO, CaCl2 (c) LiF, BeF2, BeO
Write all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?
Use a Born-Haber cycle (Sec. 5-13) to calculate the lattice energy of MgF2 using these thermodynamic data. Compare this lattice energy with that of SrF2, −2496 kJ/mol. Explain the difference in the values in structural terms.
Calculate the enthalpy of reaction for HCN(g)H(g)+C(g)+N(g) from enthalpies of formation (see Appendix C). Given that the CH bond enthalpy is 411 kJ/mol, obtain a value for the CN bond enthalpy. Compare your result with the value given in Table 9.5.
The lattice energy of KF is 794 kJ/mol, and the interionic distance is 269 pm. The Na—F distance in NaF, which has the same structure as KF, is 231 pm. Which of the following values is the closest approximation of the lattice energy of NaF: 682 kJ/mol, 794 kJ/mol, 924 kJ/mol, 1588 kJ/mol, or 3175 kJ/mol? Explain your answer.
Estimate H for the following reactions using bond energies given in Table 8.5. 3CH2=CH2(g) + 3H2(g) 3CH2CH3(g) The enthalpies of formation for C6H6(g) and C6H12 (g) are 82.9 and 90.3 kJ/mol. respectively. Calculate H for the two reactions using standard enthalpies of formation from Appendix 4. Account for any differences between the results obtained from the two methods.
Bond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?
hat is meant by the term driving forces? Why are mailer spread and energy spread considered to be driving forces?
Compare your answers from parts a and b of Exercise 69 of Chapter 3 with H values calculated for each reaction using standard enthalpies of formation in Appendix 4. Do enthalpy changes calculated from bond energies give a reasonable estimate of the actual values?