Calculate the lattice energy of AgCl(s) using the following thermodynamic data (all data is in kJ/mol). Note that the data given has been perturbed, so looking up the answer is probably not a good idea. Ag(s) AHsublimation = 265 kJ/mol Ag(g) Ionization energy = 711 kJ/mol Cl-CI(g) Bond energy = 223 kJ/mol CI(g) Electron affinity = -369 kJ/mol AgCl(s) AH°r=-147 kJ/mol kJ/mol Do you expect this value to be larger or smaller than the lattice energy of AgBr(s)?

Calculate the lattice energy of AgCl(s) using the following thermodynamic data (all data is in kJ/mol). Note that the data given has been perturbed, so looking up the answer is probably not a good idea. Ag(s) AHsublimation = 265 kJ/mol Ag(g) Ionization energy = 711 kJ/mol Cl-CI(g) Bond energy = 223 kJ/mol CI(g) Electron affinity = -369 kJ/mol AgCl(s) AH°r=-147 kJ/mol kJ/mol Do you expect this value to be larger or smaller than the lattice energy of AgBr(s)?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

KBr has a lattice energy -671 kJ/mol . Consider a hypothetical salt XY. X2+ has the same radius of K+ and Y2− has the same radius as Br−. Estimate the lattice energy of XY.
1a)Rank the following ionic compounds in order of lattice energy, from the least exothermic (least negative lattice enthalpy) to the most exothermic (most negative lattice enthalpy): KCI, SrO, RbBr, CaO 1b)Rank the following elements in order of decreasing metallic character (from most metallic to least metallic): S, CI, K, Cs, Se 1c) by using the table of bond enthalpies, predict ?rH of the following reaction in kJ/mol H2C=CH2 + Cl2 ---> Cl-CH2-CH2-Cl
1. Given the following information, calculate the lattice energy for LiI(s). Show all work and construct a diagram(cycle) that shows each step in the process of forming LiI(s) from gaseous ions.
Calculate the average A-B bond energy in AB3(g). AH for AB3(g)=-75.9 kJ/mol, AH, for A(g) = 288.9 kJ/mol, AH, for B(g) = 134.9 kJ/mol, AH for A2(g) = 0 kJ/mol, AH for B2(g)=0 kJ/mol. Enter a number in kJ/mol to 1 decimal place.
9. Use the following data to calculate the lattice energy of Cao. The enthalpy of formation of Cao is –636 kj/mol. The enthalpy of sublimation of Ca is +192 kj/mol, the first ionization energy of Ca is +590 kj/mol, and the second ionization energy of Ca is +1145 kj/mol. The enthalpy of dissociation of 02 is +494 kj/mol of 02 molecules, the first electron affinity of O is -141 kj/mol of 0 atoms, and the second electron affinity of 0 is +845 kj/mol of 0¯ ions.
Calculate the lattice energy of RbH (s) using the following thermodynamic data (all data is in kJ/mol). Note that the data given has been perturbed, so looking up the answer is probably not a good idea. AHsublimation 61 kJ/mol Ionization energy = 383 kJ/mol Rb (s) Rb (g) H - H (g) Bond energy = 416 kJ/mol H (g) Electron affinity = -93 kJ/mol RbH (s) AHOf = -72 kJ/mol kJ/mol
PCl3(g) + Cl2 (g) --><-- PCl5(g) A. Use a bond energy to find deltaHo for the reaction. Cl - Cl, 339 kJ/mole; P - Cl, 289 kJ/mole. B. Calculate the value of deltaSo for the reaction. So(PCl5) = 364.2 J/mol * K; So(PCl3) = 311.6 J/mol * K; So(Cl2) = 165.2 J/mol * K.
Calculate the standard energy of formation of CI0 from the following bond energies. f Cl2: 242.7 kJ/mol O2: 498.7 kJ/mol C10: 206 kJ/mol kJ/mol
Given the following information, use the Kapustinskii equation (shown below and included in the additional information sheet I encouraged you to download and have available) to calculate the lattice energy for Cr2S3 in kJ/mol. Ionic radii: Cr3+ (62 pm), S2− (184 pm) d* = 34.5 pm Κ = 1.21 × 105 kJ pm/mol
For Na (s) + 1/2 Cl2 (g) ---> NaCl (s) ΔH = -410 kJ, ΔH is the ionization energy endothermic energy heat of formation bond energy lattice energy
Calculate the lattice energy of TIF (s) using the following thermodynamic data (all data is in kJ/mol). Note that the data given has been perturbed, so looking up the answer is probably not a good idea. TI (S) TI (g) F - F (g) F (g) TIF (s) AHsublimation = 161 kJ/mol Ionization energy = 569 kJ/mol Bond energy = 138 kJ/mol Electron affinity = -348 kJ/mol AH°f = -345 kJ/mol kJ/mol
Which of the following ionic compounds has the largest lattice formation enthalpy (lattice energy); that is, which compound is most favorable to a stable lattice? A) Csl B) Lil C) LiF D) CsF E) MgO