Calculate the lattice energy of RbH (s) using the following thermodynamic data (all data is in kJ/mol). Note that the data given ha been perturbed, so looking up the answer is probably not a good idea. Rb (s) Rb (g) H - H (g) Bond energy = 416 kJ/mol H (g) Electron affinity = -93 kJ/mol RbH (s) AH°f = -72 kJ/mol kJ/mol ΔΗsublimation = 61 kJ/mol Ionization energy = 383 kJ/mol

Calculate the lattice energy of RbH (s) using the following thermodynamic data (all data is in kJ/mol). Note that the data given ha been perturbed, so looking up the answer is probably not a good idea. Rb (s) Rb (g) H - H (g) Bond energy = 416 kJ/mol H (g) Electron affinity = -93 kJ/mol RbH (s) AH°f = -72 kJ/mol kJ/mol ΔΗsublimation = 61 kJ/mol Ionization energy = 383 kJ/mol

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

Use the Born-Haber cycle to calculate the lattice energy of KF. [The heat of sublimation of K is 91.6 kJ·mol−1 and ΔfH(KF) = −567.3 kJ·mol−1. Bond enthalpy for F2 is 158.8 kJ·mol−1. Other data may be found in the Ionization Energies Table and the Electron Affinities Table.]
The lattice energy of NaCl is 769 kJ/mole. Which of the following is a correct statement about NaCl? When one mole each of gaseous Nat and CI- ions form solid NaCl, 769 kJ of heat is consumed. It requires 769 kJ to separate one mole of solid NaCl into one mole of each gaseous Na* and CI- ions. It requires 769 kJ to separate one mole of solid NaCl into gaseous one mole of Na* and two moles of CI- ions.
2. Use the data provided below to calculate the lattice energy of calcium chloride. Electron affinity of Cl = -348.7 kJ/mol 1st ionization energy of Ca = 590.0 kJ/mol 2nd ionization energy of Ca = 1145.0 kJ/mol Bond energy of Cl2 = 242.6 kJ/mol Sublimation energy of Ca = 178.0 kJ/mol AH¡ [CaCl. (s)] =-795.0 kJ/mol
Consider the reaction below. Mg2+ (g) + 2 Br (g) →→ MgBr₂ (s) - When this type of reaction occurs, energy is emitted The energy involved in producing MgBr₂ (s) in this way is known as the lattice energy of MgBr₂.
KBr has a lattice energy -671 kJ/mol. Consider a hypothetical salt XY. X3+ has the same radius of K+ and Y3− has the same radius as Br−. Estimate the lattice energy of XYXY.
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): Rbl, CaO, SrO, NaCl 1b)Rank the following elements in order of increasing metallic character (from least metallic to most metallic): Ca, S, Rb, Ar, Se 1c) by using the attached table of bond enthalpies, predict ?rH of the following reaction in kJ/mol H2N-NH2 + O2 ---> N2+ 2H2O
Use the data given below to construct a Born-Haber cycle to determine the lattice energy of CaO. A H°(kJ) Ca(s) → Ca(g) 193 Ca(g) → Cat (g) + e 590 Cat (g) → Ca2+(g) + e 1010 20(g) → O2(g) -498 O(g) + e O(g) -141 O(g) + e → O2(g) 878 Ca(s) + O2(g) → CaO(s) -> -635 O-2667 kJ O-3414 kJ O +1397 kJ +3028 kJ O-2144 kJ
The enthalpy change for the following reaction is 81.7 kJ. I2(g) + Br2(g) -- > 2IBr(g) Estimate the Br-Br bond energy in Br2(g), using tabulated bond energies (linked above) for the remaining bonds. Br-Br bond energy = ?
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.
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 KCI(s) using the following thermodynamic data (all data is in kJ/mol) K(s) AHsublimation = 69 kJ/mol K(g) Ionization energy = 399 kJ/mol CI-CI(g) Bond energy = 223 kJ/mol Cl(g) Electron affinity = -369 kJ/mol KCI(s) AH°r= -457 kJ/mol kJ/mol
16) ( , Using the thermochemical data below calculate the lattice energy for the formation of Na₂O. Na(s) → Na(g) 107.3 kJ/mol Na(g) → Na*(g) + 1 e 495.9 kJ/mol 2 Na(s) + O₂(g) → Na₂O(s) -418 kJ/mol 1/2 O₂(g) → O(g) 249.1 kJ/mol O(g) + 1 e→O(g) -141 kJ/mol -1484.5 kJ/mol O(g) + 1 e0²(g) s) If 115 or pressu