determine the enthalpy of formation for KBr, Use this data Hsub (K)= 79 kJ/mol; IE (K) = 418.8kJ/mol; Hvap (Br2) = 29.8 kJ/mol; Br2 bond energy = 190.2, IE (Na) = 496kJ/mol; EA (Br2) =-324.7 kJ/mol.
determine the enthalpy of formation for KBr, Use this data Hsub (K)= 79 kJ/mol; IE (K)...
The enthalpy of formation of MX is ΔHf° = –527 kJ/mol. The enthalpy of sublimation of M is ΔHsub = 139 kJ/mol. The ionization energy of M is IE = 475 kJ/mol. The electron affinity of X is ΔHEA = –309 kJ/mol. (Refer to the hint). The bond energy of X2 is BE = 223 kJ/mol.
Review Problem 8.065 Construct an enthalpy diagram with the following data to calculate the electron affinity of bromine. The standard heat of formation of NaBr is -360.0 kJ molº?. The energy needed to vaporize one mole of Br2(l) to give Br2(g) is 31 kJ mol-1. Energy needed to vaporize one mole of Na(s) is 107.8 kJ. The first ionization energy of Na is 495.4 kJ mol-1. The bond energy of Br2 is 192 k) per mole of Br- Br bonds....
Consider the following information. The lattice energy of LiCl is ΔH lattice = −834 kJ/mol. The enthalpy of sublimation of Li is ΔH sub = 159.3 kJ/mol. The first ionization energy of Li is IE 1 = 520 kJ/mol. The electron affinity of Cl is ΔH EA = -349 kJ/mol. The bond energy of Cl2 is BE = 243 kJ/mol. Determine the enthalpy of formation, ΔHf, for LiCl(s).
it's okay just solve the a and b then
(a) Calculate the enthalpy of formation of KF based on the following data. 0 Compound ΔΗ' 1st IE 2nd IE ΔΗ 1st EA 2nd EA ΔΗ. lattice (K,g) (K) (K) (F,g) (F) (F) (KF) f - 105 567 (all values are in kJ/mol) (b) Knowing 1(K2+)-95pm, r(F-)=116pm, estimate the lattice energy of the hypothetical compound KF2 (rutile structure, A=2.408) (c) Calculate the enthalpy of formation of KF2. What factor prevents the...
Consider the following information. The lattice energy of NaCl is ΔH lattice=−788 kJ/mol The enthalpy of sublimation of Na is ΔHsub=107.5 kJ/mol The first ionization energy of Na is IE1=496 kJ/mol. The electron affinity of Cl is ΔHEA=−349 kJ/mol. The bond energy of Cl2 is BE=243 kJ/mol. Determine the enthalpy of formation, ΔHf, for NaCl(s). ΔHf= kJ/mol
The standard enthalpy of formation of NaF(s) is -573.6 kJ/mol, and the standard enthalpy of formation of NaF(aq, 1m) is -572.8 kJ/mol. Determine the standard enthalpy of solution of NaF.-0.8 kJ/mol-572.0 kJ/mol+0.8 kJ/mol-1146.4 kJ/mol+1146.4 kJ/mol
4. The standard enthalpy of formation of NH3 (g) is -46.11 kJ mol-' at 298 K. Given the heat capacity data below and the data in Problem 2, calculate the standard enthalpy of formation at 1200 K Cp.m (H2 (9))/ J mol K-1 = 29.1 - (0.84 x 10- K-)T Cpm (N2 (g))/ J mol K-1 = 26.98 +(5.9 x 10-'K-!)T
Using the standard enthalpy of formation data, show how the standard enthalpy of formation of HF(g) can be used to determine the bond energy. (Enter unrounded values.) (a) bond energy calculated from standard enthalpy of formation kJ/mol (b) average bond enthalpy from the bond enthalpy table k]/mol Average Bond Enthalpies bondAH bond (kJ/mol) bond AHbond (kJ/mol) bond AH bond (kJ/mol) bond AH bond (kJ/mol) O-H 0-0 467 146 495 185 203 156 364 522 335 544 413 347 614 839...
6. Calculate the lattice enthalpy of RbCI (s) given the following thermodynamic data where IE and EA are ionization energy and electron affinity respectively. Show all chemical equations, states, and calculations for credit. (8 points) + 121.3 kJ/mol Cl 349.0 kJ/mol C EA [CI]- AH [Rb(g)]80.9 kJ/mol Rb IE [Rb]- +403.0 kJ/mol Rb - 435.4 kJ/mol RbCl AH [RbCl(s)]-
The standard enthalpy of combustion of cyclopropane is -2091 kJ/mol at 298 K. The enthalpy of formation of CO_2 (g) and H_2 O (I) are -393 kJ/mol and -286 kJ/mol, respectively. Calculate the enthalpy of formation of cyclopropane Given that the enthalpy of formation of propene is 20.42 kJ/mol, please calculate the enthalpy of isomerization of cyclopropane to propene.