Bond Dissociation Energy
Suppose there is an element X which occurs naturally as
X2(g).
X2(g) + 2O2(g) →
X2O4(g)
X2O4 has a structure
ΔHof of O(g) is 249
kJ/mol
ΔHof of X(g) is 478.5
kJ/mol
ΔHof of
X2O4(g) is 15 kJ/mol
The X-X single bond energy is 106 kJ/mol
Use the above data to estimate the average bond energy in
X2O4.
Give your answer to the nearest 1 kJ/mol. |
Bond Dissociation Energy Suppose there is an element X which occurs naturally as X2(g). X2(g) +...
Bond Dissociation Energy Suppose there is an element X which occurs naturally as X2(g). X2(9) + 202(g) → X204(9) --- X204 has a structure AH°F of O(g) is 249 kJ/mol AH°F of X(9) is 450.5 kJ/mol AH°F of X204(9) is 17 kJ/mol The X-X single bond energy is 104 kJ/mol Use the above data to estimate the average X----O bond energy in X204. Give your answer to the nearest 1 kJ/mol.
Calculate AH® for the reaction using the given bond dissociation energies. CH, (g) +202(9) — CO2(g) + 2 H2O(g) Bond AH° (kJ/mol) 0-0 | 142 H-0 459 C-H 411 C=0 799 O=0 498 C-0 358 This reaction is kJ/mol AH° = O endothermic. O exothermic.
QUESTION 23 Using the provided bond dissociation energies, determine the change in enthalpy (AH) in kilojoules for the following reaction. (Note - the reaction is shown two different ways to help you properly interpret it.) Y2+ 2 X2 - 2 YX2 Y-Y+ 2 X-X - 2 X-Y-X -Y X X X Y Bond Dissociation energy (kJ/mol) 449 272 174
1. Calculate the bond energy of the CI-F bond using the following data: Cl2(g) + F2(g) → 2CIF(g) AH = -108 kJ Bond enthalpies (kJ/mol): CI-CI (239); F-F (159) CI-C1 = 239 F.F : 159 1 2. Find the experimental Lattice energy of aluminum oxide using a Born-Haber cycle using the following information: AH® (aluminum oxide) = -1676 kJ/mol IE, (aluminum) = 577.6 kJ/mol IE, (aluminum) =1816.7 kJ/mol IE(aluminum) = 2744.8 kJ/mol AH® (aluminum atom, g) = 329.7 kJ/mol AHⓇEAI...
Use bond energies, values of electron affinities, and the ionization energy of hydrogen (1312 kJ/mol) to estimate AH for the following reaction Bond Energies Electron Affinities H-F (565 kJ/mol) F() (-328 kJ/mol) H-CI (427 kJ/mol) C1(9) (-349 kJ/mol) -(295 kJ/mol) 1(9) (-295 kJ/mol) 0_H(467 kJ mol) OH(g) (-180. kJ/mol) H2O(g) + H+ (g) + OH (9) AHL b HCI(g) + H+ (g) + CI" (9) AH = kJ
5. (15 points) Estimate the C-C bond energy from the provided information below: CH.(g) + H2(g) → CH.(g) AH®rxn-- 137 kJ Bond Bond Energy (kJ/mol) C-C611 C-H 414 C=C 837 H-H 436
Calculate the AGº for X, in k], from the data given below at 325 K: 2x(g) → X2(9) X(g) X2(9) So (J/mol-K) AH° (kJ/mol) 58. 1 5 4.1 97.6 112.0
The following equation represents the decomposition of a generic diatomic element in its standard state. X,(g) + X(g Assume that the standard molar Gibbs energy of formation of X(9) is 4.75 kJ molat 2000. K and-62.62 kJ. mol-'at 3000. K. Determine the value of K (the thermodynamic equilibrium constant) at each temperature. At 2000. K, we were given: AG = 4.75 kJ. mol-! What is k at that temperature? Number Kat 2000. K- At 3000. K, we were given: AG=-62.62...
The equation represents the decomposition of a generic diatomic element in its standard state. X,(8) - X(8) Assume that the standard molar Gibbs energy of formation of X(g) is 5.02 kJ mol-'at 2000. K and 64.75 kJ mol at 3000. K. Determine the value of K (the thermodynamic equilibrium constant) at each temperature. K at 2000. K = K at 3000. K Assuming that AHin is independent of temperature, determine the value of AH; from this data. AHin = KJ-mol...
The equation represents the decomposition of a generic diatomic element in its standard state. X,(8) - X(8) Assume that the standard molar Gibbs energy of formation of X(g) is 5.02 kJ mol-'at 2000. K and 64.75 kJ mol at 3000. K. Determine the value of K (the thermodynamic equilibrium constant) at each temperature. K at 2000. K = K at 3000. K Assuming that AHin is independent of temperature, determine the value of AH; from this data. AHin = KJ-mol...