Born-4-Iaber cycles, such as those shown in Figures 6.7 and 6.8,are called cycles because they form dosed loops. If any five of the six energy changes ¡n the cycle are known, the value of the sixth can be calculated. Use the following five values to calculate the lattice energy in kilojoules per mole for sodium hydride, NaH(s): E ea for H ( g ) = − 72 . 8 kJ/mol E i1 for Na ( g ) = + 495 . 8 kJ/mol Heat of sublimation for Na ( s ) = + 1 0 7 . 3 kJ/mol Bond dissociation energy for H 2 ( g ) = + 435 . 9 kJ/mol Net energy change for the formation of NaH2 ( s ) from its elements = − 6 0 kJ/mol
Born-4-Iaber cycles, such as those shown in Figures 6.7 and 6.8,are called cycles because they form dosed loops. If any five of the six energy changes ¡n the cycle are known, the value of the sixth can be calculated. Use the following five values to calculate the lattice energy in kilojoules per mole for sodium hydride, NaH(s): E ea for H ( g ) = − 72 . 8 kJ/mol E i1 for Na ( g ) = + 495 . 8 kJ/mol Heat of sublimation for Na ( s ) = + 1 0 7 . 3 kJ/mol Bond dissociation energy for H 2 ( g ) = + 435 . 9 kJ/mol Net energy change for the formation of NaH2 ( s ) from its elements = − 6 0 kJ/mol
Born-4-Iaber cycles, such as those shown in Figures 6.7 and 6.8,are called cycles because they form dosed loops. If any five of the six energy changes ¡n the cycle are known, the value of the sixth can be calculated. Use the following five values to calculate the lattice energy in kilojoules per mole for sodium hydride, NaH(s):
E
ea
for H
(
g
)
=
−
72
.
8 kJ/mol
E
i1
for Na
(
g
)
=
+
495
.
8 kJ/mol
Heat of sublimation for Na
(
s
)
=
+
1
0
7
.
3 kJ/mol
Bond dissociation energy for H
2
(
g
)
=
+
435
.
9 kJ/mol
Net energy change for the formation of NaH2
(
s
)
from its
elements
=
−
6
0
kJ/mol
Using the following data, calculate the lattice energy of calcium chloride:
Ca2+(g) + 2Cl– (g) → CaCl2(s) ΔHlattice = ?
Sublimation enthalpy of calcium ΔH = 177.8 kJ/mol
First ionization energy of calcium ΔH = 590.2 kJ/mol
Second ionization energy of calcium ΔH = 1144.2 kJ/mol
First electron affinity of chlorine ΔH = –349 kJ/mol
Heat of formation of CaCl2(s) ΔH = –795.4 kJ/mol
Bond energy of Cl2 (see Table 2)
Use Hess’s law to calculate the lattice energy of calcium chloride. set-up must show all the chemical equations and you must show how their H values add up to give your answer.
The standard heat of formation of BaBr2BaBr2 is −−764 kJ/molkJ/mol. The first ionization energy of BaBa is 503 kJ/molkJ/mol and its second ionization energy is 965 kJ/molkJ/mol. The heat of sublimation of Ba[Ba(s)→Ba(g)]Ba[Ba(s)→Ba(g)] is 175 kJ/molkJ/mol. The bond energy of Br2Br2 is 193 kJ/molkJ/mol, the heat of vaporization of Br2(l)Br2(l) is 31 kJ/molkJ/mol, and the electron affinity of BrBr is −−325 kJ/molkJ/mol.
Calculate the lattice energy of BaBr2BaBr2.
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY