Question

Draw the Born-Haber cycle for the formation of CaH2, and calculate the value for lattice energy? (You will have to look up the required thermodynamic data)

Answer #1

Heat of formation= Heat of atomization+ Dissociation energy+ (sum of Ionization energies)+ (sum of Electron

affinities)+ Lattice energy

Heat of formation of CaH2 = -181.5 Kj/mol

Heat of atomization --> Ca(s) --> Ca(g) = 187 Kj/mol

IE1 + IE2 of Ca ---> 589.8 and 1145.4 KJ/mol

Dissociation energy of H2 ----> 436 Kj/mol

Electron affinity = 72.769 KJ/mol *2 = 145.538 KJ/mol

Substitute in the above formula

-181.5 = 187 + 589.8 + 1145.4 + 436 + 145.538 + Lattice energy

Lattice energy = -2685.238 KJ/mol

calculate the lattice energy of CsCl using a Born-Haber
cycle.

Construct a Born-Haber cycle to calculate the lattice energy of
MgCl2.
The CRC Handbook of Chemistry and Physics lists the
MgCl2 lattice energy as 2540 kJ mol-1. How does your answer compare
to the literature value?

Use the Born-Haber Cycle to calculate the lattice energy of an
ionic solid which includes a polyatomic ion.

Construct a Born-Haber cycle diagram that would be used to
determine the lattice energy for RbBr. You will need to draw a
clear diagram with arrows show each step transition. Each step
should clearly have any states and charges noted. There are no
calculations for this question

Construct a Born-Haber cycle for the formation of the
hypothetical compound NaCl2, where the sodium ion has a 2+ charge
(the 2nd ionization energy for sodium is given in Table 7.2 in the
textbook).
Part B
If we were to estimate the lattice energy of NaCl2 to be roughly
equal to that of MgCl2 (2326 kJ/mol from Table 8.2 in the
textbook), what value would you obtain for the standard enthalpy of
formation, ΔH∘f, of NaCl2?
Express your answer using...

Use the Born Haber cycle (show relevant steps) to determine the
lattice energy of CsCl (s) from the following data:
Hf 0 [CsCl(s)] = -442.8 kJ/mol; enthalpy of sublimation of
Cesium is 78.2 kJ/mol; enthalpy of dissociation of Cl2 (g) = 243
kJ/mol Cl2 ; IE1 for Cs(g) = 375.7 kJ/mol; electron affinity
enthalpy-EA1 for Cl(g) = -349kJ/mol.
- need answer fast - thanks

Born-Haber cycle for MgO.
a. write the equation illustrating the steps shown in each part
of the Born-Haper cycle.
b. using the information below, calculate the stadarn enthalpy
formation for MgO. Be sure to label the steps of the cycle with
equations and corresponding energy values. values.
Lattice energy for MgO: -3791 kj/mol
heat of sublimination for Mg: +147.7 kj/mol
Bond dissociation for O2: +498.4 kj/mol
First ionization energy for Mg: +738 kj/mol
second ionization energy for Mg: +1451 kj/mol...

Use the Born-Haber cycle, and the following data to
calculate the bond dissociation energy of F2.
Na(g) → Na+(g) + e-(g) ΔrH = IE1 =
500 kJ mol-1
Na(s) → Na(g) ΔsubH = 107 kJ
mol-1
F-(g) → F(g) + e-(g) ΔrH = EA1 = 329
kJ mol-1
Na(s) + 1/2 F2(g) → NaF(s) ΔfH =
-569 kJ mol-1
Na+(g) + F-(g) → NaF(s) ΔlattH =
-928 kJ mol-1

1. Which of the following transition(s) is/are necessary to
construct a Born Haber Cycle for the formation of NaCl solid?
Multiple answers: You can select more than one option
A) Na(s) → Na(l)
B) Na(s) → Na(g)
C) Na(g) → Na^++(g) + e^-−
D) Cl_22(g) → 2Cl(g)
E) Na(s) + ½ Cl_22(g) →NaCl(s)
2. Which of these transitions are exothermic processes? Multiple
answers are accepted.
A) Na(g) → Na(l)
B) Na(s) → Na(g)
C) Na(g) → Na^++(g) + e^-−
D)...

Using the thermochemical data and an estimated value of -2235.2
kJ/mol for the lattice energy for potassium oxide, calculate the
value for the second electron affinity of oxygen
[O− + e- → O2−]. (The answer is 748.5
kJ/mol)
Quantity
Numerical Value
(kJ/mol)
Enthalpy of atomization of K
89
Ionization energy of K
418.8
Enthalpy of formation of solid K2O
-363
Enthalpy of formation of O(g) from O2(g)
249.1
First electron attachment enthalpy of O -141.0

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