Question

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?

Answer #1

**Heat of formation of MgCl2 = sublimation of Mg +First
Ionization energy of Mg + second ionization energy of Mg
+**

**
dissociation of Cl2 + 2 x electron affinity of Cl + Lattice energy
fo MgCl2**

**-641.1 KJ/mol = 150 + 737.7 + 1450.7 + 243 -2(348.57)
+Lattice energy of MgCl2**

**Lattice enrgy = -2525 KJ/mol**

**Thus we get value of 2525 KJ/mol compared to 2540
KJ/mol**

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

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...

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)

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

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

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

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

Using standard thermodynamic tables and the following data,
compute the crystal enthalpy of AgBr(c) using the Born-Haber cycle.
The CRC Handbook lists the value as 904 kJ/mol. Compute the %
difference between this value and your result.
Data:
Ag(g) Ag+(g) +
e-
7.576 eV
Br(g) + e-
Br-(g)
324.5 kJ/mol

Post lab question reguarding bomb calorimetry:
Heat capacity for calorimeter: 10403.64
J/◦C
Delta H TTCC: -6864.20 kJ/mol
Resonance energy benzene: 423.01 kJ/mol
ΔE = -7096.54kJ/mol
1. How does the bomb get sealed when it is charged with oxygen
gas?
2. Why is 1 mL of water added to the bomb before the oxygen gas
is added? Would one drop (0.05 mL) of water be satisfactory?
3. Is the mechanical energy of the stirrer included in the heat
capacity of the...

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