The equations for the heats of the formation of copper (I) oxide,Cu2O and copper(II) oxide,CuO are:

2Cu(s) +1/2 O2(g) CuO(s); ∆Hof =-166.7kj/mol
Cu(s) +1/2 O(g) CuO(s); ∆Hof= -155.2kj/mol
The first and second ionisation energies of copper are 750 and 2000kj/mol respectively;its atomisation energy is 339.3kj/mol.Draw the born haber cycle and calculate the latice energies (∆Hlatt) of two oxides.

To calculate the lattice energies (∆Hlatt) of the two oxides, Cu2O and CuO, we can use the Born-Haber cycle. The Born-Haber cycle is a series of steps that allow us to determine the overall energy change involved in the formation of an ionic compound from its constituent elements.

First, let's start by drawing the Born-Haber cycle:

Cu (s) + 1/2 O2 (g) → CuO (s) (∆Hof = -166.7 kJ/mol)
|
+----- Cu (g) -----------------------------------+
| |
+----- 1/2 O2 (g) → O (g) (bond dissociation energy: D(O-O) = ΔH = + 249.2 kJ/mol)
| |
+----- Cu (g) → Cu (g) + (atomization energy: ΔHsub = + 339.3 kJ/mol)
1st ionization energy: ΔHion1 = + 750 kJ/mol |
|
Electronegativity
difference (+165.0 kJ/mol)
|
+----- O (g) + |
| Cu (g) → Cu+ (g) + e- |
+----- O (g) + |
| Cu+ (g) → Cu2+ (g) + e- |
+----- O2- (g) + |
2e- → O2- (g) |
|
O2- (g) + Cu+ (g) + → Cu2O (s) (∆Hf = ?)

Now, let's calculate the lattice energy (∆Hlatt) of each oxide using the Born-Haber cycle:

For CuO:
Starting from Cu (s) and 1/2 O2 (g), we can see that the overall energy change involves the following steps:
1. Atomization of Cu (g): +339.3 kJ/mol (endothermic process)
2. Formation of Cu+ (g): +750 kJ/mol (endothermic process)
3. Formation of O2- (g): +249.2 kJ/mol (endothermic process)
4. Combination of Cu+ (g) and O2- (g) to form CuO (s): -166.7 kJ/mol (exothermic process)

Using the principle of Hess's Law, the overall energy change (∆Hlatt) for the formation of CuO (s) can be calculated as:
∆Hlatt = ΔHsub + ΔHion1 + ΔHf(O) + ΔHf(Cu) + ΔHLattice
∆Hlatt = +339.3 + 750 + 249.2 + (-166.7) = +1171.8 kJ/mol

For Cu2O:
Starting from Cu (s) and 1/2 O2 (g), we can see that the overall energy change involves the following steps:
1. Atomization of Cu (g): +339.3 kJ/mol (endothermic process)
2. Formation of Cu+ (g): +750 kJ/mol (endothermic process)
3. Formation of O2- (g): +249.2 kJ/mol (endothermic process)
4. Combination of 2 Cu+ (g) and O2- (g) to form Cu2O (s): ∆Hf = ?

To find the ∆Hf for Cu2O, we need to consider the difference in electronegativity (EN) between Cu+ and O2-.

The difference in electronegativity (∆EN) = EN(O) - EN(Cu) = 3.5 - 1.9 = 1.6

The ∆Hlatt for Cu2O can be calculated using the following equation:
∆Hlatt = ∆Hsub + ∆Hion1 + ∆Hion2 + ∆Hf(O2) - ∆Hf(Cu2O) + ∆HLattice
∆Hlatt = +339.3 + 750 + 2000 + 155.2 - ∆Hf(Cu2O) = ∆Hf(Cu2O)

Now, you can calculate the lattice energy (∆Hlatt) for Cu2O using the given values.

To calculate the lattice energies (∆Hlatt) of Cu2O and CuO using the Born-Haber cycle, we need to consider several steps:

1. Formation of gaseous copper atoms:
Cu(s) → Cu(g) (Sublimation) ∆Hsub = Atomization energy = 339.3 kJ/mol

2. Formation of gaseous oxygen atoms:
1/2 O2(g) → O(g) (Bond dissociation) ∆Hbond = Bond dissociation energy of O2 = ? (not given)

3. Formation of copper(I) oxide (Cu2O):
2Cu(g) + 1/2 O2(g) → Cu2O(s) ∆Hf = -166.7 kJ/mol (Given)

4. Formation of copper(II) oxide (CuO):
Cu(g) + 1/2 O2(g) → CuO(s) ∆Hf = -155.2 kJ/mol (Given)

5. Formation of gaseous copper(I) ions:
Cu(s) → Cu+(g) + e- ∆Hion1 = First ionization energy = 750 kJ/mol

6. Formation of gaseous copper(II) ions:
Cu+(g) → Cu2+(g) + e- ∆Hion2 = Second ionization energy = 2000 kJ/mol

7. Formation of gaseous oxygen ions:
O(g) + e- → O-(g) ∆Hea = Electron affinity of O = ? (not given)

8. Formation of solid copper(I) oxide (Cu2O) by lattice energy:
Cu+(g) + O-(g) → Cu2O(s) ∆Hlatt(Cu2O) = ? (to be calculated)

9. Formation of solid copper(II) oxide (CuO) by lattice energy:
Cu2+(g) + O-(g) → CuO(s) ∆Hlatt(CuO) = ? (to be calculated)

To calculate the lattice energy, we can use the following equation:

∆Hlatt = -∆Hf - ∆Hsub - ∆Hbond - ∆Hion1 - ∆Hion2 - ∆Hea

However, since the bond dissociation energy of O2 (∆Hbond) and the electron affinity of O (∆Hea) are not given, we cannot calculate the lattice energies (∆Hlatt) of Cu2O and CuO accurately based on the given information alone.