Hydrazine,N2H4 burns in oxygen...
A...what are their product?(in chemical equation).
B..How many bondes are broken?
C..How many new bonds are formed from the. product side...
D.Total energy required to break the bond?
E.Total energy realised when new bonds are formed?
F.the overal delta H
Calculate total energy needed to break the bond of the gas hydrazine burns in oxygen
When Hydrazine burn in oxygen,6 bonds are broken. Below is the list of bonds broken;
4xN-H
N-N
O=O
Number of bonds formed
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When Hydrazine burn in oxygen,6 bonds are broken. Below is the list of bonds broken;
4xC-H
N-N
O=O
3 bonds
3 bonds formed
I assume the products are NO2 and H2O
N2H4 + 3O2 ==> 2NO2 + 2H2O
I will get you started but I'm having trouble understanding why you can't count bond broken and bonds formed.
For bonds broken, look at N2H4. There are four N-H bonds broken plus a N-N bond broken to make 5.
Look up the N-H bond to see how much energy is need to break that bond, multiply by 4 and add in the N-N bond. Then look up the O-O bond and multiply that by 3. Add that to the N2H2 bonds. That gives you the total energy needed to break the starting materials. Do the reverse for products.
delta H = reactants - products.
calculate the total energy required to break the bonds
The total energy required to break the bonds in hydrazine can be calculated using the bond dissociation energies (in kJ/mol) of the bonds that are being broken.
The bonds that are being broken are:
- 4 N-H bonds (each N-H bond has a bond dissociation energy of around 391 kJ/mol)
- 1 N-N bond (the N-N bond dissociation energy is around 160 kJ/mol)
- 1 O=O bond (the O=O bond dissociation energy is around 498 kJ/mol)
So the total energy required to break the bonds in hydrazine is:
(4 x 391 kJ/mol) + (1 x 160 kJ/mol) + (1 x 498 kJ/mol) = 2194 kJ/mol
This means that 2194 kJ of energy would be required to completely break apart one mole of hydrazine into its constituent atoms.