- The Haber process is a widely used industrial process to produce ammonia. - It involves the reaction of nitrogen and hydrogen in the presence of a catalyst to produce ammonia. - This reaction is reversible, so it establishes an equilibrium between the reactants and products.

2. - is a most widely used process to produce ammonia.
- It is mainly the reaction of nitrogen from the air with
hydrogen from natural gas to produce ammonia.

3. Chemical reaction
Chemical reaction is the process that leads transformation of one
set of chemical substances in two another substances. In most
chemical reactions a set of substances completely transfer into
another substances.
Example - A + B C
Here there is no left over A or B. Nearly all of the atoms are converted
into C.
REVERSE REACTION Press Here if
Click Here if you can to see the reverse reaction You give Up!

4. Chemical reaction
Chemical reaction is the process that leads transformation of one
set of chemical substances in two another substances. In most
chemical reactions a set of substance completely transfer into another
substances.
Example - A + B C
Here there is no left over A or B. Every single atom is converted into C.
REVERSE REACTION Press Here if
Click Here if you can, to see the reverse reaction You give Up!

5. Chemical reaction
Chemical reaction is the process that leads transformation of one
set of chemical substances in two another substances. In most
chemical reactions a set of chemical substance completely transfer
into another.
Example - A + B C
Sorry ONLY reversible chemical reactions have reverse reaction
Here there is no left over A or B. Every single atom is converted into C.
Press Here if
You give Up!

6. Chemical reaction
REVERSE REACTION
Click Here if you can, to see the reverse reaction
Chemical reaction is the process that leads transformation of one
set of chemical substances in two another substances. In most
chemical reactions a set of chemical substance completely transfer
into another.
Example - A + B C
Here there is no left over A or B. Every single atom is converted into C.
Press Here if
You give Up!

7. Chemical reaction
Chemical reaction is the process that leads transformation of one
set of chemical substances in two another substances. In most
chemical reactions a set of chemical substance completely transfer
into another.
Example - A + B C
Here there is no left over A or B. Every single atom is converted into C.
REVERSE REACTION
Click Here if you can to see the reverse reaction Press Here if
You give Up!

8. Chemical reaction
Chemical reaction is the process that leads transformation of one
set of chemical substances in two another substances. In most
chemical reactions a set of chemical substance completely transfer
into another.
Example - A + B C
Here there is no left over A or B. Every single atom is converted into C.
REVERSE REACTION Press Here if
Click Here if you can to see the reverse reaction You give Up!

9. Reversible Chemical reaction
In Reversible Chemical reaction the chemical reaction doesn’t go
to completion. Instead it involves both forward reaction ( to
produce product) and back reaction ( to produce reactants ).
Example - A + B C
Here A and B react to produce C.
and C decompose to produce
REVERSE
Click Here to see the reverse reaction

10. Reversible Chemical reaction
In Reversible Chemical reaction the chemical reaction doesn’t go
to completion. Instead it involves both forward reaction ( to
produce product) and back reaction ( to produce reactants ).
Example - A + B C
Here A and B react to produce C.
and C decompose to produce
Reverse reaction is possible.

11. Application in Haber Process
During Haber process Nitrogen and Hydrogen react and form
ammonia. This reaction is reversible that it involves both the production
of reactant and product.
N2 + 3H2 2NH3
In the forward reaction , with the help of a catalyst Nitrogen and hydrogen
produce ammonia and the reverse reaction decomposes ammonia in to
Nitrogen and Hydrogen.
Nitrogen Hydrogen Ammonia

12. Application in Haber Process
During Haber process Nitrogen and Hydrogen react and form
ammonia. This reaction is reversible that it involves both the production
of reactant and product.
N2 + 3H2 2NH3
In the forward reaction , with the help of a catalyst, Nitrogen and hydrogen
produce ammonia and the reverse reaction decomposes ammonia in to
Nitrogen and Hydrogen.
Nitrogen Hydrogen Ammonia Heat

13. Application in Haber Process
During Haber process Nitrogen and Hydrogen react and form
ammonia. This reaction is reversible that it involves both the production
of reactant and product.
N2 + 3H2 2NH3
In the forward reaction , with the help of a catalyst, Nitrogen and hydrogen
produce ammonia and the reverse reaction decomposes ammonia in to
Nitrogen and Hydrogen.
Nitrogen Hydrogen Ammonia Heat

14. Application in Haber Process
During Haber process Nitrogen and Hydrogen react and form
ammonia. This reaction is reversible that it involves both the production
of reactant and product.
N2 + 3H2 2NH3
In the forward reaction , with the help of a catalyst, Nitrogen and hydrogen
produce ammonia and the reverse reaction decomposes ammonia in to
Nitrogen and Hydrogen.
Nitrogen Hydrogen Ammonia Heat

15. Application in Haber Process
During Haber process Nitrogen and Hydrogen react and form
ammonia. This reaction is reversible that it involves both the production
of reactant and product.
N2 + 3H2 2NH3
In the forward reaction , with the help of a catalyst, Nitrogen and hydrogen
produce ammonia and the reverse reaction decomposes ammonia in to
Nitrogen and Hydrogen.
Nitrogen Hydrogen Ammonia Heat

17. Definition
The state of a reaction in which both the concentration of the reactant and
the product stays the same through out the reaction is called Equilibrium
state.
Watch Animation
FeOH
Nitrogen Hydrogen Ammonia
When both the forward and the reverse reactions start going at the same rate ,
the reaction achieve equilibrium state.
For a reaction to enter equilibrium state it needs to take place in a closed
system.

18. Definition
The state of a reaction in which both the concentration of the reactant and
the product stays the same through out the reaction is called Equilibrium
state.
FeOH
Nitrogen Hydrogen Ammonia
When both the forward and the reverse reactions start going at the same rate ,
the reaction achieve equilibrium state.
For a reaction to enter equilibrium state it needs to take place in a closed
system.

19. Change in Equilibrium

20. Effect of
Once an equilibrium is established ,
the concentration of the reactant and the product
stays the same through out time ...
FeOH
Nitrogen Hydrogen Ammonia
But what will happen if the concentration of one of
the substances change ... ?
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia

21. Effect of
Once an equilibrium is established ,
the concentration of the reactant and the product
stays the same through out time ...
FeOH
Nitrogen Hydrogen Ammonia
But what will happen if the concentration of one of
the substances change ... ?
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia

22. Effect of
Once an equilibrium is established ,
the concentration of the reactant and the product
stays the same through out time ...
FeOH
Nitrogen Hydrogen Ammonia
But what will happen if the concentration of one of
the substances change ... ?
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia

23. Effect of
Once an equilibrium is established ,
the concentration of the reactant and the product
stays the same through out time ...
FeOH
Nitrogen Hydrogen Ammonia
Increase in Nitrogen Concentration
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia

24. Effect of
Once an equilibrium is established ,
the concentration of the reactant and the product
stays the same through out time ...
FeOH
Nitrogen Hydrogen Ammonia
Increase in Hydrogen Concentration
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia

25. Effect of
Once an equilibrium is established ,
the concentration of the reactant and the product
stays the same through out time ...
FeOH
Nitrogen Hydrogen Ammonia
Decrease in Ammonia Concentration
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia

26. Effect of
If a system at equilibrium experiences a change, the
system will shift its equilibrium to try to compensate
for the change. In doing this new equilibrium will be
achieved.
FeOH
Nitrogen Hydrogen Ammonia
The reaction move to the right and more ammonia will
be produced.
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia

27. Effect of
Once an equilibrium is established ,
the concentration of the reactant and the product
stays the same through out time ...
FeOH
Nitrogen Hydrogen Ammonia
Decrease in Nitrogen Concentration
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia

28. Effect of
Once an equilibrium is established ,
the concentration of the reactant and the product
stays the same through out time ...
FeOH
Nitrogen Hydrogen Ammonia
Decrease in Hydrogen concentration
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia

29. Effect of
Once an equilibrium is established ,
the concentration of the reactant and the product
stays the same through out time ...
FeOH
Nitrogen Hydrogen Ammonia
Increase in Ammonia
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia

30. Effect of
If a system at equilibrium experiences a change, the
system will shift its equilibrium to try to compensate
for the change. In doing this new equilibrium will be
achieved.
FeOH
Nitrogen Hydrogen Ammonia
The reaction move to the left and more Hydrogen and
Nitrogens will be produced.
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia

31. FeOH
Nitrogen Hydrogen Ammonia

32. When the temperature of the reaction decrease , the
exothermic reaction will be favoured because it will
produce the heat that was lost.
FeOH
Nitrogen Hydrogen Ammonia

33. When the temperature of the reaction decrease , the
exothermic reaction will be favoured because it will
produce the heat that was lost.
FeOH
Nitrogen Hydrogen Ammonia

34. When the temperature of the reaction decrease , the
exothermic reaction will be favoured because it will
produce the heat that was lost.
FeOH
Nitrogen Hydrogen Ammonia

35. FeOH
Nitrogen Hydrogen Ammonia

36. When pressure increases , the system will shift so the least
number of gas molecules are formed. The more gas molecules
there are, the more collisions there are. These collisions and
the presence of gas molecules are what cause the pressure to
increase. Also, when pressure decrease, the system will shift so
the highest number of gas molecules are produced.
FeOH
Nitrogen Hydrogen Ammonia
N-N (2) 3 x { H-H ( 2 )} 3 x {N-H-H-H}
2 molecules 3 molecules 3 molecules

37. When pressure increases , the system will shift so the least
number of gas molecules are formed. The more gas molecules
there are, the more collisions there are. These collisions and
the presence of gas molecules are what cause the pressure to
increase. Also, when pressure decrease, the system will shift so
the highest number of gas molecules are produced.
FeOH
Nitrogen Hydrogen Ammonia
N-N (2) 3 x { H-H ( 2 )} 3 x {N-H-H-H}
2 molecules 3 molecules 3 molecules

38. When pressure increases , the system will shift so the least
number of gas molecules are formed. The more gas molecules
there are, the more collisions there are. These collisions and
the presence of gas molecules are what cause the pressure to
increase. Also, when pressure decrease, the system will shift so
the highest number of gas molecules are produced.
FeOH
Nitrogen Hydrogen Ammonia
N-N (2) 3 x { H-H ( 2 )} 3 x {N-H-H-H}
2 molecules 3 molecules 3 molecules