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 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. Chemical reaction REVERSE REACTION Click Here if you can to see the reverse reaction Press Here if You give Up!

4. 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. Chemical reaction REVERSE REACTION Click Here if you can, to see the reverse reaction Press Here if You give Up!

5. 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. Chemical reaction Sorry ONLY reversible chemical reactions have reverse reaction Press Here if You give Up!

6. 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. Chemical reaction REVERSE REACTION Click Here if you can, to see the reverse reaction Press Here if You give Up!

7. 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. Chemical reaction REVERSE REACTION Click Here if you can to see the reverse reaction Press Here if You give Up!

8. 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. Chemical reaction REVERSE REACTION Click Here if you can to see the reverse reaction Press Here if You give Up!

9. 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 Reversible Chemical reaction REVERSE Click Here to see the reverse reaction

10. 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 Reversible Chemical reaction Reverse reaction is possible.

11. During Haber process Nitrogen and Hydrogen react and form ammonia. This reaction is reversible that it involves both the production of reactant and product. N 2 + 3H 2 2NH 3 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. Application in Haber Process NitrogenHydrogenAmmonia

12. 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. During Haber process Nitrogen and Hydrogen react and form ammonia. This reaction is reversible that it involves both the production of reactant and product. N 2 + 3H 2 2NH 3 Application in Haber Process NitrogenHydrogenAmmonia Heat

13. 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. During Haber process Nitrogen and Hydrogen react and form ammonia. This reaction is reversible that it involves both the production of reactant and product. N 2 + 3H 2 2NH 3 Application in Haber Process NitrogenHydrogenAmmonia Heat

14. 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. During Haber process Nitrogen and Hydrogen react and form ammonia. This reaction is reversible that it involves both the production of reactant and product. N 2 + 3H 2 2NH 3 Application in Haber Process NitrogenHydrogenAmmonia Heat

15. 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. During Haber process Nitrogen and Hydrogen react and form ammonia. This reaction is reversible that it involves both the production of reactant and product. N 2 + 3H 2 2NH 3 Application in Haber Process NitrogenHydrogenAmmonia Heat

17. Definition NitrogenHydrogenAmmonia 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 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. Watch Animation

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

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

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

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

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

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

26. Effect of NitrogenHydrogenAmmonia FeOH Use the arrows to control the concentration. The reaction move to the right and more ammonia will be produced. Nitrogen HydrogenAmmonia 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.

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

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

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

30. Effect of NitrogenHydrogenAmmonia FeOH Use the arrows to control the concentration. The reaction move to the left and more Hydrogen and Nitrogens will be produced. 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. Nitrogen HydrogenAmmonia

31. NitrogenHydrogenAmmonia FeOH

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

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

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

35. NitrogenHydrogenAmmonia FeOH

36. NitrogenHydrogenAmmonia FeOH 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. N-N (2)3 x { H-H ( 2 )} 3 x {N-H-H-H} 2 molecules 3 molecules

37. NitrogenHydrogenAmmonia FeOH 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. N-N (2)3 x { H-H ( 2 )} 3 x {N-H-H-H} 2 molecules 3 molecules

38. NitrogenHydrogenAmmonia FeOH 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. N-N (2)3 x { H-H ( 2 )} 3 x {N-H-H-H} 2 molecules 3 molecules