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Haber Process

Haber Process. Touch The screen. Exit. Reversibility. Equilibrium. Haber Process. - 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. Reversibility. Chemical reaction.

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Haber Process

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  1. Haber Process Touch The screen

  2. Exit Reversibility Equilibrium Haber Process - 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. Reversibility. 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. Press Here if You give Up! REVERSE REACTION Click Here if you can to see the reverse reaction

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

  5. Reversibility. 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. Sorry ONLY reversible chemical reactions have reverse reaction 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!

  6. Reversibility. 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. Reversibility. 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 You give Up! Click Here if you can to see the reverse reaction

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

  9. Reversibility. 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. Reversibility. 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. Reversibility. 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. Watch Animation Nitrogen Hydrogen Ammonia

  12. Reversibility. 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 Reverse reaction Forward reaction

  13. Reversibility. 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 Reverse reaction Forward reaction

  14. Reversibility. 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 Reverse reaction Forward reaction

  15. Reversibility. 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 Reverse reaction Forward reaction

  16. Reversibility. Now You have a good knowledge about Reversible reactions So check out what Equilibrium state is. Equilibrium

  17. Equilibrium. 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. Equilibrium. 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. Equilibrium. Change in Equilibrium Factors which affect equilibrium of a reaction. Concentration Pressure Temperature

  20. Equilibrium. 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 ... ? Concentration Use the arrows to control the concentration . Hydrogen Ammonia Nitrogen

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

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

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

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

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

  26. Equilibrium. 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. Concentration FeOH Nitrogen Hydrogen Ammonia The reaction move to the right and more ammonia will be produced. Use the arrows to control the concentration . Hydrogen Ammonia Nitrogen

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

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

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

  30. Equilibrium. 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. Concentration 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 . Hydrogen Ammonia Nitrogen

  31. Equilibrium. FeOH Nitrogen Hydrogen Ammonia Temperature

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

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

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

  35. Equilibrium. FeOH Nitrogen Hydrogen Ammonia Pressure

  36. Equilibrium. 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. Pressure FeOH Nitrogen Hydrogen Ammonia 3 x {N-H-H-H} N-N (2) 3 x { H-H ( 2 )} 3 molecules 3 molecules 2 molecules

  37. Equilibrium. 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. Pressure FeOH Nitrogen Hydrogen Ammonia 3 x {N-H-H-H} N-N (2) 3 x { H-H ( 2 )} 3 molecules 3 molecules 2 molecules

  38. Equilibrium. 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. Pressure FeOH Nitrogen Hydrogen Ammonia 3 x {N-H-H-H} N-N (2) 3 x { H-H ( 2 )} 3 molecules 3 molecules 2 molecules

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