| What is the Haber Process Equation? | Its: N₂ + 3H₂ ⇌ 2NH₃ [+ Heat] |
| How is the Nitrogen and Hydrogen Obtained? | -Nitrogen can be gained from the Air [76% = Nitrogen]
-Hydrogen can be gained from Hydrocarbons in Natural Gases or Crude Oil |
| What is the Ammonia used for? | -Simply for Fertilisers |
| In the Haber Process, what are the Conditions used in Industry? | -There is a Pressure of 200 atm [200MPa]
-There is a Temperature of 450 Degrees
-There is an Iron Catalyst present |
| Why is the Pressure, for the Haber Process, like that? | -This is because the High Pressure shifts the Equilibrium Position to the side with the Least Amount of Moles, and here being the Ammonia
-This means the overall Yield is Higher
-Although, the reason why its only 200 atm, and not 1000 atm is because of Expense. It would be an absolutely Nightmare to have a Plant that can Withstand it, and then actually Fund it |
| Why is the Temperature, for the Haber Process, like that? | -Increasing the Temperature would actually mean the Position of Equilibrium will go Against that, and go the Endothermic route making more Hydrogen and Nitrogen, which Isn't needed
-However, Temperature also affects the Rate of Reaction, which means the Lower the Temperature, the Longer it Takes
-450 Degrees is then a Compromise between the Yield and the Rate |
| Why is there a Iron Catalyst in the Haber Process? | -The Catalyst doesn't affect the Equilibrium Position, but it does affect the Rate of Reaction
-This means it allows the Temperature to be Lower, and therefore the Cost Decreases. |
