4. the harber process 2.0 / 5 based on 1 rating ? ChemistryHaber and industrial processesGCSEAQA Created by: Vicky FursdonCreated on: 03-03-13 16:38 Define reversible reaction: This is when in a reaction the the product can react themselves to produce the original reactant 1 of 11 Define the equilibrium: When the amount of reactants and products being produced is at a balance 2 of 11 What conditions has the a reversible reaction have to be in for a state of equilibrium? A closed system 3 of 11 If the temperature is raised what happens to the reversible reaction? The endothermic direction would increase 4 of 11 What happens to the reversible reaction if the pressure is lowered? The direction with the most volume will increase 5 of 11 Why are catalysts used ? To speed up both direction of the reaction by the same amount 6 of 11 Where is the nitrogen and hydrogen gained in the harber process? Nitrogen - air, hydrogen - natural gas / crude oils 7 of 11 what are the industrial conditions for the harber process? Pressure - 200 atmospheres, temperature - 450 oc, catalyst - iron 8 of 11 Why is 1000 atmospheres used for the harber process? Because it would be too expensive to build a container that can hold 1000 atmospheres 9 of 11 Why is a high temperature used? Because a high temperature produces yield at a quicker rate than a lower temperature 10 of 11 What happens to the unused nitrogen and hydrogen? It is recycled 11 of 11
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