Dynamic Equilibrium Flashcards
What are dynamic equilibriums?
Reversible reactions where, in a closed system, the proportions of products and reactants stabilise so the forward and backward reactions move at the same rate, so the amount of products and reactants don’t change
What is Le Chatelier’s principle?
When conditions are changed to alter the proportions of reactant and product, the equilibrium will resist the change
What is the Haber Process and what conditions are needed?
Making ammonia from nitrogen and hydrogen. 450 degrees, 200atm and an iron catalyst.
Why is 200 atm used?
The reaction will try to resist the high pressure by decreasing the pressure, by having less moles of gas. 2 moles is less than 4, so equilibrium shifts right and the yield of ammonia increases.
Why is pressure not put above 200atm?
The cost to run the pressure would exceed the price received for the ammonia, and it would be a safety hazard because the vessel would explode.
Why is 450 degrees used?
The reaction will try to resist a high temperature by decreasing it. The reaction is exothermic, so it will try to make less heat to counter the temperature. The equilibrium shifts left and the yield of ammonia decreases. However, the temperature speeds up the reaction. 450 degrees is when a reasonable amount of ammonia can be made in a reasonable time. The reaction is still quite slow, so an iron catalyst is used to speed the reaction up.
