200atm, 450*C, in the prescense of a iron catalyst.
2 of 10
Describe rate of reaction, when pressure is increased.
One mole of H, and two moles of N ---> two moles of NH3. Higher pressure increases yield of ammonia.
3 of 10
Describe the iron catalyst.
Speeds up rate of reaction, but, it has NO EFFECT on production of ammonia.
4 of 10
How is the ammonia removed from the system? What happens to the unreacted H2, and N?
Removed by cooling (forms a liquid). Unreacted H2, and N are recycled back into the system.
5 of 10
Describe Le Chatelier's principle.
Le Chatelier stated that a system will shift equilibrium to oppose any change placed upon the system.
6 of 10
The the equilibrium: temperature.
For every reversible reaction one direction will always be exothermic (-ve ΔH) and the other way will always be endothermic (+ve ΔH). Increasing/decreasing temp. will cause the system to oppose the change.
7 of 10
Describe the equilibrium: pressure.
If we increase the pressure then equilibrium will shift to oppose this change. The reaction which results in the fewest number of moles will be favoured as this lead to a reduction in pressure. Descrease pressure will favour side with most moles fav.
8 of 10
Describe the temperature compromise.
Low Temperature •Using low temperature will shift the equilibrium to favour the exothermic reaction. The forward reaction is exothermic (-ve ΔH) so more products will be produced, this will oppose the change. Too low a temp.
9 of 10
Describe the pressure compromise.
High Pressure. This will shift equilibrium to favour forwards reaction which leads to fewer number of moles. However, too high a pressure is expensive.
10 of 10
Other cards in this set
Card 2
Front
Describe the conditions used for the process.
Back
200atm, 450*C, in the prescense of a iron catalyst.
Card 3
Front
Describe rate of reaction, when pressure is increased.
Back
Card 4
Front
Describe the iron catalyst.
Back
Card 5
Front
How is the ammonia removed from the system? What happens to the unreacted H2, and N?
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