The harber process Flashcards
what is the equation for Haber process?
N2(g) +3H2(g) - 2NH3(g)
Where are the sources of nitrogen and hydrogen from?
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What is the name of the catalyst used to speed up the reaction?
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Why is it that when ammonia is produced it is quickly liquified?
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Why is high-pressure preferable for a higher yield of ammonia?
High pressure is preferable as it causes the equilibrium to move to the side with the least amount of mols meaning, in this case, the right which is the production of ammonia meaning that it would increase the rate of reaction and also the yield.
What is the downside of high pressure and what is the compromise made?
High pressures can have an extreme downside, first, it is quite cost-effective while it may help increase the reaction it causes a lot of problems. Also, it could have quite a lot of hazardous problems.
The compromise pressure is 200 atmospheres (20 MPa)
What is the forward and back reaction?
As this reaction is exothermic the forward reaction is exothermic but the opposite is endothermic.
why are low temperatures better for the increase of yield?
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What is the downside of low temperatures and how does it affect the rate?
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what is the compromised temperature?
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How does the graph involving yield reactions show the effects of temperature and pressure and why certain compromises were made?
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what happens to the nitrogen and hydrogen that has not been used up?
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