Equilibrium law
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Chemists use equilibrium constants to predict whether or not reactions tend to go.
It is important to bear in mind that even if a reaction tends to go it may yet go very slowly or not at all.
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- I'm doing an investigation on the reaction: Ethanoic acid + ethanol -> ethyl ethanoate + water I have to investigate into any aspect of this equation but I have no idea what to do. I can't find any information on it anywhere. I don't know whether it needs a catalyst or what temperature I can expect the best results. I thought I could investigate into the results at different temperatures but I don't know how I would go about this and I'm supposed to get in a list of apparatus and chemicals before the end of next week. I don't want anybody to do the work for me, I just would like a bit of help please! 220908
- If the reversible reaction: 2H2O(g) --> 2H2(g) + O2(g) occurs at 1 atm pressure and 20% of the steam is converted to hydrogen and oxygen, how do we find the equilibrium partial pressures (in atm) of the components of the equilibrium? 140408
- I recently came across a question in a past examination paper which did not resemble any of the examples I had previously worked out. The question concerns homogeneous pressure equilibria, specifically the equilibrium reaction of the Haber process, N2(g) + 3H2(g) -> 2NH3(g). The question read as follows: nitrogen and hydrogen are introduced into a vessel of fixed volume, each of partial pressure 2 atm. The vessel is maintained at 500 K when the gases react to form an equilibrium mixture having a total pressure of 3.6 atm. Estimate the partial pressures of all gases at equilibrium, and deduce a value for Kp for the equilibrium at 500 K. Any help with shedding some light on how to go about tackling this question would be much appreciated. 130408
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updated: 21 August 2003
