aommaster Posted February 10, 2004 Share Posted February 10, 2004 Ok, i already know that the making of ammonia is an example of a reversible reaction. When u increase the pressure, the forward reaction is encourages. Can u give me an example where the backward reaction is encouraged when the pressure is increased? Thanx alot guys! Link to comment Share on other sites More sharing options...
JaKiri Posted February 10, 2004 Share Posted February 10, 2004 aommaster said in post # :Ok, i already know that the making of ammonia is an example of a reversible reaction. When u increase the pressure, the forward reaction is encourages. Can u give me an example where the backward reaction is encouraged when the pressure is increased? Thanx alot guys! Rewrite the equation so it goes the other way. Link to comment Share on other sites More sharing options...
greg1917 Posted February 10, 2004 Share Posted February 10, 2004 Any equilibrium with more moles of gas on the right. Link to comment Share on other sites More sharing options...
Neurocomp2003 Posted February 10, 2004 Share Posted February 10, 2004 pick up a standard chem book Link to comment Share on other sites More sharing options...
aommaster Posted February 10, 2004 Author Share Posted February 10, 2004 well, i know the theotry already, if there is a higher volume produced thatn is used! Can u please specify an example? Link to comment Share on other sites More sharing options...
VendingMenace Posted February 10, 2004 Share Posted February 10, 2004 Burning of Glucose -- or pretty much any hydrocarbon or carbohydrate Link to comment Share on other sites More sharing options...
JaKiri Posted February 10, 2004 Share Posted February 10, 2004 VendingMenace said in post # :Burning of Glucose -- or pretty much any hydrocarbon or carbohydrate That's not a reversable reaction involving gases, though, is it? Link to comment Share on other sites More sharing options...
VendingMenace Posted February 10, 2004 Share Posted February 10, 2004 why not? Link to comment Share on other sites More sharing options...
JaKiri Posted February 10, 2004 Share Posted February 10, 2004 VendingMenace said in post # :why not? Look at it this way. If I gathered together H2O and CO2, you wouldn't see glucose crystalising out of the air. Link to comment Share on other sites More sharing options...
VendingMenace Posted February 10, 2004 Share Posted February 10, 2004 ah...too much theory, not enough thought on my part. Yeah. Of course in this sense lots of reactions are not reversible. YOu can always get random side products. WHile in theory, all reactions could be reversed. OK, so for reversible, how about Sodium being added to water. Yeah, i think that is a pretty good one, have to think about it, but i have to grade now, so i will try that one for now Link to comment Share on other sites More sharing options...
Cap'n Refsmmat Posted February 10, 2004 Share Posted February 10, 2004 OK, so for reversible, how about Sodium being added to water. Yeah, i think that is a pretty good one, have to think about it, but i have to grade now, so i will try that one for now Sodium would burn/explode, and so I doubt that it's possible. I don't think you can make sodium compressing hydrogen and sodium something (I forgot the rest of the name). Unless the means you were being sarcastic, I wouldn't know. Link to comment Share on other sites More sharing options...
-Demosthenes- Posted February 10, 2004 Share Posted February 10, 2004 Na (sodium) won't explode, it will sizzle a little and make a little light though. If you want something to explode in water you want Francium. It will completely explode on cantact with water, because of the oxygen in water. I think that You can reverse a reaction. If it took in energy to react, then take energy out, and visa versa. It seems logical. Link to comment Share on other sites More sharing options...
greg1917 Posted February 11, 2004 Share Posted February 11, 2004 The question is not whether a reaction can be reversed - many reactions are reversible and reach a state of equilibrium. And francium would explode in theory, yes. You might encounter a problem in the fact that it doesnt occur naturally though, and when it is created it decays almost instantly.You're thinking of caesium. Link to comment Share on other sites More sharing options...
JaKiri Posted February 11, 2004 Share Posted February 11, 2004 Or rubidium Link to comment Share on other sites More sharing options...
wolfson Posted February 11, 2004 Share Posted February 11, 2004 N2(g) + 3H2(g) ‡ 2NH3(g) Backward reaction, ammonia breaks down to give nitrogen and hydrogen Link to comment Share on other sites More sharing options...
wolfson Posted February 11, 2004 Share Posted February 11, 2004 Although for reactions Dalton Law of Partial Pressures usually comes into play, if you add a constant volume of a gas, so that the overall pressure increases, then the volume would be constant so NO change to concentration and NO change in shift. Link to comment Share on other sites More sharing options...
aommaster Posted February 11, 2004 Author Share Posted February 11, 2004 hmm... either i didn't understand what u said, or that this reaction doesn't work Cause, i am looking for a reaction which involves gasses only. The higher the pressure, the less react, as they have reached a point of equilibrium Link to comment Share on other sites More sharing options...
wolfson Posted February 11, 2004 Share Posted February 11, 2004 Mine was Gas Gas Gas Link to comment Share on other sites More sharing options...
YT2095 Posted February 11, 2004 Share Posted February 11, 2004 an easier one that you perform in the lab is that of Lithium Nitrate, the nitrate complex will easily dissasociate with the lithium under temprature, and then quite easily recombine again as the resultant after heating is LiOH and the nitrate complex don`t kid yourself into thinking this same reaction will work with any other nitrate salt, it wont in addition, there are other reactions (more simple) that will occur under pressure and heat, that will revert back to their original states before these conditions were applied. Link to comment Share on other sites More sharing options...
aommaster Posted February 11, 2004 Author Share Posted February 11, 2004 hmmm.... cause my teacher was telling me that there are some reactions that the lower the pressure, the more the forewards reaction. As for wolson's one, the more the presure, the more the forwards reaction to making ammonia! YT, i don't understand ur reactions, could u please explain further? Link to comment Share on other sites More sharing options...
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