NH4OAc(s) ---> AcOH(l) + NH3(g)
i imagine this could be a problem, since NH3(g) is constantly
removed from the equilibrum. if this is not a problem, then
why?
Because the reaction between acetic acid and ammonia is exothermic. For the reaction to go the other way, it would require added energy to do so.
But that kinda makes me think, because all I really know is that the reaction between an ammonium salt and an acid is exothermic. And one reason for that is most definately the formation of water in the reaction. So if the ammonia atom isn't protonated, and there's no water to be formed, then will the reaction be exothermic, or will it happen at all? I'd bet it will, but now it's just got me thinking. ::)
Post 71294 (missing)
(lugh: "Re: Anhydrous or not....", Methods Discourse)