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From: Thomas Koenig <tkoenig@netcologne.de>
Newsgroups: comp.arch
Subject: Re: Continuations
Date: Sat, 20 Jul 2024 08:53:26 -0000 (UTC)
Organization: A noiseless patient Spider
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Michael S <already5chosen@yahoo.com> schrieb:
> On Fri, 19 Jul 2024 11:28:17 -0000 (UTC)
> Thomas Koenig <tkoenig@netcologne.de> wrote:
>
>> Michael S <already5chosen@yahoo.com> schrieb:
>> > On Thu, 18 Jul 2024 18:48:45 -0000 (UTC)
>> > Thomas Koenig <tkoenig@netcologne.de> wrote:
>> >  
>> >> Michael S <already5chosen@yahoo.com> schrieb:  
>> >> > On Thu, 18 Jul 2024 17:06:52 -0000 (UTC)
>> >> > Thomas Koenig <tkoenig@netcologne.de> wrote:    
>> >> >> It does work far away from the equilibrium (which is the
>> >> >> point).    
>> >> >
>> >> > But how far?
>> >> > Does it work for EA/RT outside of, say [-10:+12] ?    
>> >> 
>> >> Ea is almost always positive; if if was negative, it would mean
>> >> that a reaction is is slowed down by increasing temperature (and
>> >> by this don't mean the reverse reaction).   
>> >
>> > In the branch of physical chemistry that I was taught before
>> > switching to completely different profession, that's not that rare.
>> > For example, when temperature grows from 1500 degrees toward 1550
>> > the transfer of phosphorus from molten steel to slag decelerates
>> > greatly.  
>> 
>> Do you happen to recall if that process was limited by thermodynamic
>> equilibrium, by mass transfer or indeed by a chemical reaction?
>
> I don't know, but would think that what causes it is an approuch to
> equilibrium. But at 1550 degrees equilibrium is still pretty far away
> (50-70 degrees away? I don't remember) and despite that a slowdown is
> already very significant.

That would also be covered by the Arrhenius equation - you have one
reate for the forward reaction and one rate for the backward reaction.