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From: Thomas Koenig <tkoenig@netcologne.de>
Newsgroups: comp.arch
Subject: Re: Continuations
Date: Fri, 19 Jul 2024 11:28:17 -0000 (UTC)
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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?
To me, that would sound like maybe one of the first two, but
knowing nothing about this, I am now firmly speculating :-)

>> And to make sense, -Ea/(RT) is always less then zero.  Reasonable
>> example: Ea = 30 kJ/mol, R=8.314, T=600 K gives you -6.01 as the
>> argument of the exponent, so the term is then ~ 0.002444 .
>
> So, something like [-10:0] ?

Activation energies can also be 180 kJ/mol, but I don't really
know the range that people might want to calculate these values.