[Stoves] Re Alexis Belonio article

[Robert Penn Taylor]

The equation Hugh gives looks like a one-step forward reaction rate of 
CO to CO2.  There's no nitrogen involved because this rate equation only 
describes the reaction:

CO + OH --> CO2 + H

where OH is created (I assume) via:

O + H2O --> OH + OH

These two reactions can be written as a single reaction:

2 CO + H2O + O --> 2 CO2 + 2 H

and by dividing stoichiometric coefficients to remove the 2 in front of 
CO we get the form:

CO + 0.5 H2O + 0.25 O2 --> CO2 + H

As Hugh mentioned, the terms [CO], [O2], etc in the expression for 
forward reaction rate are the molar concentrations of the respective 
chemical species.  The exponents on these terms come directly from the 
stoichiometry of the reaction, so [CO] gets an exponent of 1, [H2O] gets 
an exponent of 0.5, and [O2] gets an exponent of 0.25.  The remainder of 
the equation is an Arrhenius expression for the rate constant associated 
with this combined reaction.

--Penn Taylor

andrew wrote:
> On Friday 06 April 2007 08:40, Burnham-Slipper Hugh wrote:
>> The rate of the carbon-monoxide-to-carbon-dioxide reaction is
>> given by:
>>
>> [CO] x [O2]^0.25 x [H2O]^0.5 x 2.24e12 x exp(-1.8e8/RT)
> 
> Wow, where does that lot come from, it looks like a partial pressures 
> sum? Can you explain a bit more? What happened to the nitrogen?
> 
> AJH
> 
> 
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