Mandinka2 said:
"One, who, through the fault of his parents conception, is a skid mark in society's collective underwear."
You, my good sir, are an assclown.
http://www.urbandictionary.com/define.php?term=assclown
Can I nominate the topic since none of you girls are willin to step up? What about the entrophic pathway common to the steam cracking of ethene within bioreactor design? Make it easier - just at steady-state...
You got me there, good sir- because steam "cracking" is not performed
on ethene, rather than to precursors to
produce ethene as I have described below. As for "entrophic," I have no idea what that means, I'm not sure it's even a word. Did you mean
endothermic?
Ethene can be produced either by
Extraction from natural gas using fractional distillation followed by
steam cracking (the technique for converting alkanes to alkenes)(750 - 900oC) followed by liquefaction of the gas (-100oC) and then further fractional distillation
OR
Extraction from crude oil using fractional distillation followed by
steam cracking(750 - 900oC) of the naphtha or gas-oil fractions followed by liquefaction of the gas (-100oC) and then further fractional distillation.
The cracking process typically involves
endothermic equilibrium reactions such as:
C2H6(g) C2H4(g) + H2(g) H = +138 kJ mol-1
C3H8(g) C2H4(g) + CH4(g) H = +81 kJ mol-1
To maximize the rate of the cracking reactions
1. the temperature can be increased so that the gas particles move more quickly and collide more often
2. increase the pressure which forces the gas particles closer together and collide more often
3. no catalyst is needed to increase the rate of this reaction since the steam provides the required activation energy
To maximize the yield of ethene, by Le Chetalier's Principle
increasing the temperature of the reactions favours the formation of products since the reactions are endothermic. So increasing the temperature speeds up the rate of the reaction and increases the yield of ethene.
a decrease in pressure would favour the the formation of products since there are more gaseous product molecules than there are gaseous reactant molecules. However, a decrease in pressure would slow down the rate of the reaction. For this reason the pressure is kept at or below atmospheric pressure.
removing the product will favour the formation of more product thereby increasing the yield of product. Equilibrium is therefore never actually achieved.
Now I don't know much about bioreactor design, but I can only guess that your poorly worded question asks how is this steam cracking process used within bioreactor design?
My guess is that you're merely referring to the fact that the steam, by virtue of increased pressure and temperature facilitates the breakdown of higher alkanes into lower alkanes which can then be easily dehydrogenated into hydrogen gas (H2) and Methane (CH4) as well as ethene and propene.
What you do with the coke byproduct I still can't understand.
Problem is that steam cracking has a low selectivity, is highly endothermic, and you still have that coke byproduct to deal with.
Personally, I would prefer straight ethane, propane, or butane dehydrogenation or even methane coupling as alternative processes.
Or did I over-analyze and by refering to the "steady state" were you in fact referring to the
propagation step of steam cracking, in which case the answer would be:
H3C + H3CH3 --> CH4 + H3CH2
H3-CH2 --> H2C=CH2 + H
H + H3CH3-CH3 --> H2 + H3CH2
H3CH2 --> etc...
thank you for playing.....assclown