partykid_lsd
Bluelighter
anyone know where i can get some good recipes to make moonshine. Thanks
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OD Moderators: Keif’ Richards | negrogesic
Any one know how to make moonshine?!
- Thread starter partykid_lsd
- Start date
Jabberwocky
Frumious Bandersnatch
Ask Uncle Jesse.
Those DAMN DUKE BOYS!!!!!!!!!!!
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"I dislike the drug you are using, but I would defend with my life your right to use it."
- Paraphrase on Voltaire
"He who makes a beast of himself gets rid of the pain of being a man."
- Dr. Johnson
"We do not sense imagination enough to sense what we are missing."
-Jean Toomer
Those DAMN DUKE BOYS!!!!!!!!!!!
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"I dislike the drug you are using, but I would defend with my life your right to use it."
- Paraphrase on Voltaire
"He who makes a beast of himself gets rid of the pain of being a man."
- Dr. Johnson
"We do not sense imagination enough to sense what we are missing."
-Jean Toomer
Hey Optimus....which poison are you talking about? All you are doing is evaporating ethanol and recondensing it in a more concentrated form. There isn't a lot of reaction going on right? It is the easiest thing in the world to make....probably a pain in the ass if you start with mash, but a pressure cooker some tubes and vodka will get ya by jusssss fine. Ethanol evaporates at a lower temp than water, so if you simmer a mixture of ethanol/ water (something like vodka) the ethanol will rise out of the mash and you can cool and collect it. That’s it’s that simple.
"Ethanol evaporates at a lower temp than water"
well.. they are both evaporating at the same temperatures.. ethanol just evaporates FASTER at a lower temp, and BOILS at a lower temp.. so you put the temp above the bioling of ethanol, and below 100 deg celcius, collect the gas coming off and cool it in a seperate container, voila.
well.. they are both evaporating at the same temperatures.. ethanol just evaporates FASTER at a lower temp, and BOILS at a lower temp.. so you put the temp above the bioling of ethanol, and below 100 deg celcius, collect the gas coming off and cool it in a seperate container, voila.
ActiveMatx
Bluelighter
- Joined
- Apr 5, 2001
- Messages
- 745
you can also use juice.
get bunch of apple, grape, etc juice
get it to evaporate at a low temp, collect the steam into a diffrent container and there you have it!
but be careful, your dealing with alchol and fire (heat) be sure not to blow yourself up
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www.matx.net
get bunch of apple, grape, etc juice
get it to evaporate at a low temp, collect the steam into a diffrent container and there you have it!
but be careful, your dealing with alchol and fire (heat) be sure not to blow yourself up
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www.matx.net
This only works if you let the juice ferment. Ethanol is yeast poo. no yeast no poo........guys in jail get jelly and mix it with water and let it sit until it becomes booze. Prune-0 is what I think it is called. Yummy yummy yummy.....The danger here is that you grow some god awful fungus in the juice that will make you really sick. but if you have no other means I guess it would work. barf........
go get some Jack.
go get some Jack.
well.
technically the correct way of saying that is "the vapor pressure of ethanol at the distillation temperature is higher than the vapor pressure of water".
vapor pressure being the partial pressure of the vapor in the atmosphere above the liquid.
the vapor pressure of one component of a mixture of liquids b and c is given by Raoult's law:
P_b = (x_b,l)(P*_b)
where P_b is the vapor pressure of b, x_b,l is the molar fraction (= n_b,l/n_b,l+n_c,l) of liquid b in the mixture, and P*_b is the vapor pressure of pure b at the temperature T of the system.
Raoult's law can also be used to find the composition of a mixture of vapors above a liquid:
x_b,v = (x_b,l)(P*_b) / P, and
x_c,v = (x_c,l)(P*_c) / P
where P is the sum of the partial vapor
pressure of the system:
P = P*_bP*_c / x_b,v(P*_c - P*_b) + P*b
exciting innit?
well, you can then use this to plot an incredibly, almost unbelievably exciting curve--actually, an area bounded by two curves, which you can use to easily predict the composition of the vapor!
but only at constant temperature, yo.
so you have to adapt this and get the constant-pressure version:
x_b,l = P* - P*_c(T) / P*_b(T) - P*_c(T)
and
x_b,v = P*_b (T) P* - P*_c(T) / P* P*_b(T) - P*_c(T)
which you can then use to predict the dependence of the composition of the vapor upon the boiling point of the mixture!
yup, you can actually trace lines up from x°_b to the lower curve of the resultant graph, then over to where it intersects the upper curve, then back down, and that's your new x_b,l2.
this is when things start to suck.
because a simple distillation will result in a mixture having molar fraction of b = x_b,l2 < 1. less than 1? right. this is a problem for those of you who want a) 95% ethanol from rotting grain-ethanol-water b) absolute ethanol from ethanol-methanol.
so you have to do a fractional distillation. you don't actually *use* plates like an oil refinery, you use a column packed with glass rings or something, and allow the vapor to rise slowly, creating a heat gradient wherein the vapor refluxes slowly as it climbs upward, resulting essentially in a large number of distillations equivalent to a certain number of "theoretical plates".
until you get to 95% ethanol, and then intermolecular attraction causes ethanol and water to have the same boiling point. look, it's an azeotrope!
now, since you're probably going to dilute this, it doesn't really matter, but if there's any methanol in there you're going to have a problem.
i don't know the vapor pressure of methanol, and i wouldn't do the calculations anyway.
the basic idea is that roches himself has been called on the following:
a) saying that the boiling point of a substance is the point at which the vapor pressure of the gas phase above the mixture is equal to the atmospheric pressure, when it is in fact the TEMPERATURE at which the vapor pressure of the gas above the mixture is equal to the atmospheric pressure, and
b) pronouncing "azeotrope" incorrectly.
this is especially interesting in light of the fact that no one else in the class knew either one.
and the end result of the abovementioned facts is that you, even if you were me and had a fractional distilling apparatus, will inevitably arrive at one of the following:
a) you drink methanol, go blind, and wish you had spent the $4.25 on a 40 of OE 800,
b) you do the extraction correctly, still end up with some methanol cause you didn't do the fermentation correctly, but it's not enough to hurt you, or
c) you wonder exactly why you're distilling ethanol from water when you have a fractional distillation column, because you're in the same room as a 500 gram jar of o-chlorobenzonitrile and no one's looking.
technically the correct way of saying that is "the vapor pressure of ethanol at the distillation temperature is higher than the vapor pressure of water".
vapor pressure being the partial pressure of the vapor in the atmosphere above the liquid.
the vapor pressure of one component of a mixture of liquids b and c is given by Raoult's law:
P_b = (x_b,l)(P*_b)
where P_b is the vapor pressure of b, x_b,l is the molar fraction (= n_b,l/n_b,l+n_c,l) of liquid b in the mixture, and P*_b is the vapor pressure of pure b at the temperature T of the system.
Raoult's law can also be used to find the composition of a mixture of vapors above a liquid:
x_b,v = (x_b,l)(P*_b) / P, and
x_c,v = (x_c,l)(P*_c) / P
where P is the sum of the partial vapor
pressure of the system:
P = P*_bP*_c / x_b,v(P*_c - P*_b) + P*b
exciting innit?
well, you can then use this to plot an incredibly, almost unbelievably exciting curve--actually, an area bounded by two curves, which you can use to easily predict the composition of the vapor!
but only at constant temperature, yo.
so you have to adapt this and get the constant-pressure version:
x_b,l = P* - P*_c(T) / P*_b(T) - P*_c(T)
and
x_b,v = P*_b (T) P* - P*_c(T) / P* P*_b(T) - P*_c(T)
which you can then use to predict the dependence of the composition of the vapor upon the boiling point of the mixture!
yup, you can actually trace lines up from x°_b to the lower curve of the resultant graph, then over to where it intersects the upper curve, then back down, and that's your new x_b,l2.
this is when things start to suck.
because a simple distillation will result in a mixture having molar fraction of b = x_b,l2 < 1. less than 1? right. this is a problem for those of you who want a) 95% ethanol from rotting grain-ethanol-water b) absolute ethanol from ethanol-methanol.
so you have to do a fractional distillation. you don't actually *use* plates like an oil refinery, you use a column packed with glass rings or something, and allow the vapor to rise slowly, creating a heat gradient wherein the vapor refluxes slowly as it climbs upward, resulting essentially in a large number of distillations equivalent to a certain number of "theoretical plates".
until you get to 95% ethanol, and then intermolecular attraction causes ethanol and water to have the same boiling point. look, it's an azeotrope!
now, since you're probably going to dilute this, it doesn't really matter, but if there's any methanol in there you're going to have a problem.
i don't know the vapor pressure of methanol, and i wouldn't do the calculations anyway.
the basic idea is that roches himself has been called on the following:
a) saying that the boiling point of a substance is the point at which the vapor pressure of the gas phase above the mixture is equal to the atmospheric pressure, when it is in fact the TEMPERATURE at which the vapor pressure of the gas above the mixture is equal to the atmospheric pressure, and
b) pronouncing "azeotrope" incorrectly.
this is especially interesting in light of the fact that no one else in the class knew either one.
and the end result of the abovementioned facts is that you, even if you were me and had a fractional distilling apparatus, will inevitably arrive at one of the following:
a) you drink methanol, go blind, and wish you had spent the $4.25 on a 40 of OE 800,
b) you do the extraction correctly, still end up with some methanol cause you didn't do the fermentation correctly, but it's not enough to hurt you, or
c) you wonder exactly why you're distilling ethanol from water when you have a fractional distillation column, because you're in the same room as a 500 gram jar of o-chlorobenzonitrile and no one's looking.
FreyGrimrod
Bluelighter
- Joined
- Jul 10, 2001
- Messages
- 169
I ferment my own alchol its a fun hobby not necessarily worth it unless you A. enjoy it like me. or B. cant legally buy and are sick of bugging people also like me. or C. make products you like but cant find in a liquore store like mead or dandelion wine rose wine etc. etc. etc. also like me.
I however DO NOT distill my own alchol since thats illegal.
I however DO NOT distill my own alchol since thats illegal.
thanks for the clarification Roches.. i knew i had something wrong with my comment... we didn't touch much on vapor presure in my chem class, some on pure mixtures.. but we never messed with the changes in vapor presure from more than one substance in a solution... oh well. i did get a 3 on the hardest exam i've ever taken in my life, so it's all good (well actually it's not all good cause the statement that i made could have led to trouble..). back to reading about NDMA receptors...
FreyGrimrod
Bluelighter
- Joined
- Jul 10, 2001
- Messages
- 169
A 3 out of a hundred?
lol, 3 out of 5, and that gives me credit for college (the AP course is actually a shitload HARDER than the entry level chem course at FSU so really i'm not getting ENOUGH credit!).. but it's based on how everyone does nationally, and i know my percentage correct was LOW (well i don't know.. but i mean it was the hardest test of any subject i've ever taken.. ever. and everybody at our school in AP Chem thought so, too.. and our teacher is GOOD so it wasn't that.).. so basically nationally... everyone sucked on it.
i think you mean NMDA.
N-methyl-D-aspartate.
back when i was jus a lil karbon-thugling, keepin' it balanced wit tha OSC squad, all jumpin' up lighta in tha air for tha phat reactions bein thrown down back then, i used to think that NMDA was my personal enemy because it was responsible for reality.
remove NMDA, no reality, happy roches.
OH.
check this.
i think this is hilarious myself. all tha molecular biologis' inside!
the A the T the K the A the V
the C the V the L the K the G
the D the G the P the V the Q
the G the I the I the N the F...
["whut whut?" you ask. "that shit be wack, yo," you say. now HOLD IT DOWN INSIDE...]
but this be th'original dubplate bidness, see? be dj zinc wit tha supaoxide dismutase, see? nuff respect, nuff respect. now we be reducin all the free radical inside the place, see? some noise! reverse dem dubplates, come again selekta!
roches' special note: superoxide dismutase has a Cu-Zn ligand which makes it EVEN MORE FUNNY.
N-methyl-D-aspartate.
back when i was jus a lil karbon-thugling, keepin' it balanced wit tha OSC squad, all jumpin' up lighta in tha air for tha phat reactions bein thrown down back then, i used to think that NMDA was my personal enemy because it was responsible for reality.
remove NMDA, no reality, happy roches.
OH.
check this.
i think this is hilarious myself. all tha molecular biologis' inside!
the A the T the K the A the V
the C the V the L the K the G
the D the G the P the V the Q
the G the I the I the N the F...
["whut whut?" you ask. "that shit be wack, yo," you say. now HOLD IT DOWN INSIDE...]
but this be th'original dubplate bidness, see? be dj zinc wit tha supaoxide dismutase, see? nuff respect, nuff respect. now we be reducin all the free radical inside the place, see? some noise! reverse dem dubplates, come again selekta!
roches' special note: superoxide dismutase has a Cu-Zn ligand which makes it EVEN MORE FUNNY.
heh, 3 outta 5... yeah i remember all that "yo, im badass cause my high school chemistry course is harder than college, yo" from the AP crew...
my college had two first-year chemistry courses though
and i took the hard one.
particle in a three-dimensional box what?
i loved how we learned molecular orbital theory on the first day.. all these kids were facing the sudden realization that they werent gonna be doctors and i'm like...
I shall study the structure and reactivity of compounds containing carbon.
i wouldn't have gotten 3 out of 5 though.
i'm good at chemistry, not taking exams.
my college had two first-year chemistry courses though
and i took the hard one.
particle in a three-dimensional box what?
i loved how we learned molecular orbital theory on the first day.. all these kids were facing the sudden realization that they werent gonna be doctors and i'm like...
I shall study the structure and reactivity of compounds containing carbon.
i wouldn't have gotten 3 out of 5 though.
i'm good at chemistry, not taking exams.
mother fucker! (that's me yelling at myself). that's so my luck, to go on flaunting how i'm doing research on NMDA and shit and i go and make a typo and give myself -5 respect points instead of +5; fuck! i think it was habbit thinking i was typing in MDMA... or something.. SHUT UP! STOP LAUGHING AT ME! now i need to start reading my posts before i click submit.
p.s.
chemistry makes the world go 'round... those damn physics people don't know what's up. the science teachers at my school would always get in these little prank contests.. the chem teachers would always win, obviously...
p.s.
chemistry makes the world go 'round... those damn physics people don't know what's up. the science teachers at my school would always get in these little prank contests.. the chem teachers would always win, obviously...