Doug's Lab - 2015-01-02
In this video, I explain the usefulness of carbon monoxide in the laboratory and industry and show a simple generator of the gas.
Brings back childhood memories of my first attempt at making formic acid- I was feeling very much like a real scientist LOL- i had fashioned Na formate using paraformaldehyde and fairly dilute aqueous H2O2- then i concentrated the liquid, used NaOH to neutralize ( of course, being a kid, i didnt pay very much attention to the weight of the base i added-AND the para was otc with significant impurities...AND I DIDNT KNOW HOW TOUGH IT WAS TO GET RID OF ALL THE WATER TRAPPED IN my homemade NaCOOH- so my stoichiometry was way off, I thought that I had way more NaCOOH than i did by weight and using 98% H2SO4 in large excess...!!!! luckily, after distilling for a while, feeling odd- I aborted--Im STILL sensitive to CO!! Chemistry is NOT for the faint of heart
lesson learned: use hydrochloric instead of sulfuric acid for making formic acid
This is how science class is supposed to be
Beautiful flame color! I like how you put the black board behind it. I have wanted to do this for awhile, but lost my formic acid. anyways good video!
Didnt know you would be in this comment section, But i love your videos! :D
I'm liking your videos more and more lately, thank you for the trip into
the world of chemistry. Sometimes looks almost like MythBusters. I have
a question. Which do you reckon would produce more CO? 2 parts formic
with 1 part sulfuric or 1 part formic with 2 parts sulfuric? Please tell
where did you based your answer. Thanks
"Carbon and monoxide, that old Detroit perfume..."(Papa Hobo, Paul Simon)
Can i carry this reaction in tin canisters?
Thanks for uploading. Your videos are a pleasure to watch.
wow, I did not know that Carbon Monoxide was flammable. that was fascinating to follow along with.
u r a real cat lol
Very interesting video.
I have some questions though.
the endproduct that comes out of the experiment has what consentraition of carbonmonoxide?
How much is roughtly generated in Mol or volume per minute in your setting?
how long will this generate?
regards and thanks for the video
I too had no idea that carbon monoxide was flammable, very informative video Doug thankyou!
i'd like to make CO using UV light from a deuterium lamp to break up CO2,
How much heat will be produced (in Celsius pls), i know its exothermic. and how long did it take to fully end this reaction ?
degrees Celsius is a measure of temperature not heat production. You're looking for a measurement in btu, calories, watts or some other equivalent unit.
I certainly learn something new. I consider myself somewhat of a Layman scientist if such a thing could exist, but I never knew that carbon monoxide was flammable.
Duuuude I hope you had a fume hood. Making CO with concentrated acids and using a BLOW TORCH ON THE GLASS? Not cool man.
At 0:40 there are two smileys! Can you find them?
+Hadinos Sanosam those are covalent bonds
+LargeVirus Destroyed
LV except they are not, they are pairs of electrons
You can also make CO by reacting iodoform with aqueous silver nitrate. Btw, as CO and C2H4 density is equal to air density, these 2 gases are not retained by any gas mask (gas masks work by diferentiating gases based on their density)
Strange, I was given the impression in my hazmat classes that our gas masks essentially worked by filtering and reacting the incoming gas stream within the matrix of the chlorine impregnated activated carbon filter.
Can you tell me more about making a gas drying train, and an absorption unit? Also, in what videos do you use CO?
Interesting video, mainstream states that CO is produced from incomplete combustion from a carbon based fuel and yet I noticed in your production there was a very clean combustion. Care to explain the inconsistency? Also the flame burns with a blue flame yet I've never known carbon to burn blue. So what are you actually burning?
Such an excellent video! I was looking at a table of explosive limits for gasses, saw carbon monoxide and thought whaaa? Carbon monoxide is flammable/explosive?!? Then I tried to find some information and, of course, didn't see anything about it until I found your video. Great demonstration and explanation on the utility of CO in chemistry and metal refining, I'm looking forward to seeing you use it in some reactions.
Can I done this reaction in tin canisters?
Doug plz make a video of how to oxidize methanol using a copper catalyst and how to contain formaldehyde generated by this method ..great channel
Its a bit late now, but I kind of wish you'd added links to the videos you produced certain chemicals for.
make metal carbonyls and can you do a video on making red phosphorous and one on making pyridine from niacin
Yes.. Nickel carbonyl. AKA "liquid death"
@TheBackyardScientist this guy is immortal, uhm he made carbon monoxide
He even survived marriage recently if I'm not mistaken.
Cannot understand you talk too fast!
Would Carbon Monoxide be able to react with Nitrogen monoxide to produce Carbon dioxide and Nitrogen Gas? 2CO + 2NO -> 2CO2 + N2
probably
any videos about NOx please tag me in
Carbon Dioxide is "harmless" LOL.... we should keep in our lungs as much as we can of CO2 then and we could run non stop LOL ...... hey, maybe we can even sell it in bottles for others to breathe it in .... NO, CO2 is harmful, we breathe in Oxygen in Air and we release CO2 ..... actually the faster and longer that we exchange these gases the longer we leave and the more weight we lose...... we eat carbon compounds and dispose most of it the other way but lose the most in weight by exhaling CO2..... and I was going to add something else but I will leave it in suspense for next episode .... nice video and thanks for the opportunity to comment .... ; )
does this work with 85% formic acid? in my knowledge this should work just as fine but i am not sure
Maybe. Remember, this works because H2SO4 dehydrates HCOOH, and too much water in the HCOOH will make the sulfuric absorb all that water instead of the H2O in the HCOOH.
Nice video, sulphur burns with a blue flame which is flammable and which is in sulphuric acid, which also produces hydrogen that is also flammable. Even formic acid contains hydrogen. I really can't understand how it's carbon monoxide. Anyone care to shed some light?
What about putting charcoal into a ceramic tube, igniting it at one end and feeding in oxygen (from a tank or an oxygen concentrator)? The charcoal will heat, initially producing CO2, then producing CO through CO2 + C > 2CO. This can continue as long as charcoal remains in the tube and oxygen is fed in. Rate is controlled by controlling rate of oxygen feed.
hi can you make zippo gas
Carbon dioxide is harmless ... hmmm???
It is
Good afternoon. You have not tried to obtain gasoline from water gas by the Fischer Tropsch reaction. With your level of equipment you can carry out such an experience. If you are interested in course. It is necessary to let water gas flow over a cobalt or iron catalyst. I have studied enough literature on this subject. But so far there is no access to equipment. But it is very interesting to carry out such a reaction. I did primitive experiments and got the smell of gasoline from the reactor, but there were no temperature controllers and everything else.
In general, if you are interested, I can tell you how to make a catalyst and other conditions of experience.
Would this example create a lethal dose?
But if one were to heat the flask with nothing more that a hot water bath, would it be sufficient ?
I read an article in a science magazine talking about the affects of carbon monoxide on the human body, and it is actually as poisonous as hydrogen cyanide gas!
No, actually it is not. Carbon monoxide is quite toxic, no doubt about that. But far less toxic than hydrogen cyanide. Not only carbon monoxide, hydrogen sulfide is also listed under category 4 in health rating. But, they are not same in the toxicity level. Hydrogen sulfide is often compared with hydrogen cyanide in toxicity but actual it is not that toxic. It is because they attack our body almost in the same way but their toxicity levels are different. Our body can tolerate some toxic gases like hydrogen sulfide & ammonia and it converts them into non toxic compounds if the exposure is low. But the story is different in the case of hydrogen cyanide. It will kill you even on short time exposure.
@Shiva Chemist I probably mistaked for something else
Josh Deffenbaugh there is a lot of misinformation out there too
how many ppm
At 7:23 you said you tested that apparatus setup by using it to generate smoke to ensure it was all going out the fume hood - what chemical(s) did you use to generate some smoke?
Is there a simple and safe combo thats ideal for that kinda test? I get I could just light a smoke bomb, but if there's a reaction that can easily be done in a glass setup like yours, without generating too much heat or annoying side products, that would be neat.
If it's exothermic how does it help to warm it up?
@Krisztián Szirtes You are wrong, and bad example.
It was not bad example and he is right in general. When reaction takes place it is because particles interact. However, they don't have to interact everytime they bump into each other. They need right orientation and enough energy in order to form product. the faster those particles are the more energy they have and also more bumping occurs. This happens whether the reaction is exo- or endothermic. What type of reaction it is determines only if energy is released or consumed.
His example was right because you are essentially saying in your first comment that you're doubting heating up the mixture will help it react faster. If it wasn't helping, every exothermic reaction would happen without any action of ours. That would mean that wood would combust on its own, for example. Hence that was good example and you only showed your arrogance.
bad example because by heating firewood you pyrolytically decompose it into charcoal and light hydrocarbon fractions(including methane) which catch on fire, so by heating firewood you preparing fuel(mix of flamable gasses). It is bases of burning wood, burning charcoal is another story and would be better example.
As for adding heat: there is thermodynamic equilibrium, at some point, after adding more heat, numbers of reactions will go slower and eventually in reverse path, so reactions like 2co + o2 = 2co2 after adding too much heat will result in decomposing of co2 into co and o2, same with 2h2 + o2 = 2h2o.
@Lukáš J. can i get full yield without heating?
@That's One Minute Sorry I don't remember the exact situation, but in general exothermic reations will have lower yield with higher temperature and vice versa. Ask more if you will.
When making carbon monoxide, why would you direct the flow of carbon monoxide into a water bath? I saw someone make it this way and the tubing went into the bottom of a two gallon plastic container one fourth full of water, with a second tube coming out the other side of the water bath container. The carbon monoxide was fed through a tube into the water where you could see the bubbles of it coming up through the water, then into the top half of the plastic container, with the second tubing on the top where the gas was going from the plastic water container. Why would they direct the gas into water?
can you react carbon monoxide and hydrogen to create methanol?
I'm no expert, but given the triple bond and hydrogen's electron deficiency, I see no reason why that wouldn't work. How you'd go about doing it or if you need a catalyst is unknown to me, however.
thor holton water gas(mixture of CO and H2)do react to form CH3OH(methanol).However it is endothermic and The resulted methanol also burns.
@Pumpkin McEggington
You'd basically have to hydrogenate the CO. I think that a palladium catalyst should do the trick.
You can but you need very extreme conditions. On the english wiki page on Methanol it says: "Carbon monoxide and hydrogen react over a catalyst to produce methanol. Today, the most widely used catalyst is a mixture of copper and zinc oxides, supported on alumina, as first used by ICI in 1966. At 5–10 MPa (50–100 atm) and 250 °C (482 °F), the reaction is characterized by high selectivity (>99.8%)" so definitly not lab friendly :D
How would I use it to synthesize phosgene?
you don't.
Max Klemke aka myfanwy. Look him up buddy.
What's the polarity of the molecule, the oxygen should have the positive dipole because one of it's normally antibonding pairs is involved in the triple bond, but that doesn't seem right. My instincts say it should have a slight dipole moment with the negative charge being on the oxygen like in all other carbonyl and carboxylic acid, but the fact it's triple bonded with 10 electrons says it has to be positive charge on the oxygen.
Dom Vasta Oxygen is electron-withdrawing through the sigma bond, but electron-donating by the involvement of its lone pair. It turns out that the electron-donating effect and the resulting triple bond character predominate (based on the very short bond length of CO) and that carbon monoxide has a small dipole moment with the negative charge polarized towards the carbon atom.
So why aren't car mufflers flamethrowers
low amount of monoxide and no oxygen in exhaust gas
Idiots often do run their engines super rich without mufflers and add a spark plug to create said flame thrower effect on cars.
wb5rue - 2016-06-06
I didn't know that "Gently" and "torch" could be used in the same sentence.
Atlas WalkedAway - 2018-01-10
Its essentially sloppy PWM control. You can use a million btu element or burner to apply an average of 1btu.
J H - 2020-08-11
@Atlas WalkedAway You consider him torching the flask to speed up the reaction as a form of pulse-width modulation? lol
Atlas WalkedAway - 2020-08-11
@J H Lol, yes. Did you see him controlling the temperature by varying the intensity of a constantly applied flame, or by controlling how long a non varying flame was contacting the glass in pulses of varying time scales?...