In stage 2 it is better to pressurize the gasses in order to promote more trioxide due to applying gas laws with equilibrium (less room means they bind together). Then as stage 3 occurs it is much easier to equip the chimney with a thermal condenser to liquefy the gasses, removing the need for a chimney and having the reaction fall back down to be captured as "recycling" stated in the video. Edit: My comment is more for small scale experiments when trying to produce the material as needed when the product chemicals are otherwise unobtainable (when testing at home, trying to extract from scratch/natural sources, or due to budget cuts but chemicals are required).
The contact process Sulfuric acid is very valuable. It is used in the manufacture of detergent, dyes, paint, fabric, fertilizers, etc. It is made in a 3 stage process called the contact process. Stage 1- Sulfur is obtained in its elemental form, a solid, it is melted and then combusted. The product formed at this stage is sulfur dioxide. The chemical equation for this is, Stage 2- The sulfur dioxide is converted into sulfur trioxide. The reaction is in equilibrium which means that as the product is formed, the reverse reaction can also occur and it can break down into its reactants. This reaction can be sped up to form sulfur trioxide adding a catalyst, vanadium oxide. This is an exothermic reaction, which means it gives out heat. Usually, this means that the formation of sulfur dioxide the backwards reaction would be favored at higher temperatures. However, the catalyst needs a temperature over 400 degrees centigrade for it to work so the idea is a trade off. The reaction actually takes place at 450 degrees centigrade. You need the gases to reach equilibrium within the very short time that they are in contact with the catalyst in the reactor so having an increased temperature ensures a high rate of reaction meaning you established a forward reaction quickly. Stage 3- Sulfur trioxide is converted into a very concentrated sulfuric acid and the equation is, This liquid is also known as Oleum. It’s very viscous, and releases acidic fumes. It is very important at this stage, to add water carefully, usually as a MIST to sulfur trioxide. This is because the reaction is very exothermic so mixing it with pure water would release a mist of sulfuric acid that would escape into the air. 99.5% pure sulfuric acid is then collected and is shipped off to where it’s needed next. There are some acidic waste gases from stage three which can escape and cause local acid rain. The chimney is usually fitted with acidic scrubbers. These are bases, like sodium carbonate. On contact, they neutralize the fumes forming salt and water.
I m in 8th standard and I was confused between sulphurous acid and sulphuric acid but I think this explanation is beyond my understanding 😅 but anyways thanks for the help
Most of the sources show SO3 to react with H2SO4 in stage 3 to make oleum. My doubt isn't clear yet. What is the source of that H2SO4 which created with SO3 to form oleum? could you kindly explain?
Thank you very much for your simple and clear explanation but I have one question, in the last stage there is sulphuric acid used in converting SO3 to H2S2O7 (oleum), where the first sulphuric acid comes from while the process concerning with manufacturing of it?
It is actually the H2SO4 obtained from the output, which is "recycled" back into the 3rd chamber The reason for why this is done: Initially when the factory is just started, assume that the "first sulphuric acid supply" does not exist. This will produce a resulting sulphuric acid which has low concentration. As this low concentrated H2SO4 is supplied back to the 3rd chamber, the production of oleum (and thus converting back to acid by addition of H2O) will be highly concentrated. And as you can guess, this concentrated result is again resupplied back to the 3rd chamber, and it repeats. What we see in this video is a "steady state" moment, and your question has asked how the "initial state" is started. This is my understanding, please correct me if I'm wrong!
@@AB-80X Thank you for the video!! it made me understand better.. Although I think if I watched that video (in the link) first instead of this one I wouldn't have understood well ^^
YOO I PASSED WITH a B . QUITE GOOD FOR ME😂😂CAUSE THE PAPER WAS VERY TOUGH!! 😫 AND THE WHOLE CLASS DIDNT DO QUITE WELL SO IM HAPPY AND B IS NOT BAD IN O LEVEL S😉
He's very wrong on two points. One is the fact that a plant will NEVER react SO3 with water in the absorption tower, as that would lead to a catastrophic malfunction at the plant. The SO3 gas is diluted by a mist of 98% Sulfuric acid. Secondly, the scrubbers are NOT acidic scrubbers. They are BASIC acid scrubbers.
At the end reaction, you still have one sulfur and the three oxygen from sulfur trioxide. But when you add water, the final product must also have another oxygen and two hydrogens, so in H2SO4, you have sulfur trioxide add water. You basically just add the oxygen and hydrogens from the water onto the sulfur trioxide, if that makes sense.
can you please explain me in detail "why sulphuric acid is added while preparing sulphuric acid?" and another fact if we need to get sulphuric acid while preparing itself is sulphuric acid, for the first time from where we can get it???
i thought they would use condensers on stage "free" aka three you would collect the remaining HSO4 by making it a closed loop system instead of venting off any usable acid.
![[TH] 2024 PMSL SEA W2D5 | Fall | พลาดวันนี้ จะต้องเสียใจ](http://i.ytimg.com/vi/A5-Cuo12p6A/mqdefault.jpg)
Me watching this half an hour before my exam👁👄👁
Best of luck!
Now how was exam goes?
My exams tomorrow
The fact that I’m watching it while I only have 62 mins exactly away from the exam
@@aarohanyt7374 no one asked
The animations helps alot
One of the best chemistry videos I have ever seen . the explanation was just perfect.
Thank you! Glad you think so!
Catalysts DO NOT affect equilibrium. Steering students wrong.
In stage 2 it is better to pressurize the gasses in order to promote more trioxide due to applying gas laws with equilibrium (less room means they bind together). Then as stage 3 occurs it is much easier to equip the chimney with a thermal condenser to liquefy the gasses, removing the need for a chimney and having the reaction fall back down to be captured as "recycling" stated in the video.
Edit: My comment is more for small scale experiments when trying to produce the material as needed when the product chemicals are otherwise unobtainable (when testing at home, trying to extract from scratch/natural sources, or due to budget cuts but chemicals are required).
Chemistry paper tomorrow, its 3:06 am in my country, watchind dis just to get some better concepts :)
From pakistan, right?
And what did you get btw?
SHADOW FIRST LMAO I saw this question coming, I don’t think he’ll respond
@@kingdribs9286 same lol
pakistani logon ke comment literally har youtube educational video pe hain
Did you passed out?
3:10 am for me lol
Well explained and simplified for easier understanding
The contact process
Sulfuric acid is very valuable. It is used in the manufacture of detergent, dyes, paint, fabric, fertilizers, etc.
It is made in a 3 stage process called the contact process.
Stage 1- Sulfur is obtained in its elemental form, a solid, it is melted and then combusted. The product formed at this stage is sulfur dioxide. The chemical equation for this is,
Stage 2- The sulfur dioxide is converted into sulfur trioxide. The reaction is in equilibrium which means that as the product is formed, the reverse reaction can also occur and it can break down into its reactants. This reaction can be sped up to form sulfur trioxide adding a catalyst, vanadium oxide.
This is an exothermic reaction, which means it gives out heat. Usually, this means that the formation of sulfur dioxide the backwards reaction would be favored at higher temperatures. However, the catalyst needs a temperature over 400 degrees centigrade for it to work so the idea is a trade off. The reaction actually takes place at 450 degrees centigrade.
You need the gases to reach equilibrium within the very short time that they are in contact with the catalyst in the reactor so having an increased temperature ensures a high rate of reaction meaning you established a forward reaction quickly.
Stage 3- Sulfur trioxide is converted into a very concentrated sulfuric acid and the equation is,
This liquid is also known as Oleum. It’s very viscous, and releases acidic fumes. It is very important at this stage, to add water carefully, usually as a MIST to sulfur trioxide. This is because the reaction is very exothermic so mixing it with pure water would release a mist of sulfuric acid that would escape into the air.
99.5% pure sulfuric acid is then collected and is shipped off to where it’s needed next.
There are some acidic waste gases from stage three which can escape and cause local acid rain. The chimney is usually fitted with acidic scrubbers. These are bases, like sodium carbonate. On contact, they neutralize the fumes forming salt and water.
I m in 8th standard and I was confused between sulphurous acid and sulphuric acid but I think this explanation is beyond my understanding 😅 but anyways thanks for the help
Wow ultimately explain love the way you teach I am chemistry lover its brilliant explanation I never get
so3 Ka o Kaha se ayaa
@@wanderwonder20 The extra O comes from O2 because of high temp. Without the temperature, SO3 would've not been created.
Most of the sources show SO3 to react with H2SO4 in stage 3 to make oleum. My doubt isn't clear yet. What is the source of that H2SO4 which created with SO3 to form oleum? could you kindly explain?
It is safer to dissolve SO3 in sulphuric acid than in water, so you use some of the acid previously made for this in a sort of recycling process.
this is very helpful for remembering the reaction in exam time
Yeah , true
I scrolled downt to comment that "very well explained "but there are already comments like that
Like if even you scrolled down like me 😂
Great video, thanks for taking the time to explain this concept, really appreciate it!!
Glad you liked it!
heartly thaks for this video....
In simple language explaination i got it...... Really thankful uhh u taech us very well way keep it up this simple way 😃😃😃😃
Glad it was helpful!
Sir SO3 is reacted with sulphuric acid to get oleum ... My question is how u got sulphuric acid to react with SO3 ?
By synthesis process
I guess
We use recycle tanks already filled with sulphuric acid and with recycle pumps we pump it into an absorption column where the reaction takes place
From lead chamber process
the best one ever. the most underrated channel in the whole of TH-cam.
Aww thank you! Much appreciated ♥️
@@fuseschool Are u single ur voice is very nice
Thank you very much for your simple and clear explanation but I have one question, in the last stage there is sulphuric acid used in converting SO3 to H2S2O7 (oleum), where the first sulphuric acid comes from while the process concerning with manufacturing of it?
It is actually the H2SO4 obtained from the output, which is "recycled" back into the 3rd chamber
The reason for why this is done: Initially when the factory is just started, assume that the "first sulphuric acid supply" does not exist. This will produce a resulting sulphuric acid which has low concentration.
As this low concentrated H2SO4 is supplied back to the 3rd chamber, the production of oleum (and thus converting back to acid by addition of H2O) will be highly concentrated.
And as you can guess, this concentrated result is again resupplied back to the 3rd chamber, and it repeats.
What we see in this video is a "steady state" moment, and your question has asked how the "initial state" is started.
This is my understanding, please correct me if I'm wrong!
please make a video on ostwald process of Nitric Acid Preparation
This was really helpful. Thank you so much for this video
nothing to comment except NO#1 youtube studychannel
So nice of you! Thank you! ❤️
@@fuseschool yours welcome
Thanks i was struggling with chemistry
so good this video I got so clear about the topic from this thanku
Very nice
3:24, no it forms sodium sulfate, co2 and water
Step wise explanation is nice for instant revising!
For those who are lazy to read like me.
Your explanation was super. I love it. Thank u
You are welcome 😊
this was very helpful
u helped me in my homework
Thanks a lot!!!!!!! :)
Wow 😮 what an explanation!
very good
Nice one sir
Me-(
Very much helpful. So well explanation. Best sulfuric acid explanation video.
Really? Then watch this. th-cam.com/video/_zj3bMjFclA/w-d-xo.html
He's both wrong and vague in his explanation.
@@AB-80X Thank you for the video!! it made me understand better.. Although I think if I watched that video (in the link) first instead of this one I wouldn't have understood well ^^
Love that this is short
thank you so much!
thanks, got a huge test tmr about hydrocarbons, leChateliers principle, haber process, contact process and equilibrium. :(
Hope it goes well! 🤞
The only awesome..
Outstanding presentation thank you very much guys :-)
Thank you! Glad you liked it!
thanks a lot
very well explained♥️
Thank you 🙂
congrats!!!, YOU just got a subscriber
Nice! Thank you!
thanks for all
Thank you FuseSchool, very cool.
Glad you liked it!
good
This helps lots tommorow is my igcse chemistry exam
Hope your exam went well 🤞
this video really helped me a lot
1:33 Shouldn't the catalyst be Vanadium Pentoxide?
Hey.. Learning made easy with such presentation.. 😉😉
Glad you liked it 😊
Finally I get it thankyou :)
Best explanation!
Thanks!
LolZ I have a chem paper after 2 days this vdo helped a lot 😉 I HOPE I GET GOOD GRADE :( IM NERVOUS FOR MY FINAL EXAM 😥😥
You got this 🙌 We hope you do well!
YOO I PASSED WITH a B . QUITE GOOD FOR ME😂😂CAUSE THE PAPER WAS VERY TOUGH!! 😫 AND THE WHOLE CLASS DIDNT DO QUITE WELL SO IM HAPPY AND B IS NOT BAD IN O LEVEL S😉
Nice 👍 Well done!
Really great explaination!! much appreciable👍👍
Glad you liked it!
What acid fumes are released into the scrubber stacks?
I knew that there was going to be a British accent before watching the video due to the spelling of "sulphuric" haha
well understood teacher i really appreciate.
thank u so much.....!
Most welcome!
This process is very heppfull in my project 😊😊😊😊😊😊😊
Great 👍
wow, well briefed and understood
Thank you! Glad you liked it!
thank u so much ur a beast
No problem!
Thanks you Soo much it's really helpful
Most welcome! Glad it was helpful!
Well explained
Simply handy🤗
Wow Well explained
thanks very much very accurate. but at the end u said acidic scrubbers. isn't it basic scrubbers?
Natrium carbonate scrubs the acid.. so its an acid scrubber
He's very wrong on two points. One is the fact that a plant will NEVER react SO3 with water in the absorption tower, as that would lead to a catastrophic malfunction at the plant. The SO3 gas is diluted by a mist of 98% Sulfuric acid.
Secondly, the scrubbers are NOT acidic scrubbers. They are BASIC acid scrubbers.
Karishmagunnss G hi
Why is sulphur trioxide reacted with sulphuric acid to produce sulphuric acid ? It doesn't make sense !
Thankz
in the 3rd stage we have sodium trioxide in gas state , how can we get H2SO4 by just treating SO3 with H2O fine mist?? please explain
At the end reaction, you still have one sulfur and the three oxygen from sulfur trioxide. But when you add water, the final product must also have another oxygen and two hydrogens, so in H2SO4, you have sulfur trioxide add water. You basically just add the oxygen and hydrogens from the water onto the sulfur trioxide, if that makes sense.
I am fan your brilliant explaination
Glad you like it!
Does catalyst does not used in last stage of the process? And which temperature is used?
(This reaction)
H2SO4 + SO3->H2S3O7
H2S3O7 + H2O-> 2H2SO4
From Tanzania
Thank you soooo much sir 🙏
Most welcome!
Sulphur reacts with oxygen to form Sulphur dioxide.
extremely helpful..👍👍👍
Glad you think so!
thank you very much for this video
You are most welcome!
@@fuseschool can you make videos on igcse book chemistry and biology
thanks a lot!!!
No worries!
Catalyst used is vanadium pentaoxide
Acid Scrubbers? What are they made from and what is their expected lifespan?
If the objective of this process is to get Sulphuric acid, then how do we get Sulphuric acid in stage 3 when SO3 is being reacted to produce Oleum?
Then oleum is reacted with water to form conc s.acid
Super keep it up
Thank you so much!
katalyst doesnt't affext equilibirium. it only decrease activation energy.
It does. Why? Because the catalyst only favours the forward reactions, thus increasing rate of reaction forward, while backwards remains the same
So that equilubrium is reached faster as correctly stated in the narration.
c
yea exactly
This easy method to learn
😎🙌
Chamber process plz
can you please explain me in detail "why sulphuric acid is added while preparing sulphuric acid?" and another fact if we need to get sulphuric acid while preparing itself is sulphuric acid, for the first time from where we can get it???
factorio modders looking to expand the sulfuric acid production line
stage free and fit ve chimneys wiv
Thank 🙏💕 u soo much air
You're welcome 😊
i thought they would use condensers on stage "free" aka three
you would collect the remaining HSO4 by making it a closed loop system instead of venting off any usable acid.
This was very esy to study
Selfuric Acid used in batteries .....is it Correct????
it's too good
very well explained
😘😘😘😘😘😘
ayam kachok ikan kacek
Thank you so much for this clear explanation. :)
Goof work
Please provide me the equation of making of sulfuric acid
Thank you so much!
No worries!
Senku will be pleased
SIR CONTACT PROCESS KAUNSE THEME ME AATA HAI
this guy is gud
i"m sorry but isn't the catalyst Vanadium Pentoxide? V 0
2 5?