Manufacturing Sulphuric Acid | Reactions | Chemistry | FuseSchool

Manufacturing Sulphuric Acid | Reactions | Chemistry | FuseSchool

Learn the basics about manufacturing sulphuric acid as part of the equilibrium topic within reactions.

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[upinderk]

Me watching this half an hour before my exam👁👄👁

[chandanbs]

One of the best chemistry videos I have ever seen . the explanation was just perfect.

[shahmeeriqbal]

Chemistry paper tomorrow, its 3:06 am in my country, watchind dis just to get some better concepts :)

[sulli]

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).

[adibakhanaastha]

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.

[parthakiran]

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?

[pavankumari.b]

Wow ultimately explain love the way you teach I am chemistry lover its brilliant explanation I never get

[bethgacheru]

Well explained and simplified for easier understanding

[chetanhosalli]

this is very helpful for remembering the reaction in exam time

[amrendrasuman]

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

[abdallahthabit]

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?

[kznspraynozzlesandsystemsp]

Great video, thanks for taking the time to explain this concept, really appreciate it!!

[blanche]

Thanks i was struggling with chemistry

[roshnirs]

Sir SO3 is reacted with sulphuric acid to get oleum ... My question is how u got sulphuric acid to react with SO3 ?

[ghufranranjha]

nothing to comment except NO#1 youtube studychannel

[naveenr]

the best one ever. the most underrated channel in the whole of YouTube.

[suhana.sigdel]

so good this video I got so clear about the topic from this thanku

[annamaheshwari]

In simple language explaination i got Really thankful uhh u taech us very well way keep it up this simple way 😃😃😃😃

[tommyzhao]

3:24, no it forms sodium sulfate, co2 and water

[shifamuhammad]

This was really helpful. Thank you so much for this video