Chemical equilibrium with real examples
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- Опубликовано: 7 сен 2024
- In this video two experiments showing the chemical equilibrium and the law of mass action are explained.
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Finally, a video with actual demonstrations instead of just a bunch of talk and calculations to melt your brain
I once made a Nitrogen dioxide equilibrium jar back when I started chemistry. I kept it all the way up until a few weeks ago. It stayed with me through moving houses two times. When I finally tried opening it, it had sealed itself and I had to destroy the lid of the jar. Good to see you back, my friend!
I made a few of these a while ago and I occasionally play with them, when I look through my stuff. It's like a Fitzroy's Storm Glass. Once you make it, you can have a look at it now and then.
😂
thank you sir performing experiments makes us more clear about the topic of equilibrium
Awesome video! Exactly what I need for my chemistry exam!
Thanks! Glad I could help! :)
@Orville Lam Can i ask something? How old are you?
@@fourinchorange How old do u think I am?
@@orvillelam3550 I dont know man, I just wondered how old you learn these lesson in your country.
@@fourinchorange In where I'm from, they teach only teach Chemistry in high schools, and then re-teach the topics taught in high schools in the first semester of year 1 in universities (at least for me)
Nic video.I watch from India 🇮🇳
What a great video . I'm chemistry edu student from Indonesia. Thanks for the explanation sir. I really need this. I'd like to use your video as a reference for my final project. Hope you don't mind about it. Thank you.
Best regards ~ Sriza Hayati
Lovely. Thanks for this. I will have to use the thiocyanate one: I don't have a good demo to show the effect of the stoichiometric coefficients: at least I didn't until now.
Good job. It really helped me :)
thanks
very nice demonstration ! for sure not something intuitive still you see it with your eyes
I am a teacher. i liked it very much.
What is the middle beaker 3:47 in the video? Is it a total equilibrium, with the other 2 beakers favoring reactants on the right and products on the left?
Also is there any safe home chemicals I can use for this experiment?
It's a diluted solution of the iron thiocyanate complex as a comparison. To the left more thiocyanate solution was added and to the right more iron(III) solution. Both cause the equilibrium to shift to the right side of the equation.
@@MarvynG Iron(III) chloride and potassium thiocyanat are pretty safe to use.
Great work sir 👍
Can you explain why dinitrogen dioxide is a not existent molecule?
Great examples!
Iron(III) and thiocyanate makes complex ions. [Fe(III)(SCN)]++ -ion makes the color.
To be very precisely it's three red complexes and equilibria and there are also aqua ligands :
[Fe(SCN)(H2O)5] 2+, [Fe(SCN)2(H2O)4] + and [Fe(SCN)3(H2O)3].
Nevertheless, in some literature it's simply Fe(SCN)3 and within the law of mass action it does look less complicated.
Yes. It is pretty simple system but there is lot of variation how these are explained. I have wondered is [Fe(SCN)3(H2O)3] soluble because it is neutral? I have had impression that the red color is mostly due [Fe(SCN)(H2O)5] 2+ but I could be wrong. If you have info about good articles about the subject I would be pleased to know of them. This reaction is fascinating because of it bloody color.
@@BadPete81 The neutral complex tends to precipitate at some conditions, but it is soluble. There are lots of neutral compounds which are soluble.
There seems to be a whole book about it: link.springer.com/book/10.1007/978-3-030-27316-3
I've got the german book "Anorganische Chemie" 4th edition by Erwin Riedel. On p. 819 it is written, that all three complexes are red. The color is surely due to a charge transfer, so there might be some information if you look for iron(III) thiocyanate and charge transfer.
How many milliliters was your Fe(SCN)3 solution diluted into before being poured into the 3 test tubes? 2:50
however subsequently after adding the FeCl3 to KSCN and letting the solution sit, wouldnt there be significant iron hydrolysis as well? So would the solution need to be acidified in order to prevent the formation of ferric hydroxide. Could you advise me on how I should go about conducting this experimenting so that I may avoid this problem. thank you!
If there would be a problem with the hydrolysis of FeCl3 you can acidify the solution with diluted hydrochloric acid.
good job
I always wondered how one measures the concentrations
By titration.
but titration changes the equilibrium
@@ShroomLab So? You asked how to measure concentration.
@@user255 yeah and you are right. I saw the definition of the equlibrium constant and thought how to measure the concentations to get Kc
I'd guess a titration might be possible by adding a substance that either forms a complex with free iron ions or the ones in the present complex.
Another method would be spectrophotometry. You know the concentrations of the added solutions and measure the attenuation of the right wavelength at different concentrations. You can determine the concentration of the complex and then you know how the other two concentrations should be. And you can determine Kc.
What were the materials used in the experiment?
Glass Ampule
Nitrogen Dioxide
4 beakers
Water
FeCl3 8.11g
Graduated Cylinder
Distilled Water
Stirring rod
0.46g Potassium Thiocyanate
Clamp Stand
Funnel with filter paper
Test tubes
Pipette
Test tube rack
Gloves
@@raymondtagle7163 wowwer chemist
you can use Audacity to remove noise from the audio, it's a free software
I know Audacity, but the last time I tried to remove some noise (with a few programs), I had to work a lot with other effects to make the rest of the audio sound good again. So, I'm waiting to get my hands on a good mic.
awesome!
So, it's absorbing heat at the beginning right
Fantastic thanks a lot my dear lad
How can I get the NO2 gas?
I made this by decomposition of lead(II) nitrate.
What's the clear liquid where 10 ml of both solutions were added?
The solution with the thiocyanate.
reaction between dry ammonia and n2o4
Hi im a student with a chemistry for the IB program and was wondering where you got the nitrogen dioxide for this experiment?
I heated dry lead(II)-nitrate until it decomposed. The product also contains oxygen, but this is not a problem in this case.
good
How u removed potassium from KSCN
R u from Indonesia?
Who is from the flashcards??
mee
Gg pakkkkk