I calculated the volume of a mole of 1 inch spheres. It was rather mind blowing. One side of a cube (a mole) of 1 inch spheres will extend from Capitola, CA to Chicago, IL The results were illustrative of how tiny atoms really are and how big, 10^23, really is.
Are you sure you did the homework right? That distance you mentioned according to Google is 3500km = 3.5*10^8, in inches (your damn imperial system, you should really leave that behind...) Makes it around 1.4*10^8, so we are missing many many orders of magnitude...
If we substitute the one inch sphere for a 40mm sphere, then a regulation table tennis ball (ping pong ball) is a convenient representation. So an avogardro number of table tennis balls would exceed the current annual production of balls multiplied by the approximate age of the earth. By many orders of magnitude. This would not be well received by the IOC or China. Such a shame. K.
Great video! The uncanny thing is that over the last few days, I've been thinking about Avogadro's number and wish I had understood this in high school, and "Bam!" TH-cam algorithm suggests your video to me. Pretty wild. I haven't searched for it. Merely thought about it.
nice video, i almost got kinda lost with the sodium, calculation, cause we say Natrium, or cause i am a little untalented with the subject, but thanks to your and so many other nice videos, ill get it.
This is the sort of thing that I had trouble with in school. Why does one mole of oxygen plus two hydrogen make two water? Where does the extra volume go? Energy?
it doesn't make two volumes of liquid water, it makes two volumes of water vapour. it's because, assuming they're at the same temperature and pressure, the same number of molecules of gases occupy the same volume. 2 litres of H2 and 1 litre of O2 turn into 2 litres of H2O. what stays the same is the total number of atoms. but they're arranged in fewer molecules, so they occupy a smaller volume. that assumes the pressure and temperature are maintained.
The key idea that seems to be left out is that in a gas the molecules are so spaced apart that effectively any molecule in a gas takes up the same proportionate amount of "space". E.g., a penny in a stadium and a quarter in a stadium both take up the same "space" if we are only comparing the stadium and how much it's space takes up in a convenient. This means that for gasses, for all practical purposes every (gas) molecule has the same size as every other and so we simplify everything down to pretending there is only one type of gas molecule. This then allows you to do a direct comparison among molecules because if they take up the same "volume" then you can assume they have the same number. This then lets you ignore the number and pretend you are just working with single molecules which lets you do stoichiometry(which the video does talk about. But one has to understand that the space around a molecule of hydrogen and a molecule of oxygen is the "same" space and can be treated as "point particles". Once one can do that then the number is directly related to the volume and one can use the volume to compare numbers(hence leading to stoichiometry). With enough measurements one could eventually use volume relationships to determine molecule relationships in various reactions and then deduce atomic relationships in molecules. Of course there is no reason to necessarily use volume which may be difficult to measure in some cases but transfer that to pressure calculations. Of course once one starts understanding how molecules compose in volume relationships then one starts to understand how they "react" and one can start to understand the molecular substructural relationships.
The term "mole" to mean a large number IS related to the small burrowing mammal . Moles (the small mammals) make piles due to their digging hence the saying " Mountains Out Of Mole Hills. I suspect the etymology you cited used the burrowing small mammal association with making piles . This might be an analogy to " How Many Angel's Can Dance On The Head Of A Pin ? " 😅
This mole shit was troubling me for age... because of my illiterate chem teacher in my 9&10th grade.....how the hell they can be so dumb not to give this same example for starters and i was the brightest in my chem..... Thax mate for making mole go away from my back 😂
Hmmm, I understand how you determine a mole of a molecule by weight, but clearly you can’t weigh out a mole of photons, how do you determine a mole of a massless particle?
I have noticed in more than one video you avoid mentioning where the number seemengly come from... I understand the mole being the number if atoms in 12g of C12 us not the most accurate thing, but is there a reason in particular to avoid this definition? I was 'raised' in chemistry with this 😄
Quite often a foreign-agent Chemist will introduce a Mole into their team pretending she's another Chemist he knows when she's really a physicist, and then she'll undermine their experiment at the crucial moment with a physics thing and disappear back to some physics lab. John Le Carre wrote several novels about this.
Hey best professor can you make a video teaching band gap or detailed look of semiconductors. Thank you for the effort for making such priceless videos .
When chemists mix chemicals, the molecules they're trying to make hava a certain number of each kind of atom. So you need to mix two molecules of this with one molecule of that, and so on. So you want to know a weight of each kind of chemical that's proportional to the number of molecules in it. Surely that's really simple.
I had a question - Why do we even need the concept of a mole? We can just make a chart of number of atoms per gram of every element and use that as an index? What is benefit of EVEN needing the mole or having the avogadros number?
I'd say it's why Ohm Law, V=IR, isn't Seimen's Law V = I/G. (G is conductance). Using atoms per gram involves inverse mass per atom and no one want's that. Also: N_A sets the scale from microscopic to macroscopic, which is nice. Just like "c" sets the speed scale for Galileo vs Einstein, hbar sets the action scale for classical vs quantum, G (/c^4) sets the scale for Newton vs Einstein, and finally k_B sets the scale at which thermodynamics works (e.g. exact knowledge of phase space vs macroscopic averages).
@@DrDeuteron Hmm, makes sense. Its not so much science, but more about convenience then. I guess THAT should be highlighted when it is taught in school, so we know why AN is a benchmark. I guess it is like light year, it gives an idea of not just distance but time as well and convenient for extremely large distances.
I got headache when you say 2 units of water and add "vapor" in writing. Water vapor, at temperature 0⁰C isn't something I can grasp easily, ig makes me think ice-water, Arctis, how can I avoid that vapor will condense? And such. 🤔➕️🔜↪️⏩️⚡️😇
which is 18g of H20 per grain or 18 ml per grain which the chemist-chef would say is a bit much as the dish of rice would be soggy or does each grain of rice contain 6.02214x10exp 23 molecules of stuff then we have a 1:1 ratio. @@fukpoeslaw3613
A mole is needed to convert the weights of atoms or molecules in amus to their conglomerate weight in grams.... End of explanation. If it were not for the Chemistry of Gasses, we might not have 10% of the Understanding of reality that we have today.
This isnt for beginners! - never heard of Zealites. I endured a "chemistry education - 1959 _- 1964, & passd O level GCE . . Why break down Butane - a useful industrial gas, into Methane - a nuisance greenhouse gas? You lost me when talkin about Sulphites!
You are the best teacher. Trust me!
Thank you, that's very kind.
I calculated the volume of a mole of 1 inch spheres. It was rather mind blowing. One side of a cube (a mole) of 1 inch spheres will extend from Capitola, CA to Chicago, IL The results were illustrative of how tiny atoms really are and how big, 10^23, really is.
Are you sure you did the homework right? That distance you mentioned according to Google is 3500km = 3.5*10^8, in inches (your damn imperial system, you should really leave that behind...) Makes it around 1.4*10^8, so we are missing many many orders of magnitude...
@@Earthstorm84 a cube with side 3.5e8 inch will have volume of about 3e25 inch
@@ivoivanov7407 I missed the cube part I thought he was just lining up the molecule to make a distance 😄
If we substitute the one inch sphere for a 40mm sphere, then a regulation table tennis ball (ping pong ball) is a convenient representation. So an avogardro number of table tennis balls would exceed the current annual production of balls multiplied by the approximate age of the earth.
By many orders of magnitude.
This would not be well received by the IOC or China.
Such a shame.
K.
Very well done. Great approach to teaching the basics of the history of chemistry, and how it works.
Other than Periodic Videos, your content is the only other chemistry channel that is fun to watch ❤🎉
My best teacher
In the game Godville, my character has a pet “vengeful mole” that I named Avogadro. Another character had one that I named “Guaca.”
Great video! The uncanny thing is that over the last few days, I've been thinking about Avogadro's number and wish I had understood this in high school, and "Bam!" TH-cam algorithm suggests your video to me. Pretty wild. I haven't searched for it. Merely thought about it.
Thought implantation...telepathy...algorithm/telepathy receiver...
This has been a very educational video, thanks for explaining this.
Nice video, but I had to say the skit was pretty fun. Didn’t expect how the video ended! Bravo
Glad you enjoyed it!
Thanks you for this such pedagogic video. It's wonderful to be able to understand the world around us trough this knowledge !
I knew moles were involved, great film !
My god that’s outstanding! Subscribed
Thanks for the detail.
Excellent opening skit!
nice video, i almost got kinda lost with the sodium, calculation, cause we say Natrium, or cause i am a little untalented with the subject, but thanks to your and so many other nice videos, ill get it.
As always, u amaze and amuse me. I'm SO SO into chemistry bcs of u.
That's a perfect explanation, thank you!
This is the sort of thing that I had trouble with in school. Why does one mole of oxygen plus two hydrogen make two water? Where does the extra volume go? Energy?
it doesn't make two volumes of liquid water, it makes two volumes of water vapour. it's because, assuming they're at the same temperature and pressure, the same number of molecules of gases occupy the same volume.
2 litres of H2 and 1 litre of O2 turn into 2 litres of H2O. what stays the same is the total number of atoms. but they're arranged in fewer molecules, so they occupy a smaller volume. that assumes the pressure and temperature are maintained.
@@MusicalRaichu thanks for the explanation
Love this!
Well explained, I’m a little closer thanks
The key idea that seems to be left out is that in a gas the molecules are so spaced apart that effectively any molecule in a gas takes up the same proportionate amount of "space". E.g., a penny in a stadium and a quarter in a stadium both take up the same "space" if we are only comparing the stadium and how much it's space takes up in a convenient. This means that for gasses, for all practical purposes every (gas) molecule has the same size as every other and so we simplify everything down to pretending there is only one type of gas molecule. This then allows you to do a direct comparison among molecules because if they take up the same "volume" then you can assume they have the same number. This then lets you ignore the number and pretend you are just working with single molecules which lets you do stoichiometry(which the video does talk about. But one has to understand that the space around a molecule of hydrogen and a molecule of oxygen is the "same" space and can be treated as "point particles". Once one can do that then the number is directly related to the volume and one can use the volume to compare numbers(hence leading to stoichiometry). With enough measurements one could eventually use volume relationships to determine molecule relationships in various reactions and then deduce atomic relationships in molecules. Of course there is no reason to necessarily use volume which may be difficult to measure in some cases but transfer that to pressure calculations. Of course once one starts understanding how molecules compose in volume relationships then one starts to understand how they "react" and one can start to understand the molecular substructural relationships.
It's the constant by which conservation of mass is maintained
Great video - and I just loved the skit! Set the moles free! LOL!
Fun fact. We in Europe measure rice in grams (instead of cups), just like if we were all chemists.
Smart, not fun.
Everyone knows how is so much accurate measuring something in weight than in volume. Even more when you are dealing with a solid.
There are two types of countries... 😂
@@FelonyVideos This myth was already debunked. NASA used SI units for Apollo missions.
The term "mole" to mean a large number IS related to the small burrowing mammal . Moles (the small mammals) make piles due to their digging hence the saying " Mountains Out Of Mole Hills. I suspect the etymology you cited used the burrowing small mammal association with making piles . This might be an analogy to " How Many Angel's Can Dance On The Head Of A Pin ? " 😅
You should make more videos.... 🎩 ❤❤❤
This mole shit was troubling me for age... because of my illiterate chem teacher in my 9&10th grade.....how the hell they can be so dumb not to give this same example for starters and i was the brightest in my chem..... Thax mate for making mole go away from my back 😂
Hmmm, I understand how you determine a mole of a molecule by weight, but clearly you can’t weigh out a mole of photons, how do you determine a mole of a massless particle?
I have noticed in more than one video you avoid mentioning where the number seemengly come from... I understand the mole being the number if atoms in 12g of C12 us not the most accurate thing, but is there a reason in particular to avoid this definition? I was 'raised' in chemistry with this 😄
most interesting this formula spills over into weather chemistry. Is it the basis of C.A.P.E.?
Is that 23L or 22.4L
Quite often a foreign-agent Chemist will introduce a Mole into their team pretending she's another Chemist he knows when she's really a physicist, and then she'll undermine their experiment at the crucial moment with a physics thing and disappear back to some physics lab. John Le Carre wrote several novels about this.
Hey best professor can you make a video teaching band gap or detailed look of semiconductors. Thank you for the effort for making such priceless videos .
Volumes at standard pressure and temperature
Nice explanation.. kindly upload lecture on reaction mechanism in organic chemistry
When chemists mix chemicals, the molecules they're trying to make hava a certain number of each kind of atom. So you need to mix two molecules of this with one molecule of that, and so on. So you want to know a weight of each kind of chemical that's proportional to the number of molecules in it. Surely that's really simple.
i like ur little jokes, cute so nice and english.😜
13:37 Water* ❤
Since it’s just a number to scale by why not make it a simpler number?
I had a question - Why do we even need the concept of a mole? We can just make a chart of number of atoms per gram of every element and use that as an index? What is benefit of EVEN needing the mole or having the avogadros number?
I'd say it's why Ohm Law, V=IR, isn't Seimen's Law V = I/G. (G is conductance). Using atoms per gram involves inverse mass per atom and no one want's that.
Also: N_A sets the scale from microscopic to macroscopic, which is nice. Just like "c" sets the speed scale for Galileo vs Einstein, hbar sets the action scale for classical vs quantum, G (/c^4) sets the scale for Newton vs Einstein, and finally k_B sets the scale at which thermodynamics works (e.g. exact knowledge of phase space vs macroscopic averages).
@@DrDeuteron Hmm, makes sense. Its not so much science, but more about convenience then. I guess THAT should be highlighted when it is taught in school, so we know why AN is a benchmark. I guess it is like light year, it gives an idea of not just distance but time as well and convenient for extremely large distances.
★★★★★ You are a stellar educator. If you only had a sense of humour…
I got headache when you say 2 units of water and add "vapor" in writing. Water vapor, at temperature 0⁰C isn't something I can grasp easily, ig makes me think ice-water, Arctis, how can I avoid that vapor will condense? And such.
🤔➕️🔜↪️⏩️⚡️😇
Should I wash the 752 grains of rice separately before I cook them individually in very tiny pots? 😅
No, you can rinse them together.
And then separate them into tiny pots with tweezers.
@@ThreeTwentysix
😃
Depends on how many molecules of water you are going to use to cook them in, I always eyeball about 602214000000000000000 molecules per grain.
which is 18g of H20 per grain or 18 ml per grain which the chemist-chef would say is a bit much as the dish of rice would be soggy or does each grain of rice contain 6.02214x10exp 23 molecules of stuff then we have a 1:1 ratio. @@fukpoeslaw3613
Does this explain the two moles of water? 2H2 + 2O2 = 2H20
There isn't even a question there, so what's there to explain lol
I can easily imagine a million of something. A cube of 100 things on each edge.
But i also regularly use the term "brazillian". 😂
People want to convert moles to liters but they are incorrect. Moles come in LITTERS. 🤣
They use moles to spy on chemical reactions. That’s all I learned in my college Chem 101 class.
At t=8:37 he said 23 l and suggested a small fish tank. There is something fishy here...
A mole is needed to convert the weights of atoms or molecules in amus to their conglomerate weight in grams.... End of explanation.
If it were not for the Chemistry of Gasses, we might not have 10% of the Understanding of reality that we have today.
...bit of an aside.
Medics love their latin too.
So a skin mole is a pile of keratinocytes?🤔
I don't mean to alarm you, but i think there might be mole in your lab.
Mole🐀🐀🐁🐁??
Lmao had me dying. You fiend. The moles have poor eyesight, it'll take them forever
This isnt for beginners! - never heard of Zealites. I endured a "chemistry education - 1959 _- 1964, & passd O level GCE . . Why break down Butane - a useful industrial gas, into Methane - a nuisance greenhouse gas? You lost me when talkin about Sulphites!
NO I CARNT IMAGINE A MILLION MOLECULES BETWEEN YOR FINGERS BUT IMAGINING INFINITY IS EASY,
They work cheap
Is it because they are cute and furry and catch worms?
why not use them, since biologists use rats and physicists use cats?
The concept was formulated by Dr. Mohl or mol,...not "mole"!!!
And one mol-ecule is a fraction of a mol, right?
Like a millimeter is a fraction of a meter ...
@@notconnected3815 Okay, so maybe that is the origin of the name.