My teacher uses your videos every week for our AP Bio class and I just used this video because I was confused with something in my textbook, so decided to look it up :p
I think the mole concept is one of those things in science that is at the same time incredibly simple but (and it sounds like a contradiction) as just difficult to "wrap your head around". Main thing is: There are always, always, always the SAME amount (or number) of molecules in one mole: One mole of CO2 has 6.023 X 10^23 molecules (of CO2) in it. And 6.023 X 10^23 molecules happen to weight: 12+16+16 = 40 grams. It's really just a convenient constant number because as Paul points out a couple times: It's the bridge between Mass and Molecules.
Hi! I'm watching this video to try to understand mole conversions enough to tutor my sister. In the practice problem, my answer was 1.91 x 10^23. Is that what it should be? Because the solution has 1.91 x 10^22 and I wasn't sure if that is just a typo or not.
I love this teacher and I hope he continues to make more and more videos for pple to learn from. I love the cations and anoins where he says the cations are like cats who have paws and it is a "pawsitive" lol :) I'll remember this till I die.
Really interesting stuff. One caption was off (NO for CO2) but apart from that the concept of a mole was explained in a much clearer way than KA or any other source I went to.
For the question of Glucose, shouldn't it be .19 x 10^23 ? Do you move the decimal forward? because 5.72 grams of Glucose 1 mol of Glucose 6.02 x10^23 molecules of Glucose x ------------------------- x ------------------------------------------------- 180.18 g of Glucose 1 mol of Glucose = .19 x 10^23 5.72 x 6.02 = 34.4344 34.4344 ----------- = .19111111111.... 180.18
+Weeble68 Me either, I thought 9.01g of water, divided into 18.02 g of water meant that there are 2 mols of water. I don't understand the answer he came up with. Neither do I understand why the crossing off grams. I get that it's something to do with cancelling each other out but don't know how or why.
YAY!!! I got the correct answer!! Chemistry is my most difficult subject. I really struggle. But thank you sooo much for your help!! I actually got the answer correct!
5:19 where did the 3.01 come from??? On the left side you have 6.02 (from the mole equation) but then that 6.02 suddenly changes to 3.01. I have no idea where that number came from.
This video has a typo. When Mr. Anderson is talking about NO, he mentions that the a.m.u. is 30.01. When he is mentioning grams, it says that CO2 has 30.01 grams, but you just said that CO2 had 44.01 grams. Sorry to point this out like this, but it might need to be fixed.
I noticed this too and was thrown off. In the closed captions, he says it correctly, but in the video and audio, he repeats CO2 from the previous example. It should be 1 mol of NO = 30.01 g.
So summarised, would this definition be correct? "A mole is a unit that indicates a volume of a certain element, expressed in a quantity of particles, which is 6.02*10^23. This volume is reached when the number of the mass of this quantity of particles, , expressed in grams, equals ("is the same as" or "matches") the number of the atomic mass of the element, expressed in atomic mass units."
you do a mole bridge calculation. you do the conversion dividing by its atomic mass (but in the unit of grams). at 5:25 in the video, he shows the 5.72 grams of glucose. to solve this, you find the molar mass of glucose, which is 6 carbons (6*12.01~84 grams), 12 hydrogens (12*1.01~12 grams), and 6 oxygens (6*16.0~96 grams). you find the molar mass is 180 grams/mole. you then divide the given sample (5.72 grams) by the molar mass (180 g/mol) which gives you .0318 moles of glucose. that means that your sample is 3.18% of a mole of glucose. You then multiply the number of moles by avogadro's number (6.022*10^23) which gives you 1.91*10^22 molecules of glucose in the 5.72g sample. TL;DR divide gram sample by molar mass (same as atomic weight on periodic table but grams as unit), then multiply by 6.022*10^23
at 7:01 pretty sure you meant 1 mol of NO, not CO2, because the amu was referencing NO, and also, it wouldn't add up for CO2. (Which was your first example and is 44.01g.) A student I tutor pointed this video out to me, and I think it's very well done. But judging by the confusion in many of the comments, I figure anything to make them more confused can't be good.
so you are weighing carbon 12 using some presumed analytical equipment but my question is how do you estimate the mass to charge ratio and give an estimate for the total number of atoms within that sample presumably the problem when teaching this subject is that they leave the physical world out of the equation and leave students guessing
There is a mistake in the video. When you are talking about the mass of NO, then show CO2 on the screen. Shouldn't you have NO on both sides? That part did not make sense
Here he is finding the number of molecules in 9.01g of water NOT the number of moles, so after finding 0.5 you have to do the next step: 0.5 x 6.02x10^23 to get the number of molecules. I also got confused at first but then realised lol
I really want to see if I get this. For some reason this has always been hard for me to understand. In the examples you provide, is it accurate for me to say "There are 6.02 x 10^23 molecules in 30.01 grams of Nitrous Oxide." and "There are 6.02 x 10^23 molecules in 44.01 grams of Carbon Dioxide." Thanks!
Hello, the answer to the problem says to the 22 power, why the 22 and not 23rd (isnt that what the formula is?) please explain, super lost here :( Thank You!
Because, setting up the dimensional analysis you'll have 5.72*(6.022*10^23) (the many grams you have times Avogadro's number to find how many moles that's gonna give you) then divide it by 1 mole of the element (sum of it's atomic weight = 180.18). Setting it up, 34.44584*10^23 / 180.18 = approx. 0.191*10^23. (HERE IS YOUR 10^23). But you want Scientific Notation, so you can't have a zero point something. You have to displace the digit one decimal place to the right, and, by doing so, you'll eliminate one of the 10^n, THEREFORE, you'll go from 0.191*10^23 to 1.91 * 10^22.
@@juguernautajuguernauta5504 THANK YOU! I was going crazy as to why the 5.72 seemed to be converted to 57.2 to get the answer of 1.91 instead of my answer 0.191*10^23.
+Tonya Bigham one of copper would contain 3.8528 times ten to the twenty fifth power. Because a mole equals 6.02 times ten to the twenty third power. And the atomic mass of copper is 63.546, so five would make the three become a four. And now copper becomes only 64. And you multiply the amount per mole by the mass of copper, which would give you your answer. So goes for the rest.....hope I didn't confuse you
Sharing with physical science students because the book doesn't explain why a mole is important besides having another word for 6.02 x 10^23. Thanks! Off to look for thermite burning under water video.
Take a back step on all of what you listen and just reflect, he can do a lot of error. 6.02*10^23 molecules of water weigh 18.02 grams and so to have the number of molecules of water in « 9.01 GRAMS OF WATER » you need to do a CONVERSION. If you use the X product you do visually a table -> « 6.02*10^23 » at the top left and the value associated at his right « 18.02 grams » Now you have the number that do the difference so « 9.01 grams » Put it just below « 18.02 grams » and now you do the X product. « How ??? » it’s simple, you put your pen from 9.02 and you go to 6.02*10^23 « you multiply 9.02 by 6.02*10^23 » And you divided the result of this by « 18.02 ». The result of this calculus give the value searched below of 6.02*10^23 molecules so... 3.01*10^23 molecules of water for 9 grams of water.
I just think of the mole as the number of protons or neutrons I must have to equal a gram of mass which turns out to be 6.022*10^(23) protons or neutrons and therefore a mole of a molecule that has say 200 protons and neutrons = 200 grams of mass,I would just treat it as a conversion factor from grams of a molecule to number of a molecules.
indians are just more grateful in education and parents force their children to take more serious as they live in a shit third world country who are unintelligent to develop and want their child to strain their mind for themselves so their child gives them money in the future...its a stingy concept as they were unable to learn themselves.If Indian people get more intellligent with their economic state it's normal for the younger generation to slack off but the place is shit so they struggle too much being ignorant to just be a doctor and dont get luxury
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This really helps for a year 11 student studying chemistry. Keep up the good work.
Burn under water? Well now we know how sponge bob can have a campfire :P
Angelica Porro yeah right
Do you know where the chemist go shopping?
To the mole :P
Good video, thanks.
My teacher uses your videos every week for our AP Bio class and I just used this video because I was confused with something in my textbook, so decided to look it up :p
Wow, these 7 minutes have been a lot of help! THANK YOU!
I think the mole concept is one of those things in science that is at the same time incredibly simple but (and it sounds like a contradiction) as just difficult to "wrap your head around".
Main thing is: There are always, always, always the SAME amount (or number) of molecules in one mole: One mole of CO2 has 6.023 X 10^23 molecules (of CO2) in it. And 6.023 X 10^23 molecules happen to weight: 12+16+16 = 40 grams.
It's really just a convenient constant number because as Paul points out a couple times: It's the bridge between Mass and Molecules.
Hi! I'm watching this video to try to understand mole conversions enough to tutor my sister. In the practice problem, my answer was 1.91 x 10^23. Is that what it should be? Because the solution has 1.91 x 10^22 and I wasn't sure if that is just a typo or not.
oh wait nevermind I figured out what I did. forgot to move the decimal point and remove one exponnent... whoops
Thank you or this! You explain it better than my teacher does.
I'm confused a bit by the math. When I do the last division problem, I get 3.340732519*10^22 not 3.01*10^23. What am I doing wrong?
You are awesome. You have helped me learn so much material over a variety of topics within the past year. Thank you is not enough!
I love this teacher and I hope he continues to make more and more videos for pple to learn from.
I love the cations and anoins where he says the cations are like cats who have paws and it is a "pawsitive" lol :) I'll remember this till I die.
I don't understand the math behind it. Like when he's crossing off grams and then just comes up with a number what is he actually doing?
+Brooke Williams Same here.
+Rachel Walton would you need help? I understand this stuff now
Yes, i do. What have you learnd that this video doesn't fully cover?
I've got AMU of 180.18. So 1 mole 180 grams right? Than i do the same thing as Andrew did with the other example 57.2 / 180.18 = 0.31
I.ve rounded the 0.315 to 0.32
6.02 X 0.32 = 1.9264 is thos correct? It isn't 1.91 but that's maybe an calculator issue. Is the math correct here?
Someone get this guy a Nobel prize!
Did the question. Got it right = 1.91 x 10^22 . Feeling super smart. Thanks Man!
Thank you so much for these videos! They do help out a great deal in understanding everything
Extremely helpful. In seven minutes explained what took my teacher 2 hours.
5:04 what did he divide 18 by to get 3.01? how did the 3.01 come about?
*9.01* (6.02*10^23) / 18.02 = 3.01 * 10^23 molecules of water.
Really interesting stuff. One caption was off (NO for CO2) but apart from that the concept of a mole was explained in a much clearer way than KA or any other source I went to.
You have provided a awesome explanation
Thank you alot
You just explained something that I was confused about for 11 years :P
Oh My God If Only You Were My Chem Teacher!!!! Thank You.... Very Helpful
Yes, it was a huge help. These videos mean a lot to me, thanks man!
At 3:46, u said that "1 mole of C02 is 30.01 grams". It should be NO instead of CO2.. typo :)
yap thanks a lot it really helped me and i got 96 percent on mole test
This was helpful, now I know something lots of sophomores don't!
For the question of Glucose, shouldn't it be .19 x 10^23 ? Do you move the decimal forward? because
5.72 grams of Glucose 1 mol of Glucose 6.02 x10^23 molecules of Glucose
x ------------------------- x -------------------------------------------------
180.18 g of Glucose 1 mol of Glucose
= .19 x 10^23
5.72 x 6.02 = 34.4344
34.4344
----------- = .19111111111....
180.18
Your answer's right but correct scientific notation would be 1.91 x 10^22. You move the decimal and reduce 10^23 to 10^22
CoolMultiGamer oh ok. Didn't know that. Thanks.
+Kevin Falcon can you talk me through how you got your answer please? I just cant grasp this.
+Weeble68 Me either, I thought 9.01g of water, divided into 18.02 g of water meant that there are 2 mols of water. I don't understand the answer he came up with. Neither do I understand why the crossing off grams. I get that it's something to do with cancelling each other out but don't know how or why.
wat was tat again??
Thank you, Mr. Anderson!
YAY!!! I got the correct answer!! Chemistry is my most difficult subject. I really struggle. But thank you sooo much for your help!! I actually got the answer correct!
5:19 where did the 3.01 come from??? On the left side you have 6.02 (from the mole equation) but then that 6.02 suddenly changes to 3.01. I have no idea where that number came from.
This video has a typo. When Mr. Anderson is talking about NO, he mentions that the a.m.u. is 30.01. When he is mentioning grams, it says that CO2 has 30.01 grams, but you just said that CO2 had 44.01 grams. Sorry to point this out like this, but it might need to be fixed.
I noticed this too and was thrown off. In the closed captions, he says it correctly, but in the video and audio, he repeats CO2 from the previous example. It should be 1 mol of NO = 30.01 g.
Yeah that threw me off too
Yeah, he meant NO not CO2.
You are superb. Thank you for your work! You are doing an amazing job- I am very grateful for helping me!
Thank you Mr Anderson for spreading scientific knowledge. You are amazing 😁
Thank you for this video. Much appreciated and can't wait to see more from you!
So summarised, would this definition be correct?
"A mole is a unit that indicates a volume of a certain element, expressed in a quantity of particles, which is 6.02*10^23. This volume is reached when the number of the mass of this quantity of particles, , expressed in grams, equals ("is the same as" or "matches") the number of the atomic mass of the element, expressed in atomic mass units."
Great Video, it was extremely helpful and comprehensive
You may need to fix typo at the 3:49 minute mark. Otherwise, very good.
I don't really get the whole gram to molecular thing. How do you convert it to molecules?
you do a mole bridge calculation. you do the conversion dividing by its atomic mass (but in the unit of grams). at 5:25 in the video, he shows the 5.72 grams of glucose. to solve this, you find the molar mass of glucose, which is 6 carbons (6*12.01~84 grams), 12 hydrogens (12*1.01~12 grams), and 6 oxygens (6*16.0~96 grams). you find the molar mass is 180 grams/mole. you then divide the given sample (5.72 grams) by the molar mass (180 g/mol) which gives you .0318 moles of glucose. that means that your sample is 3.18% of a mole of glucose. You then multiply the number of moles by avogadro's number (6.022*10^23) which gives you 1.91*10^22 molecules of glucose in the 5.72g sample.
TL;DR divide gram sample by molar mass (same as atomic weight on periodic table but grams as unit), then multiply by 6.022*10^23
Mr Anderson, thanks for the videos! Very helpful
The basic question that needs to be answered is how did Avogadro counted the number particles?
That pretty much helped but is it that for finding the atoms, particles, molecules and formula units, Avogadro's number has to be used?
at 7:01 pretty sure you meant 1 mol of NO, not CO2, because the amu was referencing NO, and also, it wouldn't add up for CO2. (Which was your first example and is 44.01g.) A student I tutor pointed this video out to me, and I think it's very well done. But judging by the confusion in many of the comments, I figure anything to make them more confused can't be good.
i calculated the answer is 2.03x 10^22, and is that wrong?
i rounded up to 3.01
but idk maybe ur right
U reli awsme bozemann i being a indian lyks to watch ur videos which i understnd very easily
Thank you for this awesome vid
how does carbon 12 have 12.01 amu if 1 amu = carbon 12/12?
Great help!! Thank you sir!!
Great video. Thanks for sharing!
You gained a new sub, thank you.
6 years later
So if I'm asked
"What is The Mole?" In an exam, what do i have to write?
so you are weighing carbon 12 using some presumed analytical equipment but my question is how do you estimate the mass to charge ratio and give an estimate for the total number of atoms within that sample presumably the problem when teaching this subject is that they leave the physical world out of the equation and leave students guessing
thank u so much :D i love the way you explain things about science
This video is very helpful thankyou!!!!
Thanks heaps! i finally understand this concept :)
thank you very much, i needed this
3:46 it is nitric oxide
There is a mistake in the video. When you are talking about the mass of NO, then show CO2 on the screen. Shouldn't you have NO on both sides? That part did not make sense
The Math here is confusing. You somewhat glanced over the RATIOS.
5:10 to 5:19, he did the right type of calculations , but i just got 0.5, i didnt take the extra step. Would that be nessesary ?
Here he is finding the number of molecules in 9.01g of water NOT the number of moles, so after finding 0.5 you have to do the next step: 0.5 x 6.02x10^23 to get the number of molecules. I also got confused at first but then realised lol
I really want to see if I get this. For some reason this has always been hard for me to understand.
In the examples you provide, is it accurate for me to say "There are 6.02 x 10^23 molecules in 30.01 grams of Nitrous Oxide." and "There are 6.02 x 10^23 molecules in 44.01 grams of Carbon Dioxide."
Thanks!
yes that is correct
ok great. thank you!
Outstanding video. Thank you.
Awesome tutorial. Thx mate
Well explained ...got that in the first time
Better than Khan Academy. Way more organized and to the point.
Hello, the answer to the problem says to the 22 power, why the 22 and not 23rd (isnt that what the formula is?) please explain, super lost here :(
Thank You!
Because, setting up the dimensional analysis you'll have 5.72*(6.022*10^23) (the many grams you have times Avogadro's number to find how many moles that's gonna give you) then divide it by 1 mole of the element (sum of it's atomic weight = 180.18). Setting it up, 34.44584*10^23 / 180.18 = approx. 0.191*10^23. (HERE IS YOUR 10^23). But you want Scientific Notation, so you can't have a zero point something. You have to displace the digit one decimal place to the right, and, by doing so, you'll eliminate one of the 10^n, THEREFORE, you'll go from 0.191*10^23 to 1.91 * 10^22.
@@juguernautajuguernauta5504 THANK YOU! I was going crazy as to why the 5.72 seemed to be converted to 57.2 to get the answer of 1.91 instead of my answer 0.191*10^23.
Helpful as always
I still need help. How much does 1.00 mole of copper contain?
+Tonya Bigham one of copper would contain 3.8528 times ten to the twenty fifth power. Because a mole equals 6.02 times ten to the twenty third power. And the atomic mass of copper is 63.546, so five would make the three become a four. And now copper becomes only 64. And you multiply the amount per mole by the mass of copper, which would give you your answer. So goes for the rest.....hope I didn't confuse you
at 4.56 how can there be 18.02 it should be 17.01
its two hydrogens so its 2.02 + 16.00. dont worry i was tripped up too
thanks! I'm a PhD in chemistry and needed a refresher/s
i just wonder how your mind can gather all these sciences
Thanks for the help, you could have explained how to calculate the mol a little better.
Right, the big hurdle a lot of students struggle with is that amu = g/mol
Sharing with physical science students because the book doesn't explain why a mole is important besides having another word for 6.02 x 10^23. Thanks! Off to look for thermite burning under water video.
this dude can teach
Massive understatement!
Missed opportunity at 2:10 to use a mole of moles for you explanation.
Can the answer be 0.19 times 10 to the 23
Mr. Bozeman, you rock.
srry man but i aint get none of this...
Why are we dividing in h2o example
Wait, this video says 1 mole of CO2 is 30.01 grams after Mr. Anderson explained NO being 30.01 amu?
How do you get 3.01 you literally said you divided 18.02 by 18.02 and it was somehow 3.01???? HOW DOES THAT MAKE SENSE
Take a back step on all of what you listen and just reflect, he can do a lot of error.
6.02*10^23 molecules of water weigh 18.02 grams
and so to have the number of molecules of water in « 9.01 GRAMS OF WATER » you need to do a CONVERSION.
If you use the X product you do visually a table -> « 6.02*10^23 » at the top left and the value associated at his right « 18.02 grams »
Now you have the number that do the difference so « 9.01 grams »
Put it just below « 18.02 grams » and now you do the X product.
« How ??? » it’s simple, you put your pen from 9.02 and you go to 6.02*10^23
« you multiply 9.02 by 6.02*10^23 »
And you divided the result of this by « 18.02 ».
The result of this calculus give the value searched below of 6.02*10^23 molecules so...
3.01*10^23 molecules of water for 9 grams of water.
IT IS 6.02*10 THE POWER OF 23 AND IT IS LIKE A BRIDGE BETWEEN MASS AND PARTICLES.
*Nitric Oxide @3:49
I just think of the mole as the number of protons or neutrons I must have to equal a gram of mass which turns out to be 6.022*10^(23) protons or neutrons and therefore a mole of a molecule that has say 200 protons and neutrons = 200 grams of mass,I would just treat it as a conversion factor from grams of a molecule to number of a molecules.
So amu = mole?
did you divide the 18.02 and 6.02 to the nearest of what? ASAP
I still dont understand :( i think im going to fail chemistry ...
Quantum Unicorn did you fail?
I am slowly understanding... How did u end up going?
Quantum Unicorn did you fail? I know it's 3 years later and all but did you?
so dumb we indian r intelligent
indians are just more grateful in education and parents force their children to take more serious as they live in a shit third world country who are unintelligent to develop and want their child to strain their mind for themselves so their child gives them money in the future...its a stingy concept as they were unable to learn themselves.If Indian people get more intellligent with their economic state it's normal for the younger generation to slack off but the place is shit so they struggle too much being ignorant to just be a doctor and dont get luxury
Thanks a lot! Very helpful :)
i watched so many of these damn chemistry videos!!! im starting to hate chemistry everyday!!!
best teacher
Beautiful. 👍
I understand him more than my teacher.
Can anyone tell me why I keep getting 1.91 x 10^24 every time I type it into my calculator?
Thank you so much!
how did he get 3.01 x10 to the power of 23??????
very helpful
If You Need Additional Help I will be Providing Links to NOTES on this Subject BELOW⬇
_
upload.ac/zryqj2ih0vmb
upload.ac/3zmzutzbjaib
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he go to dang fast
Thank you !
The answer is 0.1911111111x10^23 or simply equivalent to 2.0x10^22
Don't round to 2.0 x 10^22, just write it as 1.911 x 10^22
+Manujendra Dalei sig figs, boy.
Got it right, friend.