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.
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.
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.
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.
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.
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!
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.
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
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.
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.
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
+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
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!
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
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.
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.
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
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.
This really helps for a year 11 student studying chemistry. Keep up the good work.
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
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.
Burn under water? Well now we know how sponge bob can have a campfire :P
Angelica Porro yeah right
Wow, these 7 minutes have been a lot of help! THANK YOU!
Someone get this guy a Nobel prize!
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.
Thank you or this! You explain it better than my teacher does.
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?
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 so much for these videos! They do help out a great deal in understanding everything
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!
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.
yap thanks a lot it really helped me and i got 96 percent on mole test
You just explained something that I was confused about for 11 years :P
Extremely helpful. In seven minutes explained what took my teacher 2 hours.
You have provided a awesome explanation
Thank you alot
Did the question. Got it right = 1.91 x 10^22 . Feeling super smart. Thanks Man!
Yes, it was a huge help. These videos mean a lot to me, thanks man!
This was helpful, now I know something lots of sophomores don't!
Oh My God If Only You Were My Chem Teacher!!!! Thank You.... Very Helpful
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.
Thank you, Mr. Anderson!
At 3:46, u said that "1 mole of C02 is 30.01 grams". It should be NO instead of CO2.. typo :)
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 😁
U reli awsme bozemann i being a indian lyks to watch ur videos which i understnd very easily
Outstanding video. Thank you.
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.
Mr Anderson, thanks for the videos! Very helpful
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!
Thank you for this video. Much appreciated and can't wait to see more from you!
Great Video, it was extremely helpful and comprehensive
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??
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."
The basic question that needs to be answered is how did Avogadro counted the number particles?
Better than Khan Academy. Way more organized and to the point.
This video is very helpful thankyou!!!!
Great help!! Thank you sir!!
Thank you for this awesome vid
Great video. Thanks for sharing!
Helpful as always
thanks! I'm a PhD in chemistry and needed a refresher/s
That pretty much helped but is it that for finding the atoms, particles, molecules and formula units, Avogadro's number has to be used?
i calculated the answer is 2.03x 10^22, and is that wrong?
i rounded up to 3.01
but idk maybe ur right
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
thank u so much :D i love the way you explain things about science
thank you very much, i needed this
The Math here is confusing. You somewhat glanced over the RATIOS.
Mr. Bozeman, you rock.
Awesome tutorial. Thx mate
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.
6 years later
So if I'm asked
"What is The Mole?" In an exam, what do i have to write?
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.
how does carbon 12 have 12.01 amu if 1 amu = carbon 12/12?
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.
Well explained ...got that in the first time
IT IS 6.02*10 THE POWER OF 23 AND IT IS LIKE A BRIDGE BETWEEN MASS AND PARTICLES.
You gained a new sub, thank you.
Thanks heaps! i finally understand this concept :)
You may need to fix typo at the 3:49 minute mark. Otherwise, very 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
Right, the big hurdle a lot of students struggle with is that amu = g/mol
this dude can teach
Massive understatement!
i just wonder how your mind can gather all these sciences
i watched so many of these damn chemistry videos!!! im starting to hate chemistry everyday!!!
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
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!
Thanks for the help, you could have explained how to calculate the mol a little better.
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 a lot! Very helpful :)
best teacher
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
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.
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.
Missed opportunity at 2:10 to use a mole of moles for you explanation.
I love you. You are my saving grace :)
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.
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
Thank you so much!
Oh, never mind, the word NITROUS OXIDE flashed across the screen. :)
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.
Thank you !
he go to dang fast
Wait, this video says 1 mole of CO2 is 30.01 grams after Mr. Anderson explained NO being 30.01 amu?
Why are we dividing in h2o example
Beautiful. 👍
3:46 it is nitric oxide
Can anyone tell me why I keep getting 1.91 x 10^24 every time I type it into my calculator?
*Nitric Oxide @3:49
Got it right, friend.
Thanks!
Thank you!!
very helpful
You're awsome! thank you!
I understand him more than my teacher.
did you divide the 18.02 and 6.02 to the nearest of what? ASAP
Can the answer be 0.19 times 10 to the 23