I can't lie. I thought this was crazy cheesy at first. This was one of my last-ditch attempts to figure this out, everything including khan academy made almost no sense. My teacher sure wasn't helping, but this actually helped me completely understand. Thank you so much Mr. Causey, even though it was a little cheesy it really helped me out.
Thank you so much for this video!! It was so helpful. I just started online school due to COVID-19 and I was not understanding the material trying to be taught online. You are awesome thank you!
I never understood this from junior high to senior high. Now that I'm in college, I got it because of this vid. Really needed this vid to review my brain for physics. Thank you!
Great sir...I was unable to understand...I have watched many videos...then I googled for this topic...and ur name was on the top...I have understood everything 👍....u rocked
I've been somewhat behind in chemistry, but this video synthesized mutiple chapters of my textbook into 10 minutes in a much easier to understand format. Thank you very much! I hope you get as much out of this as I do, because this was really helpful.
youve heard of studying the night before the test, but have you heard of missing the day it was explained then ditching school the day of the test to learn the entire concept
Thank you Mr. Causey! This is a great thing you're doing for all of us who utilize this site you've created. I'm taking a condensed summer Chem 150 course, and struggling. My professor is great, but the class goes quickly since it has to cover so much material in a short period of time. Thank you though! This is a great help...
Mr. Causey, this video helped me a lot, I could not understand about mole concept before I had watched this video, it is really amazing😁😁😁 thanks a bunch!
Success!! I finally understand the mole!! Mr. Causey, thank you so so sooo much! You make chemistry easy and understandable! I think i am actually going to pass my final on Thursday due to your videos:)
I was first taught this in my junior year of high school, then I was taught this again in my general chem class at college. I was expected to use it in my O-chem, biochem and P-chem classes. It is an important concept for stoichiometry.
Damn!! I took a test on this very stuff and failed it because I kept using 6.002*E23 when I did not have too use it!! man I wish u posted this last week, I may have aced the exam
The original calculation for the atomic mass was based on a ratio therefore you can just take the atomic mass and add grams for a mole of that substance. 1.01 grams H is one mole H.
who is making the claim that there a specific number of atoms for every 12 grams of _ name of substance that is = to some number of moles please do provide the referenced publications for how that authority figure obtained there conclusion thankyou very much have a nice day!
No one is making a claim as you have stated it. The claim is that is a specific number of atoms in 12 grams of carbon. All the other elements and compounds have the same number of particles but with a different mass. Since it was determined that carbon is 12 times more massive than hydrogen, hydrogen has the same number (mole) of particles in 1.008 grams. As far as supplying referenced publications this is a concept that began in the 1800s and can be found in most chemistry books.
Very helpful video, but I have a question. On the last problem, you say that there is no way to go directly from grams to particles, but in this example I paused the video before you set it up and worked it on my own. I set it up as: 5.21gS x (6.022x10^23 / 32.07gS) and got the correct answer. Is there a reason why I shouldn't do this every time? I'm just curious. Thanks again for the great video!
When you illustrate something with a picture that contradicts what you say - you're trying hard to confuse countless learners. The periodic table you showed said Oxygen was 15.999 but you glibly said it was "sixteen point zero zero zero". A screaming contradiction which came and went without a single murmur.
No it's not. In order to use the number that is on the periodic table you have to round it off which makes it 16.00 g/mol or 16.00 amu. This is a very standard value for oxyben. It is also very common to use 1.01 for H and 12.01 for C. It is very important to be flexible in chemistry, biology and physics because there just aren't any absolutes in science.
Sorry but when the picture says "15.999" and the narrative says "16.000" it absolutely *IS* a contradiction, and many will notice and be baffled by it. People come here to learn from you, so you can't expect them to know that what you are saying is an approximation ignoring isotopic ratios whereas what you are showing is not ignoring them.
Again, no it is not The periodic table I used has 15.999 which is 16.00. I did not say three zeroes nor did I write three zeroes. But more importantly this video is about understanding the mole and you are hung up on minutia. Sorry but you are wrong.
OK maybe I'm wrong and thank you for you're patience with me, and for not deleting my comment. Please explain what you mean when you say (above) "I used 15.999 which is 16.00". In my world "15.999 is 15.999 and it is 16.00 is not. Of course the numerical difference is trivial, but that's not the point. The point is that you say one thing and show another thing without ever acknowledging that those things are not the same thing.
When 15.999 is rounded off to the 1/100 place it will be 16.00 which is a standard scientific/mathematical practice. In most intro to chemistry classes the best significant figures anyone is going to get is going to be the 1/100 place. It is quite common to round the atomic masses to the 1/100 place. Some will even round to the units place.
I can't wrap my head around the mole! I can't understand my teacher at all. Its not her fault, but it doesn't register with me! I went in 4 times for private tutoring, but to no avail! I tried taking the textbook and working through problems. I've watched countless videos, and I still don't get it!
