Mr. Causey I want you to know that even though I have been struggling with my chemistry class all semester your videos have helped me so much. You have videos for each section of my basic chemistry class. What is difficult to learn in class you have made so easy and obvious and for that I want to thank you. I have given your information to my lab partner who has been struggling, also. I am sure that we will be more confident for our next and last test prior to our final. The test will be on Avogadro's number, empirical formulas, mole ratio. Anything and everything from our textbook chapter 6 & 8 Chemical quantities and Chemical quantities in Reactions. From:The Pearson Custom Library for Chemistry MCC: Basic Chemistry: CHM 010 Fall 2013 Timberlake/Sherman. Our final will be cumulative. I know where I will be in preparation for both exams. Thanks again.
It depends on your teacher. I use the numbers to the .01 place value some like three decimal places. As far as learning chemistry it doesn't matter. The three most common values for hydrogen: 1.0; 1.01; 1.008
So when i have to find the mass of some liquid of lets say 100 ml then i have to divide the molecular wt. of the liquid by 22.4 and multiply it by 0.1??
No. The 1.01 amu is hydrogen. The atomic masses on the periodic table have already been determined and you can use that same number for the molar mass just change the units to grams.
Question #1: Mr. Causey, so any atomic mass unit that is multiplied with 6.022*10^23 is the atomic mass unit of the atom with grams, right? Question #2: Can you show me how to solve for how many breaths it will take to burn the energy from a particular amount of sucrose in grams?
Urwa Fatema Veerji moles of an element times Avogadro's number is atoms moles of a covalent compound times Avogadro's number is molecules moles of an ionic compound times Avogadro's number is formula units
+Farhan Awan First notice that the formula tells you there is 1 mol H to 3 mol O. .5 g H /1.01 g H = .495 mol H .495 mol H x 3 mol O = 1.49 mol O 1.49 mol O x 16.0 g O = 23.84 g O
I don't get it. 12amu C is equal to 1amu H then 1 g = to 1 amu...so C12 is equal to 12 grams but 1 MOLE of C12 is equal to 6.022X10^23?? is not supposes to be 1 C equal to 1 MOLE then 1 MOLE of C12 will be equal to 12*Avogadro number ?
Do you use the microphone on your computer or an external one? Also, what program do you use to create the videos you make? They are great! I am just starting out in creating online courses :)
Thank you so much its so easy to get now :D But I was just wondering, how did avodgadroo actually conclude the number of 6.002x 10 to the 23? Thanks :D
this person needs to provide you more information and direct references regarding the original publications for the statements that are being mentioned in the video very frustrating i know
Remember chlorine is diatomic Cl2, so you have to to double the mass - 70.90 grams per mole. Now divide 350 by 70.90 to get the moles. Then multiply by 6.022 x 10^23
you know what here's what i don't understand how come the original person who name these concepts don't teach it themselves let alone leave it up to someone else to do the job
Well, not just one person is responsible for the development of the mole concept and Avogadro's number. It developed like most scientific concepts over several years with contributions from many people. The mole is just a representation of a number like a dozen is a representation of a number. However, using the for stoichiometry makes calculations easier and more manageable. BTW all the people involved in the beginning are dead.
No, the atomic mass in grams is one mole of that substance thus the molar mass. Remember, hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine and iodine are diatomic elements.
