Avogadro's number

Moderators: Chem_Mod, Chem_Admin

alexis castro 1B
Posts: 30
Joined: Wed Nov 16, 2016 3:02 am

Avogadro's number

Postby alexis castro 1B » Thu Jun 29, 2017 7:45 pm

Can someone explain, in a more simple way than what the book did, how Avogadro found the number 6.022x10^23 and knew it was universal and could be applied to any element to convert it from moles to molecules.

Posts: 27
Joined: Tue Nov 15, 2016 3:00 am

Re: Avogadro's number

Postby Daniela_Chem14A » Fri Jun 30, 2017 3:01 pm

From what I understood, Avogrado's number was based on the idea that a single atom of the Carbon isotope Carbon-12 has a mass of 1.99265x10^-23g. And since a mole refers to a dozen of something in this case a dozen of grams of carbon which equals 12g of carbon. They used these 12g of carbon and divided them by the 1.99265x10^-23g of the carbon-12 isotope to get Avogrado's number which, equals 6.0221x10^23. Avogrado's number can be used universally because Avogrado's number equals 1 mole. So whenever moles are used, Avogrado's number can be use in order to convert to atoms, particles or molecules. Hope this helps!

Mia Navarro 1D
Posts: 52
Joined: Fri Sep 29, 2017 7:04 am

Re: Avogadro's number

Postby Mia Navarro 1D » Wed Oct 04, 2017 11:10 pm

To add a little more context if you were curious as to why they picked the element and quantities that they did, the decision was arbitrary. As Dr. Lavelle explained in a lecture earlier this week, the Avogadro's number could have depended on 10g of cobalt. Though, carbon is an easily obtainable element in nature, and the molar mass was a plausible quantity of the element that could be used for the experiment.

Hope this helps!

Mia Navarro

Return to “SI Units, Unit Conversions”

Who is online

Users browsing this forum: No registered users and 1 guest