What is the mass of #6xx10^22# #"zinc atoms"#?

1 Answer
Jun 8, 2017

Answer:

Well, we use the molar quantity, #N_A=6.022xx10^23*mol^-1#, and gets approx. a mass of #6.5*g#.

Explanation:

We know that #N_A# #"zinc atoms"#, i.e. #6.022xx10^23# individual zinc atoms, have a mass of #65.39*g# precisely. How do we know this? Well, because we has access to a Periodic Table, and this EXPLICITLY tells us the mass of a molar quantity.

And so we simply have to take the equivalent mass of zinc metal, i.e. #(6xx10^22*"zinc atoms")/(6.022xx10^23*"zinc atoms"*mol^-1)xx65.38*g*mol^-1=??g#.

Capisce? This is a very important concept to master in the study of chemistry.