
#1
Sep2408, 07:27 PM

P: 2

1. The problem statement, all variables and given/known data
Oxygen has 3 isotopes. Oxygen16 has the amu of 15.995 and its natural percent abundance is 99.759. Oxygen17 has a mass of 16.995 amu and its natural percent abundance is 0.037. Oxygen18 has a mass of 17.999 amu and its natural percent abundance is 0.204. What is the average atomic mass of oxygen? 2. Relevant equations I think I forgot these... 3. The attempt at a solution I couldn't remember what the process is supposed to look like to figure this sort of problem out, so I tried to multiply the mass by the percent abundance, but the answers made very little sense. If somebody could help me figure out where I messed up, PLEASE RESPOND! 



#2
Sep2408, 08:00 PM

HW Helper
P: 2,692

The average atomic mass of an element is much like a simple mixture problem that you learn in first year Algebra such that you can resort directly to percentage contributions formula.
AverageAMU = 0.99759*16 + 0.00037*17 + 0.00204*18 



#3
Sep2408, 09:19 PM

P: 2

Thank you so much!



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