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anonymous
 4 years ago
Help please!
Gallium has two naturally occurring isotopes (Ga69 and Ga71) and has an atomic mass of 69.723 amu. The mass of Ga71 is 70.925 amu, and its natural abundance is 39.892%. Calculate the atomic mass (in amu) and natural abundance (in %) of the second isotope.
anonymous
 4 years ago
Help please! Gallium has two naturally occurring isotopes (Ga69 and Ga71) and has an atomic mass of 69.723 amu. The mass of Ga71 is 70.925 amu, and its natural abundance is 39.892%. Calculate the atomic mass (in amu) and natural abundance (in %) of the second isotope.

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anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0(atomic weight of one isotope)(x) + (atomic weight of other isotope)(1x) = the atomic mass Use algebra to find x. Don't forget to use the distributive property. Example: Cl35 weighs 34.969 amu Cl37 weighs 36.966 amu (34.969)(x) + (36.966)(1x) = 35.453 (on the table for Chlorine) 34.969 x + 36.966  36.966 x = 35.453 1.997 x = 1.513 x = 0.75764 so Cl35 abundance is 75.764% and Cl37 is 24.236 %

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0hold on..i am trying to process what you wrote ha

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0hmm this is actually kinda of confusing for me..I'll show you how I did it. 60.108% Ga69 : 0.60108 x ______amu= 39.892 % Ga71: 0.39892x 70.925 amu= 28.293 amu 10039.892 = 60.1085% Ga69 69.72328.293 = 41.4796 am Ga69 Is this correct?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0still wait lemme check

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Some of my classmates divide the 41.4796 by 0.60108? are they correct for doing that

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0hmm yeah me too...okay thanks!
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