We can use our percentage to find it as:
Percentage represents a fraction of
if in
i.e.
rearranging:
The idea here is that each isotope will contribute to the average of the element proportionally to their respective abundance. Now, the key to this problem lies in how you...
1 Answers 1 viewsThe idea with that have two naturally occurring is that the percent abundances of those two must add up to give $100%$. In calculations, it is often easier to...
1 Answers 1 viewsThe mass of Argon on is 39.948. The periodic table's is the AVERAGE weight of ALL its . If one isotope is MORE abundant than the others, the average will...
1 Answers 1 views$M_r=(sum(M_ia))/a$, where: $M_r$ = relative attomic mass ($g$ $mol^-1$) $M_i$ = mass of each isotope ($g$ $mol^-1$) $a$ = abundance, either given as a percent or amount of $g$...
1 Answers 1 viewsThe mass of antimony's second naturally occurring is $"122.902 u"$ The thing to know when doing isotope abundance problems is that the abundances of the two must add up to...
1 Answers 1 viewsSo, $10.600 (mass$ $units) = 70%xx10.000 + 30%xxM_2;$ where $M_2$ is the isoptopic mass of the other isotope. So solve for $M_2$! A priori would you expect $M_2$ to...
1 Answers 1 viewsBackground Info Most elements have different isotopes, or atoms with the same number of protons, but different numbers of neutrons. Hence, it is possible to have two atoms that are...
1 Answers 1 viewsThe average isotopic mass is the weighted average of the mass of the individual . Because the quoted average, $63.6$ $"amu"$, is closer to $""^63A$ than $""^65A$, the $""^63A$...
1 Answers 1 viewsIn each 100 $mol$ of Sb you have: $57.21$ mol of $ _ ^(121)Sb$ and $100-57.21=42.79 mol$ of $ _ ^(123)Sb$ Assuming the mass of the isotopes is integer (they...
1 Answers 1 viewsWe are given that $Z_"uranium"=92$...because this is the number of protons, massive, positively charged particles present ion the uranium nucleus. $Z="the atomic number"$ and it DEFINES the identity of the...
1 Answers 1 views