The atomic mass is the weighted average of the atomic masses of each isotope. In a weighted average, we multiply each value by a number representing its relative importance. In...
1 Answers 1 viewsThe 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 views$""^63Cu$ has $69.2%$ abundance. $""^65Cu$ has $30.8%$ abundance. So, the weighted average is $62.93xx69.2%$ $+$ $64.93xx30.8%$ $=$ $63.55$ $"amu"$. If we look at , copper metal (a mixture of isotopes...
1 Answers 1 viewsThe average of an element is determined by taking the weighted average of the atomic masses of its naturally occurring . Now, weighted average simply means that each...
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 viewsNow I hope you have been exposed to the concept of weighted average; If not here is a video Now lets get our data; Lets call our element...
1 Answers 1 viewsAnd thus the $"weighted average"$ is: $(62.93xx69.2%+64.93xx30.8%)*"amu"$ $=$ $63.55$ $"amu"$
1 Answers 1 viewsLet the percentage of the isotope $""^71Ga$ be $=x%$ Then, The percentage of the isotope $""^69Ga$ is $=(100-x)%$ We write the mass balance equation $100*69.72=x*71+(100-x)*69$ $6972=71x+6900-69x$ $2x=6972-6900=72$ $x=36$ Therefore, The...
1 Answers 1 views$"Average atomic mass"={18.473_"X"xx28.812%+19.962_"Y"xx 28.757% +21.469_"Z" xx(100-28.812-28.757)%}*"amu"$ $-=20.15*"amu"$...if I have done my 'rithmetic right... How did I get the percentage abundance of $Z$? And it is likely that we got the...
1 Answers 1 views