Asked by Rose
Naturally occurring copper is a mixture of two isotopes. One of these has 34 neutrons the other has 36. If the relative atomic mass of copper is 63.55 amu calculate the natural abundances (percentages ) of the two isotopes.
Answers
Answered by
DrBob222
Let X = fraction Cu63
and 1-X = fraction Cu65
---------------------
X*63 + (1-X)*65 = 63.55
Solve for X and 1-X and convert each from fraction to percent.
and 1-X = fraction Cu65
---------------------
X*63 + (1-X)*65 = 63.55
Solve for X and 1-X and convert each from fraction to percent.
Answered by
Anonymous
34x +36-36x --63.55
Answered by
Enock
235_
Answered by
felix
naturall occuring copper consist of two stable isotops 63/29 cu and 65/29.
There are no AI answers yet. The ability to request AI answers is coming soon!