A hypothetical element has two main iso- topes. One has a mass of 35 amu and the other has a mass of 37 amu. If the atomic weight of this element is 35.55 amu, what is the percent abundance of the 37 amu isotope?
Let x = abundance of 35 and 1-x = abundance of 37.
Then 35x + 37(1-x) = 35.55
Solve for x and 1-x. and they will be a decimal. Multiply by 100 to convert to percent abundance. Post your work if you get stuck..
To find the percent abundance of the 37 amu isotope, we can set up an equation using the given information.
Let's assume that the percent abundance of the 35 amu isotope is x% (out of 100%). Since there are only two isotopes, the percent abundance of the 37 amu isotope would be (100% - x%).
The atomic weight is the weighted average of the isotopes, taking into account their masses and abundances. Therefore, we can set up the equation as follows:
(35 amu * x%) + (37 amu * (100% - x%)) = 35.55 amu
Now let's solve for x% to find the percent abundance of the 37 amu isotope.
35x + 37(100 - x) = 3555
35x + 3700 - 37x = 3555
-2x = -145
x = 72.5
The percent abundance of the 37 amu isotope is (100% - x%) = (100% - 72.5%) = 27.5%.