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An element has the following natural abundances and isotopic masses: 90.92% abundance with 19.99 amu, 0.26% abundance with 20.99 amu, and 8.82% abundance with 21.99 amu. Calculate the average atomic mass of this element
Average atomic mass is 20.15 amu
Chemistry 101
Chapter 2
Atoms, Molecules, and Ions
Atoms, Molecules and Ions
Drexel University
University of Toronto
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this question asked us to find the average atomic mass of an element given the natural abundances of its ice atopic masses. So the isotope, with a mass of 19.99 atomic mass units, has an abundance of 90.92%. That's right. Now's a decimal here. The isotopic, the mass of 20.99 atomic mass units, has an abundance of 0.26% in the institute, with the mass. 21.99 atomic mass units has an abundance of 8.82%. So to find the average atomic mass, we multiply each of the ice, a topic topic masses by their abundance. So 19.99 times 0.9092 is 18 17 in 20.99 times 0.26 is 0.5 and 21.99 times 0.0 82 is 1.94 Then, finally, to find the average, uh, time, ask you some these weighted averages we did that you can answer of 20 point 15 and units atomic mass units. I recommend that instead of doing each of these equations one by one like this and some of them that you do all three together in your calculator so you don't round in between steps of Ray to this final answer.
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