Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass number of 22.0 is 65.0% abundant; the isotope with a mass number of 24.0 is 35.0% abundant. What is the average atomic mass for element Z? *
19.9 amu
22.7 amu
23.3 amu
23 amu
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Answer:
22.7 amu
Explanation:
Average mass of Z = (22×65+24×35)/100
=2270/100
=22.7 amu
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