Element Z has two naturally occurring isotopes. The isotope with a mass of 10.012 amu (10 Z) has a relative abundance of 19.91%. The isotope with amass of 11.009 amu (11Z) has a relative abundance of 80.09%. Calculate the average atomic mass of element Z.Be sure to type your work and round your answer to the correct number of significant figures.

Average atomic mass of element Z = 10.012 amu × 0.1991 + 11.009 amu × 0.8009 = 10.810 amu ≈ 10.81…

Element Z has two naturally occurring isotopes. The isotope with a mass of 10.012 amu (10Z) has a relative abundance of 19.91%. The isotope with a mass of 11.009 amu ("Z) has a relative abundance of 80.09%. Calculate the average atomic mass of element Z. Be sure to type your work and round your answer to the correct number of significant figures.

Element Z has two naturally occurring isotopes. The isotope with a mass of 10.012 amu (10Z) has a relative abundance of 19.91%. The isotope with a mass of 11.009 amu ("Z) has a relative abundance of 80.09%. Calculate the average atomic mass of element Z. Be sure to type your work and round your answer to the correct number of significant figures.

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU1: Alchemy: Matter, Atomic Structure, And Bonding

Section: Chapter Questions

Problem 11STP

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