**Problem 18:**The table below lists the naturally occurring isotopes of element X. Use this data to calculate the average atomic mass of element X. *(You must show your work!)*| Mass of Isotope (amu) | Isotopic Abundance (%) ||-----------------------|------------------------|| 15.33 | 28.6 || 17.26 | 13.3 || 18.11 | 58.1 |**Instructions:**1. The average atomic mass is calculated by multiplying the mass of each isotope by its relative abundance (percentage as a decimal), then summing these values. 2. Show each step of your calculation to ensure clarity and understanding.**Note:** This data will help to determine a more accurate representation of element X’s atomic mass as it appears in nature, considering the various isotopic forms it can take.

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18. The table shown below lists the naturally occurring isotopes of element X. Use this data to calculate the average at mic mass of element X. (You must show your work!!) D Mass of Isotope (amu) 15.33 17.26 18.11 Isotopic Abundance (%) 28.6 13.3 58.1

18. The table shown below lists the naturally occurring isotopes of element X. Use this data to calculate the average at mic mass of element X. (You must show your work!!) D Mass of Isotope (amu) 15.33 17.26 18.11 Isotopic Abundance (%) 28.6 13.3 58.1

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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