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A Chemistry student at Agora is calculating the average atomic mass of Potassium using the following data. Relative abundance 93-12 % 6.88% Isotope K-39 K-41 Their setup and calculation are. Atomic Mass 38.964 amu 40.962 amu Mass (amu) X Relative Abundance (% divide by 100) 38.964 40.962 0.0688 0.9312 = 2.681 = 38.144 40.823 amu The student calculated the average atomic mass to be 40.823 amu but it is 39.098 amu on the periodic table. What did the student do incorrectly? Use CER!

A Chemistry student at Agora is calculating the average atomic mass of Potassium using the following data. Relative abundance 93-12 % 6.88% Isotope K-39 K-41 Their setup and calculation are. Atomic Mass 38.964 amu 40.962 amu Mass (amu) X Relative Abundance (% divide by 100) 38.964 40.962 0.0688 0.9312 = 2.681 = 38.144 40.823 amu The student calculated the average atomic mass to be 40.823 amu but it is 39.098 amu on the periodic table. What did the student do incorrectly? Use CER!

Chemistry
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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A Chemistry student at Agora is calculating the average atomic mass of Potassium using the following data. Relative abundance 93-12 % 6.88 % Isotope K-39 K-41 Their setup and calculation are. Atomic Mass 38.964 amu 40.962 amu Mass (amu) X Relative Abundance (% divide by 100) 38.964 40.962 0.0688 0.9312 = 2.681 = 38.144 40.823 amu The student calculated the average atomic mass to be 40.823 amu but it is 39.098 amu on the periodic table. What did the student do incorrectly? Use CER!
Transcribed Image Text:A Chemistry student at Agora is calculating the average atomic mass of Potassium using the following data. Relative abundance 93-12 % 6.88 % Isotope K-39 K-41 Their setup and calculation are. Atomic Mass 38.964 amu 40.962 amu Mass (amu) X Relative Abundance (% divide by 100) 38.964 40.962 0.0688 0.9312 = 2.681 = 38.144 40.823 amu The student calculated the average atomic mass to be 40.823 amu but it is 39.098 amu on the periodic table. What did the student do incorrectly? Use CER!
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