A Chemistry student at Agora is calculating the average atomic mass of Potassium using the following data. Isotope K-39 K-41 Relative abundance 93.12 % 6.88 % Their setup and calculation are. Mass (amu) 38.964 40.962 X Atomic Mass 38.964 amu 40.962 amu Relative Abundance (% divide by 100) 0.0688 What did the student do incorrectly? Use CER! 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.
A Chemistry student at Agora is calculating the average atomic mass of Potassium using the following data. Isotope K-39 K-41 Relative abundance 93.12 % 6.88 % Their setup and calculation are. Mass (amu) 38.964 40.962 X Atomic Mass 38.964 amu 40.962 amu Relative Abundance (% divide by 100) 0.0688 What did the student do incorrectly? Use CER! 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.
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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What did the student do incorrectly?
Transcribed Image Text:### Calculating the Average Atomic Mass of Potassium
A Chemistry student at Agora is calculating the average atomic mass of Potassium using the following data:
| Isotope | Relative Abundance | Atomic Mass |
|---------|--------------------|-------------|
| K-39 | 93.12% | 38.964 amu |
| K-41 | 6.88% | 40.962 amu |
Their setup and calculations are:
| Mass (amu) | X | Relative Abundance (% divided by 100) | Product |
|------------|---|--------------------------------------|---------|
| 38.964 | | 0.0688 | 2.681 |
| 40.962 | | 0.9312 | 38.144 |
| **Total** | | | **40.823 amu** |
The student calculated the average atomic mass to be 40.823 amu, but it is actually 39.098 amu according to the periodic table.
**Question:**
What did the student do incorrectly? Use Claim-Evidence-Reasoning (CER).
**Analysis:**
The student's calculated average atomic mass is significantly higher than the accepted value. Upon reviewing the multiplication for the isotopic contributions, it appears there might have been a mix-up between the respective relative abundances and mass contributions, leading to an incorrect result. To reach an accurate calculation, ensure each isotope's mass is accurately weighted by its relative abundance, and re-calculate using a correct application of the weighted average formula.
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