What is the relative atomic mass of a hypothetical element that consists of the following isotopes in the indicated natural abundances? Isotope Isotopic mass Relative abundance (amu) 77.9 81.9 85.9 1 2 3 (%) 13.3 12.0 74.7 Express your answer to three significant figures and include the appropriate units.
What is the relative atomic mass of a hypothetical element that consists of the following isotopes in the indicated natural abundances? Isotope Isotopic mass Relative abundance (amu) 77.9 81.9 85.9 1 2 3 (%) 13.3 12.0 74.7 Express your answer to three significant figures and include the appropriate units.
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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Transcribed Image Text:**Topic: Calculating Relative Atomic Mass**
**Problem Statement:**
What is the relative atomic mass of a hypothetical element that consists of the following isotopes in the indicated natural abundances?
**Isotope Data:**
- **Isotope 1**
- Isotopic mass: 77.9 amu
- Relative abundance: 13.3%
- **Isotope 2**
- Isotopic mass: 81.9 amu
- Relative abundance: 12.0%
- **Isotope 3**
- Isotopic mass: 85.9 amu
- Relative abundance: 74.7%
**Instructions:**
Express your answer to three significant figures and include the appropriate units.
**Hints Available:**
- **Hint 1:** How to approach the problem
- **Hint 2:** Determine the mass contribution of the first isotope
- **Hint 3:** Determine the mass contribution of the second isotope
- **Hint 4:** Determine the mass contribution of the third isotope
**Input Field:**
- Enter the calculated value and units.
**Diagram Explanation:**
The diagram presents a table with isotope data, including isotopic masses and their relative abundances. Use this data to calculate the element's relative atomic mass by multiplying each isotope's mass by its abundance, summing the results, and dividing by 100 to account for percentage.
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