### Problem StatementA mystery element has two main isotopes of 62.9300 amu and 64.928 amu. Their percent abundances are 69.15% and 30.85%, respectively. What is the average atomic mass of the element?### Multiple Choice Options- ☐ 64.31 amu- ☐ 63.55 amu- ☐ 63.93 amu- ☐ 65.38 amu### ExplanationTo determine the average atomic mass of the element, we will use the formula for the weighted average based on the abundances of its isotopes.#### Steps:1. Convert the percent abundances into decimal form: - Isotope 1: 69.15% = 0.6915 - Isotope 2: 30.85% = 0.30852. Multiply the atomic mass of each isotope by its corresponding decimal abundance: - Isotope 1: 62.9300 amu * 0.6915 - Isotope 2: 64.9280 amu * 0.30853. Compute the products: - Isotope 1: 62.9300 * 0.6915 ≈ 43.514 - Isotope 2: 64.9280 * 0.3085 ≈ 20.0304. Add the two results together to get the average atomic mass: - Average atomic mass = 43.514 + 20.030 ≈ 63.544### Correct Answer- ☐ 63.55 amu

The isotopes are the elements having same atomic number but different mass number.

A mystery element has two main isotopes of 62.9300amu and 64.928amu. Their percent abundances are 69.15% and 30.85%, respectively. What is the average atomic mass of the element? O 64.31amu O 63.55amu O 63.93amu O 65.38amu

A mystery element has two main isotopes of 62.9300amu and 64.928amu. Their percent abundances are 69.15% and 30.85%, respectively. What is the average atomic mass of the element? O 64.31amu O 63.55amu O 63.93amu O 65.38amu

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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Concept explainers

Atoms and Molecules

An atom is the smallest unit of an element that possesses all the properties of that particular element. Molecules are the smallest unit of a substance that possess all the properties of that particular substance.

Question

### Problem Statement

A mystery element has two main isotopes of 62.9300 amu and 64.928 amu. Their percent abundances are 69.15% and 30.85%, respectively. What is the average atomic mass of the element?

### Multiple Choice Options

- ☐ 64.31 amu
- ☐ 63.55 amu
- ☐ 63.93 amu
- ☐ 65.38 amu

### Explanation

To determine the average atomic mass of the element, we will use the formula for the weighted average based on the abundances of its isotopes.

#### Steps:
1. Convert the percent abundances into decimal form:
- Isotope 1: 69.15% = 0.6915
- Isotope 2: 30.85% = 0.3085

2. Multiply the atomic mass of each isotope by its corresponding decimal abundance:
- Isotope 1: 62.9300 amu * 0.6915
- Isotope 2: 64.9280 amu * 0.3085

3. Compute the products:
- Isotope 1: 62.9300 * 0.6915 ≈ 43.514
- Isotope 2: 64.9280 * 0.3085 ≈ 20.030

4. Add the two results together to get the average atomic mass:
- Average atomic mass = 43.514 + 20.030 ≈ 63.544

### Correct Answer
- ☐ 63.55 amu

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