Question

If an element has three isotopes with masses of 10.00 amu, 12.00 amu, and 16.00 amu with respective abundances of 10.00% , 60.00%, and 30.00% what is the average atomic mass of the element?

Answer 1

The average atomic mass of the element is 13 amu

The average atomic mass of an element

The average atomic mass of an element is the sum of the all the relative abundance and isotopic mass of each isotope of the element.

• Average atomic mass = sum of isotopic mass × relative abundance of all isotopes

Average atomic mass of the element

From the data provided:

Isotopic masses of 10.00 amu, 12.00 amu, and 16.00 amu with respective abundances of 10.00% , 60.00%, and 30.00%

Average atomic mass of the element = 10 × 0.1 + 12 × 0.6 + 16 × 0.3

Average atomic mass of the element = 13 amu

Therefore, the average atomic mass of the element is 13 amu.

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Answer 2

The average atomic mass of the element with masses of 10.00 amu, 12.00 amu, and 16.00 amu with respective abundances of 10.00% , 60.00%, and 30.00% is 13.

HOW TO CALCULATE AVERAGE ATOMIC MASS:

• The average atomic mass of an isotope can be calculated as follows:

• According to this question, an element has three isotopes with the following masses and percentage abundance:

1. 10.00 amu - 10%
2. 12.00 amu - 60%
3. 16.00 amu - 30%

• The mass of each isotope in the element is as follows:

1. 10/100 × 10 = 1
2. 60/100 × 12 = 7.2
3. 30/100 × 16 = 4.8

Next, we find the sum of each value as: 1 + 7.2 + 4.8 = 13.

Therefore, the average atomic mass of the element with masses of 10.00 amu, 12.00 amu, and 16.00 amu with respective abundances of 10.00% , 60.00%, and 30.00% is 13.

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