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Answer :
To find the average atomic mass of the element, you will follow these steps:
1. Understand the Data Provided:
You have different isotopes of an element with their masses and natural abundances given. The data provided indicates:
- Mass of first isotope = 39.0 amu with an abundance of 93.258%
- Mass of second isotope = 40.0 amu with an abundance of 0.012%
- Mass of third isotope = 41.0 amu with an abundance of 6.730%
2. Convert Percentages to Decimals:
To use the abundances in calculations, you should first convert them from percentages to decimals:
- 93.258% becomes 0.93258
- 0.012% becomes 0.00012
- 6.730% becomes 0.0673
3. Calculate the Average Atomic Mass:
The average atomic mass is calculated by multiplying each isotope's mass by its abundance and then adding up these values. This looks like:
[tex]\[
\text{Average atomic mass} = (39.0 \times 0.93258) + (40.0 \times 0.00012) + (41.0 \times 0.0673)
\][/tex]
4. Perform the Calculations:
- [tex]\( 39.0 \times 0.93258 = 36.38462 \)[/tex]
- [tex]\( 40.0 \times 0.00012 = 0.0048 \)[/tex]
- [tex]\( 41.0 \times 0.0673 = 2.7593 \)[/tex]
5. Add the Products Together:
[tex]\[
36.38462 + 0.0048 + 2.7593 = 39.13472
\][/tex]
6. Round to an Appropriate Number of Decimal Places:
Thus, the average atomic mass of the element is approximately 39.1 amu.
In conclusion, the correct answer is 39.1 amu.
1. Understand the Data Provided:
You have different isotopes of an element with their masses and natural abundances given. The data provided indicates:
- Mass of first isotope = 39.0 amu with an abundance of 93.258%
- Mass of second isotope = 40.0 amu with an abundance of 0.012%
- Mass of third isotope = 41.0 amu with an abundance of 6.730%
2. Convert Percentages to Decimals:
To use the abundances in calculations, you should first convert them from percentages to decimals:
- 93.258% becomes 0.93258
- 0.012% becomes 0.00012
- 6.730% becomes 0.0673
3. Calculate the Average Atomic Mass:
The average atomic mass is calculated by multiplying each isotope's mass by its abundance and then adding up these values. This looks like:
[tex]\[
\text{Average atomic mass} = (39.0 \times 0.93258) + (40.0 \times 0.00012) + (41.0 \times 0.0673)
\][/tex]
4. Perform the Calculations:
- [tex]\( 39.0 \times 0.93258 = 36.38462 \)[/tex]
- [tex]\( 40.0 \times 0.00012 = 0.0048 \)[/tex]
- [tex]\( 41.0 \times 0.0673 = 2.7593 \)[/tex]
5. Add the Products Together:
[tex]\[
36.38462 + 0.0048 + 2.7593 = 39.13472
\][/tex]
6. Round to an Appropriate Number of Decimal Places:
Thus, the average atomic mass of the element is approximately 39.1 amu.
In conclusion, the correct answer is 39.1 amu.
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