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A sample of element X contains 100 atoms with a mass of 12.0 unit and 10 atoms with a mass of 14.0 unit . Calculate average atomic mass of element X .?
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A sample of element X contains 100 atoms with a mass of 12.0 unit and ...
Introduction:
The average atomic mass of an element is the weighted average of the masses of all its isotopes. It is calculated by multiplying the mass of each isotope by its fractional abundance and then adding up the products.
Given:
- 100 atoms of X with a mass of 12.0 unit
- 10 atoms of X with a mass of 14.0 unit
Calculations:
1. Calculate the total mass of all atoms of X:
- (100 atoms of 12.0 unit) + (10 atoms of 14.0 unit) = 1240.0 unit
2. Calculate the fractional abundance of each isotope:
- Fractional abundance of 12.0 unit isotope = 100/(100+10) = 0.909
- Fractional abundance of 14.0 unit isotope = 10/(100+10) = 0.091
3. Calculate the contribution of each isotope to the total mass:
- Contribution of 12.0 unit isotope = (12.0 unit) x (0.909) x (100) = 1090.8 unit
- Contribution of 14.0 unit isotope = (14.0 unit) x (0.091) x (10) = 12.74 unit
4. Calculate the average atomic mass:
- Average atomic mass of element X = (1090.8 unit + 12.74 unit)/1240.0 unit = 0.8832 x 100 = 88.32 unit
Conclusion:
The average atomic mass of element X is 88.32 unit.
The average atomic mass of an element is the weighted average of the masses of all its isotopes. It is calculated by multiplying the mass of each isotope by its fractional abundance and then adding up the products.
Given:
- 100 atoms of X with a mass of 12.0 unit
- 10 atoms of X with a mass of 14.0 unit
Calculations:
1. Calculate the total mass of all atoms of X:
- (100 atoms of 12.0 unit) + (10 atoms of 14.0 unit) = 1240.0 unit
2. Calculate the fractional abundance of each isotope:
- Fractional abundance of 12.0 unit isotope = 100/(100+10) = 0.909
- Fractional abundance of 14.0 unit isotope = 10/(100+10) = 0.091
3. Calculate the contribution of each isotope to the total mass:
- Contribution of 12.0 unit isotope = (12.0 unit) x (0.909) x (100) = 1090.8 unit
- Contribution of 14.0 unit isotope = (14.0 unit) x (0.091) x (10) = 12.74 unit
4. Calculate the average atomic mass:
- Average atomic mass of element X = (1090.8 unit + 12.74 unit)/1240.0 unit = 0.8832 x 100 = 88.32 unit
Conclusion:
The average atomic mass of element X is 88.32 unit.
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A sample of element X contains 100 atoms with a mass of 12.0 unit and 10 atoms with a mass of 14.0 unit . Calculate average atomic mass of element X .?
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A sample of element X contains 100 atoms with a mass of 12.0 unit and 10 atoms with a mass of 14.0 unit . Calculate average atomic mass of element X .? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about A sample of element X contains 100 atoms with a mass of 12.0 unit and 10 atoms with a mass of 14.0 unit . Calculate average atomic mass of element X .? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A sample of element X contains 100 atoms with a mass of 12.0 unit and 10 atoms with a mass of 14.0 unit . Calculate average atomic mass of element X .?.
A sample of element X contains 100 atoms with a mass of 12.0 unit and 10 atoms with a mass of 14.0 unit . Calculate average atomic mass of element X .? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about A sample of element X contains 100 atoms with a mass of 12.0 unit and 10 atoms with a mass of 14.0 unit . Calculate average atomic mass of element X .? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A sample of element X contains 100 atoms with a mass of 12.0 unit and 10 atoms with a mass of 14.0 unit . Calculate average atomic mass of element X .?.
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