The atomic weight of the element is 6.9408 amu.
The relative abundance of an isotope is defined as the percentage of atoms of a specific atomic mass that can be found in a naturally occurring sample of an element.
The atomic mass of the first isotope is 7.0150 amu.
The abundance of the first isotope is 92.58 %.
The atomic mass of the second isotope is 6.0150 amu.
The abundance of the second isotope is 7.42 %.
Now, abundance₁ = 92.58 % = = ( 92.58/ 100) = 0.9258
abundance₂ = 7.42 % = (7.42 / 100 ) = 0.0742
Therefore, the average atomic weight is:
Atomic mass = mass₁ × abundance₁ + mass₂ × abundance₂
Atomic mass = (7.0150) × (0.9258) + (6.0150) × (0.0742) amu
Atomic mass = 6.494487 + 0.446313 amu
Atomic mass = 6.9408 amu
The element's atomic weight is 6.9408 amu.
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