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A certain element consists of two stable isotopes.

The first has an atomic mass of 7.0160 amu and a percent natural abundance of 92.58%.

The second has an atomic mass of 6.0150 amu and a percent natural abundance of 7.42%.

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To determine the atomic mass of the element, one can use the following formula: Atomic mass = (Mass of isotope 1 × % natural abundance of isotope 1) + (Mass of isotope 2 × % natural abundance of isotope 2). This particular element is composed of two stable isotopes. The first isotope has an atomic mass of 7.0160 amu% and a natural abundance of 92.58%, while the second isotope has an atomic mass of 6.0150 amu% and a natural abundance of 7.42%. By substituting these values into the formula, we arrive at an atomic mass of 6.936442 amu.

User Vinesh Chauhan
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