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To calculate the atomic mass of element A, we need to consider the masses and relative abundances of its isotopes.
Let's assume the first isotope has a mass of x and is present 18.48% of the time. The second isotope has a mass of 116.1 and is present (100 - 18.48)% = 81.52% of the time.
We can set up the following equation based on the weighted average:
(x * 18.48%) + (116.1 * 81.52%) = Atomic mass of element A
Simplifying the equation:
0.1848x + 95.02672 = Atomic mass of element A
To solve for x, we subtract 95.02672 from both sides:
0.1848x = Atomic mass of element A - 95.02672
Now, we substitute the mass value of the first isotope (135.24) for x:
0.1848(135.24) = Atomic mass of element A - 95.02672
24.99152 = Atomic mass of element A - 95.02672
To find the atomic mass of element A, we add 95.02672 to both sides:
Atomic mass of element A = 24.99152 + 95.02672
Atomic mass of element A = 120.01824
Therefore, the atomic mass of element A is approximately 120.018 (to 3 decimal places).
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