Question

what is the relative atomic mass of the element that consists of the following isotopes in the indicated natural abundances?

isotope	isotopic mass (amu)	relative abundance (%)
2	59.93	26.16
3	60.93	1.25
4	61.93	3.66
5	63.93	1.16

express your answer to three significant figures and include the appropriate units.
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Explanation:

Step1: Calculate contribution of Isotope 1

Multiply isotopic mass by relative abundance (converted to decimal).
$57.93 \times \frac{67.76}{100} = 57.93 \times 0.6776 \approx 39.25$

Step2: Calculate contribution of Isotope 2

$59.93 \times \frac{26.16}{100} = 59.93 \times 0.2616 \approx 15.68$

Step3: Calculate contribution of Isotope 3

$60.93 \times \frac{1.25}{100} = 60.93 \times 0.0125 \approx 0.7616$

Step4: Calculate contribution of Isotope 4

$61.93 \times \frac{3.66}{100} = 61.93 \times 0.0366 \approx 2.267$

Step5: Calculate contribution of Isotope 5

$63.93 \times \frac{1.16}{100} = 63.93 \times 0.0116 \approx 0.7416$

Step6: Sum all contributions

Add the contributions from each isotope:
$39.25 + 15.68 + 0.7616 + 2.267 + 0.7416 \approx 58.7$

Answer:

58.7 amu