Question

what is the average atomic mass of the element in the data table?mass (amu) abundance (%)14.0 99.63215.0 0.36864.8 amu 24.6 amu14.0 amu 35.5 amu

Explanation:

Step1: Convert percentages to decimals

For the first isotope: \(99.632\%=0.99632\). For the second isotope: \(0.368\% = 0.00368\)

Step2: Calculate the contribution of each isotope

The contribution of the first isotope: \(14.0\times0.99632 = 13.94848\)
The contribution of the second isotope: \(15.0\times0.00368=0.0552\)

Step3: Sum up the contributions

\(13.94848 + 0.0552=14.00368\approx14.0\)

Answer:

14.0 amu