an element has two stable isotopes. 1) 6.015 amu and 0.0759 abundant 2) 7.016 amu and 0.9241 abundant what…

an element has two stable isotopes. 1) 6.015 amu and 0.0759 abundant 2) 7.016 amu and 0.9241 abundant what is the average atomic mass of the element? ? amu

an element has two stable isotopes. 1) 6.015 amu and 0.0759 abundant 2) 7.016 amu and 0.9241 abundant what is the average atomic mass of the element? ? amu

Answer

Answer:

6.941 amu

Explanation:

Step1: Recall the formula

The formula for average atomic mass is $\sum_{i}(m_i\times a_i)$, where $m_i$ is the mass of isotope $i$ and $a_i$ is the abundance of isotope $i$.

Step2: Calculate the contribution of first - isotope

For the first isotope with mass $m_1 = 6.015$ amu and abundance $a_1=0.0759$, the contribution is $m_1\times a_1=6.015\times0.0759 = 0.4565385$ amu.

Step3: Calculate the contribution of second - isotope

For the second isotope with mass $m_2 = 7.016$ amu and abundance $a_2 = 0.9241$, the contribution is $m_2\times a_2=7.016\times0.9241=6.4844856$ amu.

Step4: Find the average atomic mass

The average atomic mass $A = 0.4565385+6.4844856=6.9410241\approx6.941$ amu.