Lithium has 2 isotopos. One has a mass of

16.015 AM and the other 7.016 ANU. The on

average atomic mass is 6.941 AMU. What are

the lo abundances of each (to 2 decimal

places) ?

The isotope with mass 6.015amu = 7.5% abundance

The isotope with mass 7.016amu = 92.5%

Explanation:

Step 1: Given data

Lithium has an average atomic mass of 6.941 amu

Lithium has 2 isotopos with a mass, respectively 6.015amu and 7.016amu

Step 2: Calculate the abundances

Isotope with mass 6.015 amu has an abundance of X

Isotope with mass 7.016 amu has an abundance of Y

The average atomic mass is the average mass of the isotopes with its respectively abundance.

X+Y = 1 or X = 1 - Y

6.941 = 6.015X + 7.016Y

This gives us:

6.941 = 6.015 (1-Y) + 7.016Y

6.941 = 6.015 - 6.015Y + 7.016Y

6.941 - 6.015 = - 6.015Y + 7.016Y

0.926 = 1.001Y

Y = 0.925

Y = 92.5%

X = 1 - 92.5 = 7.5%

To control we can do the following equation:

6.015*0.075 + 7.016*0.925 = 6.941

This means the abundances of the 2 isotopes are:

The isotope with mass 6.015amu = 7.5% abundance

The isotope with mass 7.016amu = 92.5%