wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

The three stable isotopes of neon: 20 21 2210 10 Ne, Ne and Ne 10 haverespective abundances of 90.51%, 0.27% and 9.22%. The atomicmasses of the three isotopes are 19.99 u, 20.99 u and 21.99 u,respectively. Obtain the average atomic mass of neon.

Open in App
Solution

Given: The atomic masses of neon isotopes 10 20 Ne, 10 21 Ne and 10 22 Ne are 19.9u, 20.99u and 21.99u respectively and the abundances of neon isotopes 10 20 Ne, 10 21 Ne and 10 22 Ne are 90.51%, 0.27% and 9.22% respectively.

The average atomic mass of neon is given as,

m= m 1 η 1 + m 2 η 2 + m 3 η 3 η 1 + η 2 + η 3

Where, the atomic masses of neon isotopes 10 20 Ne, 10 21 Ne and 10 22 Ne are m 1 , m 2 and m 3 respectively and the abundances of neon isotopes 10 20 Ne, 10 21 Ne and 10 22 Ne are η 1 , η 2 and η 3 respectively.

By substituting the given values in the above formula, we get

m= 19.99×90.51+20.99×0.27+21.99×9.22 90.51+0.27+9.22 = 1809.2949+5.6673+202.7478 100 = 2017.71 100 =20.1771u

Thus, the average atomic mass of the neon is 20.1771u.


flag
Suggest Corrections
thumbs-up
2
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Nucleus - Common Terms
PHYSICS
Watch in App
Join BYJU'S Learning Program
CrossIcon