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Question

The three stable isotopes of neon: $$_{10}^{20}\textrm{Ne}$$, $$_{10}^{21}\textrm{Ne}$$ and $$_{10}^{22}\textrm{Ne}$$ have respective abundances of $$90.51 \%, 0.27 \%$$ and $$9.22 \%$$. The atomic masses of the three isotopes are $$19.99 u, 20.99 u$$ and $$21.99 u$$, respectively. Obtain the average atomic mass of neon.


Solution

The average atomic mass is given by,

Average atomic mass $$= \dfrac {\sum_{i = 1}^{n} { (mass_{(i)})(Abundance_{(i)})}}{100}$$

$$m=\displaystyle \frac{90.51\times 19.99+0.27\times 20.99+9.22\times 21.99}{100}$$

    $$=20.18u$$

Physics
NCERT
Standard XII

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