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 $$= \dfrac {\sum_{i = 1}^{n} { (mass_{(i)})(Abundance_{(i)})}}{100}$$$$m=\displaystyle \frac{90.51\times 19.99+0.27\times 20.99+9.22\times 21.99}{100}$$    $$=20.18u$$PhysicsNCERTStandard XII

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