13.2 The three stable isotopes of neon: <math><mmultiscripts><mrow><mrow><mi mathvariant="bold-italic">N</mi><mi mathvariant="bold-italic">e</mi></mrow></mrow><mprescripts></mprescripts><mrow><mrow><mn>10</mn></mrow></mrow><mrow><mrow><mn>20</mn></mrow></mrow></mmultiscripts><mo>,</mo></math> <math><mmultiscripts><mrow><mrow><mi mathvariant="bold-italic">N</mi><mi mathvariant="bold-italic">e</mi></mrow></mrow><mprescripts></mprescripts><mrow><mrow><mn>10</mn></mrow></mrow><mrow><mrow><mn>21</mn></mrow></mrow></mmultiscripts></math> and <math><mmultiscripts><mrow><mrow><mi mathvariant="bold-italic">N</mi><mi mathvariant="bold-italic">e</mi></mrow></mrow><mprescripts></mprescripts><mrow><mrow><mn>10</mn></mrow></mrow><mrow><mrow><mn>22</mn></mrow></mrow></mmultiscripts></math> 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.

13.2 Atomic mass of Ne1020 neon isotope, m1 = 19.99 u ad the abundance η1 = 90.51 %Atomic mass of Ne1021 neon isotope, m2 = 20.99 u ad the abundance η2 = 0.27 %Atomic mass of Ne1022 neon isotope, m3 = 21.99 u ad the abundance η3 = 9.22 %The average atomic mass of neon is given as:m = m1η1+m2η2+m3η3η1+η2+η3 = 19.99×90.51+20.99×0.27+21.99×9.2290.51+0.27+9.22 = 2017.71100 = 20.1771 u

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Physics Ncert Solutions Class 12th Physics Class 12th Nuclei

13.2 The three stable isotopes of neon: ${}_{10}^{20}{N e},$ ${}_{10}^{21}{N e}$ and ${}_{10}^{22}{N e}$ 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.

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Payal Gupta | Contributor-Level 10

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13.2 Atomic mass of ${}_{10}^{20}{N e}$ neon isotope, $m_{1}$ = 19.99 u ad the abundance $η_{1}$ = 90.51 %

Atomic mass of ${}_{10}^{21}{N e}$ neon isotope, $m_{2}$ = 20.99 u ad the abundance $η_{2}$ = 0.27 %

Atomic mass of ${}_{10}^{22}{N e}$ neon isotope, $m_{3}$ = 21.99 u ad the abundance $η_{3}$ = 9.22 %

The average atomic mass of neon is given as:

m = $\frac{m_{1} η_{1} + m_{2 η_{2}} + m_{3} η_{3}}{η_{1} + η_{2} + η_{3}}$ = $\frac{19.99 \times 90.51 + 20.99 \times 0.27 + 21.99 \times 9.22}{90.51 + 0.27 + 9.22}$ = $\frac{2017.71}{100}$ = 20.1771 u

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13.2 The three stable isotopes of neon: ${}_{10}^{20}{N e},$ ${}_{10}^{21}{N e}$ and ${}_{10}^{22}{N e}$ 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.

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13.2 The three stable isotopes of neon: Ne1020, Ne1021 and Ne1022 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.

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13.2 The three stable isotopes of neon: ${}_{10}^{20}{N e},$ ${}_{10}^{21}{N e}$ and ${}_{10}^{22}{N e}$ 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.