Average atomic weight of an element $M$ is $51.7$ . If two isotopes of $M, M^{50}$ and $M^{52}$ are present, then calculate the percentage of occurrence of $M^{50}$ in nature.

Open in App

Solution

Average Atomic weight = $F_{1} M_{1} + F_{2} M_{2} + . . . F_{n} M_{n}$

$F_{1}, F_{2}, F_{3} . . . F_{n}$ are percentage fraction.

$M_{1}, M_{2}, M_{3} . . . M_{n}$ are molecular weight of isotope.

$51.7 = x \times (50) + (1 - x) 52$

$51.7 = 50 x + 52 - 52 x$

$- 2 x = - 0.3$

$x = \frac{0.3}{2}$

$x = 0.15$

Abundance of $M^{50}$ in nature is 15%

and Abundance of $M^{52}$ in nature is 85%

Suggest Corrections

Similar questions

Q. An element have three isotopes and their isotopic weight are 11, 12, 13 unit their percentage of occurrence in nature is 85, 10, 5 respectively, then calculate the average atomic weight of element.

Q. An element Z contains two naturally occurring isotopes ³⁵Z₁₇ and³⁷Z₁₇. If the average atomic mass of this element be 35.5 u, calculate the percentage of two isotopes.

Q. The average atomic mass of an element is calculated by its isotopic percentage but what if the average atomic mass is given and we have to find the percentage of a isotopes??
eg:- average atomic mass of an element exist 16.2 u. What is the percentage of isotopes
16. . 18
. X. X
8. 8

(a) What are radioactive isotopes ? Give two examples of radioactive isotopes.

(b) Give any two uses of radioactive isotopes.

(c) An element Z contains two naturally occurring isotopes ${}_{17}^{35}Z$ and ${}_{17}^{37}Z$ . If the average atomic mass of this element be 35.5 u, calculate the percentage of two isotopes.

Q. The relative atomic mass of an element A is

16.2

there are two isotopes

_{8}^{16} A

and

_{8}^{18} A

of the element. Calculate the percentage of these two isotopes present in the element.

Join BYJU'S Learning Program

Average atomic weight of an element M is 51.7. If two isotopes of M, M50 and M52 are present, then calculate the percentage of occurrence of M50 in nature.

Average Atomic weight = F1M1+F2M2+...FnMnF1,F2,F3...Fn are percentage fraction.M1,M2,M3...Mn are molecular weight of isotope.51.7=x×(50)+(1−x)5251.7=50x+52−52x−2x=−0.3x=0.32x=0.15Abundance of M50 in nature is 15%and Abundance of M52 in nature is 85%

Average atomic weight of an element $M$ is $51.7$ . If two isotopes of $M, M^{50}$ and $M^{52}$ are present, then calculate the percentage of occurrence of $M^{50}$ in nature.