Question

An element x has two isotopes of masses 59.974 u abd 61.982 u. If their abundance is 40% and 60% respectively.Calculate,average atomic mass in u and kg​

Answer 1

60 is the answer in kg

thanks for watching my answer

Answer 2

Answer:

The average atomic mass is 61.1788u and $1.015873974\times e^{-25}$kg.

Explanation:

Let, the two isotopes are $X_A$ and $X_B$.

An element x has two isotopes of masses 59.974 u and 61.982 u. If their abundance is 40% and 60% respectively.

Now,

The mass of $X_A$  isotope is 59.974 u. Suppose its percentage in the sample is 40%.

The mass of $X_B$  isotope is  61.982 u. Its percentage in the sample will 60%.

So, Average atomic mass of $X=59.974 \times \frac{40}{100} +61.982 \times \frac{60}{100}$

Therefore,

$X=59.974 \times \frac{40}{100} +61.982 \times \frac{60}{100}\\\\X= \frac{2398.96}{100} +\frac{3718.92}{100}\\\\X=61.1788$

Hence, the average atomic mass is 61.1788u and $1.015873974\times e^{-25}$kg.

To find more answers linked with atomic mass of molecule, click on the given link below,

https://brainly.in/question/1516290

https://brainly.in/question/207972

#SPJ3