Question

An unknown element X has the following isotopes: ²⁵X (80.5% abundant) and ²⁷X (19.5% abundant). What is the Average atomic mass in amu of X?

Answer 1

Answer:

the average atomic mass in amu of X is 25.39 amu

Explanation:

The computation of the average atomic mass in the amu of X is shown below:

Average mass is

= Product sum + atomic mass of each and every isotope

Now the average mass

= (80.5 ÷ 100 × 25 amu) + (19.5 ÷ 100 × 27 amu)

= 20.125 + 5.265

= 25.39 amu

Hence, the average atomic mass in amu of X is 25.39 amu

Answer 2

The average atomic mass of X is 25.39 amu.

Atomic mass

It is the quantity of matter present within an atom of an element.

Based on the given information,

• The unknown element X has the isotopes, 25X (80.5% abundant) and 27X (19.5% abundant).

Now the atomic mass of X can be calculated by using the formula,

$=\frac{(M1*A1)+(M2*A2)}{A1+A2}$

Here, M1 and M2 are the atomic masses, and A1 and A2 are their  abundances.

Now putting the values we get,

$= \frac{(25*80.5)+(27*19.5)}{80.5+19.5} \\\\= \frac{2012.5+526.5}{100} \\= \frac{2539}{100} \\= 25.39 amu$

Thus, the average atomic mass of X is 25.39 amu.

For more information about atomic mass see here :

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