Element X has three isotopes, ^22X, ^23X, and ^25X. The relative abundances are 60%, 35%, and 5% respectively. What is the average atomic mass foe element X?

Show Work Please :)

To find the average atomic mass of element X, we need to calculate a weighted average using the relative abundances and atomic masses of each isotope.

Step 1: Gather the atomic masses of each isotope:
The atomic masses of the three isotopes are ^22X = 22 amu, ^23X = 23 amu, and ^25X = 25 amu.

Step 2: Convert the relative abundances into decimal form:
The relative abundance of ^22X is 60%, which can be written as 0.60.
The relative abundance of ^23X is 35%, which can be written as 0.35.
The relative abundance of ^25X is 5%, which can be written as 0.05.

Step 3: Calculate the weighted average atomic mass:
The weighted average atomic mass can be calculated using the following formula:
Average atomic mass = (abundance of ^22X × atomic mass of ^22X) + (abundance of ^23X × atomic mass of ^23X) + (abundance of ^25X × atomic mass of ^25X)

Plugging in the values:

Average atomic mass = (0.60 × 22 amu) + (0.35 × 23 amu) + (0.05 × 25 amu)
= (13.2 amu) + (8.05 amu) + (1.25 amu)
= 22.5 amu

Therefore, the average atomic mass of element X is 22.5 amu.

Did you post all of the question? The mass of 22X should be a little less than 22, the mass of 23X should be a little less than 23 and the mass of 25X should be a little less than 25.

(mass 22X*0.60) + (mass 23X*0.35) + (mass 25X*0.05) = Y. Solve for Y.