Question

Copying is not allowed. You must show all work in order to receive credit. Naturally occurring silver has two isotopes. Isotope A has a relative mass of 106.9051 and an abundance of 51.82%. Isotope B has a relative mass of 108.9047. Calculate the atomic mass of silver from these data.

Answer 1

Answer: The atomic mass of silver is 107.8

Step-by-step explanation:

Average atomic mass is the average mass of all the isotopes present depending on the relative abundance of each isotope.

Mass of isotope A = 106.9051

% abundance of isotope 1 = 51.82% =
`(51.82)/(100)`

Mass of isotope B = 108.9047

% abundance of isotope 2 = (100-51.82)% =
`(48.18)/(100)`

Formula used for average atomic mass of an element :

`A=\sum[(106.9051)* (51.82)/(100))+(108.9047)* (48.18)/(100)]]`

`A=107.8`

Therefore, the average atomic mass of silver is 107.8