Problem: A certain element has 2 naturally occurring isotopes with the masses and natural abundances shown below. Calculate the atomic mass of the element. Isotope - 1  78.925 amu, 60.11 %Isotope - 2 80.925 amu, 39.86 %A) 79.70 amuB) 79.93 amuC) 80.00 amuD) 79.80 amu

FREE Expert Solution

We can use the following equation to calculate the atomic mass:


Atomic Mass=[mass×f.a.]isotope 1+[mass×f.a.]isotope 2


where:

atomic mass = average atomic mass of the element 

f.a. = fractional abundance of the isotope

To get f.a., we simply need to divide the given percent abundance by 100.


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Problem Details

A certain element has 2 naturally occurring isotopes with the masses and natural abundances shown below. Calculate the atomic mass of the element. 

Isotope - 1  78.925 amu, 60.11 %

Isotope - 2 80.925 amu, 39.86 %

A) 79.70 amu

B) 79.93 amu

C) 80.00 amu

D) 79.80 amu

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