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an element, x, has two naturally occurring isotopes. isotope 1 has a mass of 2.370 x 10-22 g and a relative abundance of 66.1%. isotope 2 has a mass of 2.311 x 10-22 g. what is the average atomic mass of the element in g/mol?



Answer :

The average atomic mass of the element is 2.35 × 10^-22 g/mol if it has two naturally occurring isotopes.

The average atomic mass of the element can be calculated by using the following formula;

([atomic mass of isotope 1 × abundance of isotope 1] + [atomic mass of isotope 2 × abundance of isotope 2]) ÷ (abundance of isotope 1 + abundance of isotope 2)

As isotope 1 has a relative abundance of 66.1%, the relative abundance of isotope 2 can be calculated as follows;

relative abundance of isotope 2 = 100% - 66.1% = 33.9%

Now substitute the values in the equation as follows;

average atomic mass = ([2.370 x 10^-22 × 66.1] + [2.311 x 10^-22 × 33.9]) ÷ (66.1 + 33.9)

average atomic mass = 2.35 × 10^-22

Therefore the average atomic mass is calculated to be 2.35 × 10^-22 g/mol.

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