Weighted Average Atomic Mass of Iron,Calculate the weighted average atomic mass of iron using the following naturally occurring isotopes of the elements Fe. The masses of each isotope follow their symbols and the percent in which each exits is given: Fe-54 with 6% abundance Fe-56 with 92% abundance and Fe-57 with 2% abundance. This would be calculated much like your calculate your grades which is a waiting average.

Weighted Average Atomic Mass of Iron

The weighted average atomic mass of a particular element is the average mass of the atoms of that element when compared to 1/12th of the mass of a single carbon-12 atom. This average is determined by taking into account the mass of each of the element’s isotopes and the abundance of each isotope in nature. Iron is made up of three naturally occurring isotopes; Fe-54, Fe-56, and Fe-57. Fe-54 has an abundance of 6%, Fe-56 has an abundance of 92%, and Fe-57 has an abundance of 2% (Khan Academy, 2020). To calculate the weighted average atomic mass of iron, we need to multiply the mass of each isotope by its abundance and add them together. The mass of Fe-54 is 53.939 amu, the mass of Fe-56 is 55.935 amu, and the mass of Fe-57 is 56.935 amu (Khan Academy, 2020). We can multiply each mass by its abundance to get the following:
Fe-54: 53.939 * 0.06 = 3.236 amu
Fe-56: 55. Cont…

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