what is the atomic weight of the element? (amu)

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A certain element consists of two stable isotopes.

The first has an atomic mass of 62.9 amu and a percent natural abundance of 69.1 %.
The second has an atomic mass of 64.9 amu and a percent natural abundance of 30.9 %.

Feb 1st, 2015

To calculate the average atomic weight, each exact atomic weight is multiplied by its percent abundance (expressed as a decimal). Then, add the results together and round off to an appropriate number of significant figures.

Atomic weight= (62.9*0.69) +(64.9*0.309)

68.71

rate my answer as best please if it helps

Feb 1st, 2015

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