An unknown element Q has two known isotopes: 61Q and 63Q. If the average atomic mass is 61.2 amu, what are the relative percentages of the isotopes?
The average atomic mass of the element is the sum of the individual masses of its isoptopes , each multiplied by its relative abundance .
Let the relative abundance of 61Q isotope be x .
So the relative abundance of 63Q isotope will be 100-x.
putting the values in the formula , we get ,
61.2 = [61.x + 63(100-x)] / 100
61.2 = [61x + 6300 - 63x ] / 100
6120 = 6300 - 2x
x = 90%
And 100 - x = 100 - 90 = 10%
So the realtive percentage of 61Q is 90% and 63Q is 10%.
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