Apr 28th, 2015
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1. Element Q has three isotopes. The first has a mass of 34.8636 amu and makes up 39.2 % of a standard sample. The second isotope has a mass of 36.5076 amu and makes up 43 % of a standard sample. The third isotope has a mass of 38.1639 amu and makes up the remainder of a standard sample. What is the average atomic mass of this element?SolutionFirst isotope of element Q has 34.8636amu and makes up 39.2% of QSecond isotope of element Q has 36.5076amu and makes up 43 % of QThird isotope of element Q has 38.1639amu and makes up of (100-39.2-43) = 17.8% of QThe solution is laid out like this:(Exact weight of isotope #1) x (Abundance of isotope #1) + (exact weight of isotope #2) x (abundance of isotope #2) = average atomic weight of the elementTherefore:(34.8636 x 0.392) + (36.5076 x 0.43) + (38.1639 x 0.178) = 13.6665312+15.698268+6.7931742= 36.1579734amu is the average atom

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