Isotope Abundance
The nuclear power industry extracts Li but not Li from natural samples of lithium. As a result, the average molar mass of commercial samples of lithium is increased. The current abundace of the two isotopes are 7.42% and 95.58% respectively, and the masses of their atoms are 9.968 x 10 g and 1.165 x 10 g. What is the current molar mass of a natural sample of lithium?
Related Problems
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Given a molar mass of 116.24 g/mol and an empirical formula of CHN, find the molecular formula for this compound.
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