Silver has only two naturally occurring isotopes. The mass ofsilver-107 is 106.9

Question

Silver has only two naturally occurring isotopes. The mass ofsilver-107 is 106.9051 amu and the mass of silver-109 is108.9048 amu. Use the atomic mass of silver to calculatethe relative abundance of silver-107. _________% Use the atomic mass of silver to calculatethe relative abundance of silver-109. _________% Silver has only two naturally occurring isotopes. The mass ofsilver-107 is 106.9051 amu and the mass of silver-109 is108.9048 amu. Use the atomic mass of silver to calculatethe relative abundance of silver-107. Use the atomic mass of silver to calculatethe relative abundance of silver-107. _________% Use the atomic mass of silver to calculatethe relative abundance of silver-109. Use the atomic mass of silver to calculatethe relative abundance of silver-109. _________%

Explanation / Answer

Since 106.9051 is near the given amu of ag on the periodictable, we know it is the most abundantly occuring isotope, sosolving will give us its percentage 107.8682 = 106.9051(x) + 108.9048(1-x) 107.8682 = 106.9051x + 108.9048 - 108.9048x x = .51837 abudance of ag-107 = .51837 * 100 =51.837%
Since there is only two naturally occuring isotopes that meansthat the reamining percentage is the abudance of ag-109 so 100% - 51.837% = 48.163%
Hope this helps.

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