Question
Rubidium has two naturally occurring isotopes, rubidium-85 (atomic mass $=84.9118$ amu; abundance $=72.15 \%$ ) and rubidium-87 (atomic mass = 86.9092 amu; abundance = 27.85$\%$ ). Calculate the atomic weight of rubidium.
Step 1
This is done by dividing the percentage by 100. For rubidium-85, this gives $0.7215$ and for rubidium-87, this gives $0.2785$. Show more…
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Rubidium has two naturally occurring isotopes: Rb-85 with mass 84.9118 amu and a natural abundance of $72.17 \%,$ and Rb-87 with mass 86.9092 amu and a natural abundance of 27.83\%. Calculate the atomic mass of rubidium.
The atomic weight of rubidium is 85.4678 amu. The two naturally occurring isotopes of rubidium have the following masses: ${ }^{85} \mathrm{Rb}, 84.9118 \mathrm{amu} ;{ }^{87} \mathrm{Rb}, 86.9092$ amu. Calculate the percent of each isotope in naturally occurring rubidium.
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