Problem: 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.

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FREE Expert Solution

atomic weight = [mass×f.a.]rubidum-85 + [mass×f.a.]rubidum-87


rubidium-85: atomic mass 84.9118 amu        f.a. = 72.15% ÷ 100 = 0.7215

rubidium-87: atomic mass 86.9092 amu      f.a. 27.85% ÷ 100 = 0.2785


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Problem Details

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.

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Our tutors have indicated that to solve this problem you will need to apply the Isotopes concept. You can view video lessons to learn Isotopes. Or if you need more Isotopes practice, you can also practice Isotopes practice problems.

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Based on our data, we think this problem is relevant for Professor Tanizaki's class at UTA.