{"id":248611,"date":"2025-07-08T14:06:05","date_gmt":"2025-07-08T14:06:05","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=248611"},"modified":"2025-07-08T14:06:07","modified_gmt":"2025-07-08T14:06:07","slug":"two-isotopes-of-rubidium-occur-naturally-rb-with-mass-of-85-and-atomic-number-of-37-at-72-17-84-91-amu-and-rb-with-mass-of-87-and-atomic-number-of-37-at-27-83","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/08\/two-isotopes-of-rubidium-occur-naturally-rb-with-mass-of-85-and-atomic-number-of-37-at-72-17-84-91-amu-and-rb-with-mass-of-87-and-atomic-number-of-37-at-27-83\/","title":{"rendered":"Two isotopes of rubidium occur naturally, Rb with mass of 85 and atomic number of 37 at 72.17% (84.91 amu) and Rb with mass of 87 and atomic number of 37 at 27.83%"},"content":{"rendered":"\n

Two isotopes of rubidium occur naturally, Rb with mass of 85 and atomic number of 37 at 72.17% (84.91 amu) and Rb with mass of 87 and atomic number of 37 at 27.83% (86.91 amu). Calculate the atomic mass for rubidium using the weighted average mass method.<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

To calculate the atomic mass of rubidium using the weighted average mass method, we need to consider the relative abundances of the two isotopes and their respective atomic masses. The weighted average mass is calculated by multiplying the atomic mass of each isotope by its relative abundance (expressed as a decimal), then adding the results.<\/p>\n\n\n\n

Given:<\/h3>\n\n\n\n