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Solution for 2. The element X has three naturally occurring isotopes. The isotopic masses (amu) and % abundances of the isotopes are given in the table below.…

Feb 14, 2020 · Multiply each isotope's mass by its abundance. If your abundance is a percent, divide your answer by 100. Add these values together. There are a few ways to determine the mass number, depending on what information you have about the isotope: 1. The mass number is calculated as the sum of an isotope's protons and neutrons. 2.

The natural isotopic abundance of an element can readily be obtained by clicking a fragment consisting of a single atom of the element in question. Natural isotopic abundance data were obtained from: J. Emsley: “The Elements”, 3rd ed., Oxford University Press, 1998.

If you're given the mass of each isotope of an element, and the average atomic mass, you can calculate the percent (%) abundance of each isotope. Let "x" be...

The isotopic abundance ratio of natural silver (Ag) is the ratio of the stable isotopes Ag107 to Ag109. Its mean is 1.076, and measurements on a random sample of observed isotopic abundance ratios suggested that they are plausibly normally distributed with a sample standard deviation of 0.0026.

Naturally occurring element X exists in three isotopic forms: X-28 (27.977 amu, 92.23% abundance), X-29 (28.976 amu, 4.67% abundance), and X-30 (29.974 amu, 3.10% abundance). Calculate the atomic weight of X.