University:
Eastern Kentucky University
Course:
CHE 111 | General Chemistry
Academic year:

2021
Views:

195

Pages:

2
Author:

Trevon Bernard

Name _____________________________ Calculating Average Atomic Mass Worksheet Show ALL calculation setups. 1. The term “average atomic mass” is a _________________________average, and so is calculated differently, from a “normal” average. Explain how this type of average is calculated. ----------------------------------------------------------------------------------------------------------------------------------2. The element Copper has naturally occurring isotopes with mass numbers of 63 and 65. The relative abundance and atomic masses are: 69.2% for mass of 62.93u 30.8% for mass of 64.93u. Calculate the average atomic mass of Copper. Show ALL work for full credit. ----------------------------------------------------------------------------------------------------------------------------------3. Calculate the average atomic mass of Sulfur if: 95.00% of all Sulfur atoms have a mass of 31.972 u, 0.76% has a mass of 32.971u and 4.22% have a mass of 33.967u. Show ALL work for full credit. ------------------------------------------------------------------------------------------------------------------------------------4. Naturally occurring Strontium consists of four isotopes, Sr-84, Sr-86, Sr-87 and Sr-88. Below is the data concerning Strontium: Sr-84 0.56% Sr-86 9.86% Sr-87 7.00% Sr-88 82.58% What is the average atomic mass of Strontium? Show ALL work, for full credit. --------------------------------------------------------------------------------------------------------------------------------------5. Calculate the average atomic mass of Bromine. Show ALL work, for full credit. One isotope of Bromine has an atomic mass of 78.92u and a relative abundance of 50.69%. The other major isotope of Bromine has an atomic mass of 80.92u and a relative abundance of 49.31%.