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2. A hypothetical alloy has a face-centered cubic unit cell. Its density is 10,470 kg/m³, and its atomic weight is 106.8 g/mole. a) What is the atomic radius of the alloy in cm? b) What is the volume of the single atom of the alloy in cm3?

2. A hypothetical alloy has a face-centered cubic unit cell. Its density is 10,470 kg/m³, and its atomic weight is 106.8 g/mole. a) What is the atomic radius of the alloy in cm? b) What is the volume of the single atom of the alloy in cm3?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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PLEASE ANSWER NUMBER 2. 

I. PROBLEM SOLVING: Solve the following problems completely, neatly and orderly. Express all answers to the nearest 4th decimal place. No unit or wrong unit means wrong answer. 1. Cobalt crystallizes in a HCP unit cell. Its atomic radius is 0.1253 nm. Its density is 8,900 kg/m³. Using this information, estimate Avogadro's number. 2. A hypothetical alloy has a face-centered cubic unit cell. Its density is 10,470 kg/m2, and its atomic weight is 106.8 g/mole. a) What is the atomic radius of the alloy in cm? b) What is the volume of the single atom of the alloy in cm??
Transcribed Image Text:I. PROBLEM SOLVING: Solve the following problems completely, neatly and orderly. Express all answers to the nearest 4th decimal place. No unit or wrong unit means wrong answer. 1. Cobalt crystallizes in a HCP unit cell. Its atomic radius is 0.1253 nm. Its density is 8,900 kg/m³. Using this information, estimate Avogadro's number. 2. A hypothetical alloy has a face-centered cubic unit cell. Its density is 10,470 kg/m2, and its atomic weight is 106.8 g/mole. a) What is the atomic radius of the alloy in cm? b) What is the volume of the single atom of the alloy in cm??
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