We must first calculate the mass defect (Am) for 56Fe. Since atomic masses (which include the electrons) are given, we must decide how to account for the electron mass: 55.9349 = mass of 56 Fe atom = mass of nucleus + 26 m. 1.0078 = mass of H atom = mass of nucleus + m, Thus, since a 56Fe nucleus is "synthesized" from 26 protons and 30 neutrons, we see that Am = (55.9349 - 26 m.) - [26(1.0078 - ma) + 30(1.0087)]. Solve for Am. Am = 0.5289 amu

We must first calculate the mass defect (Am) for 56Fe. Since atomic masses (which include the electrons) are given, we must decide how to account for the electron mass: 55.9349 = mass of 56 Fe atom = mass of nucleus + 26 m. 1.0078 = mass of H atom = mass of nucleus + m, Thus, since a 56Fe nucleus is "synthesized" from 26 protons and 30 neutrons, we see that Am = (55.9349 - 26 m.) - [26(1.0078 - ma) + 30(1.0087)]. Solve for Am. Am = 0.5289 amu

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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