Explanation Explanation The atomic mass of 56 Fe = 55 .9349 amu . Mass of 1 1 H = 1 .00782 amu . The mass of neutron is 1.00866 amu . Number of protons in 56 Fe = 26 Number of neutrons in 56 Fe = 30 The mass defect is calculated by the formula, Δ m = Atomic mass of 56 Fe − [ Number of protons × mass of 1 1 H proton − Number of neutrons × mass of neutron ] Substitute the value of the atomic mass 56 Fe , the number of protons and mass of the 1 1 H proton and that of the neutron in the above equation. Δ m = 55 .9349 − [ ( 26 × 1.00782 ) + ( 30 × 1.00866 ) ] Δ m = − 0.589 amu / nucleus The conversion of amu / nucleus to Kg/nucleus is done as, 1 amu = 1.66 × 10 − 27 Kg Therefore, the conversion of − 0.589 amu / nucleus into kg/nucleus is, − 0.5289 amu / nucleus = ( − 0.5289 × 1 × 1.66 × 10 − 27 ) kg/nucleus = - 0 . 8 7 7 9 × 1 0 - 2 7 K g / n u c l e u s _ Therefore, the mass defect ( Δ m ) of 56 Fe is - 0

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ISBN: 9781305079243

Author: Steven S. Zumdahl, Susan A. Zumdahl

Publisher: Cengage Learning

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Writing and Balancing Nuclear Equations

A nuclear equation is a symbolic representation of a nuclear reaction using certain symbols. It is studied in nuclear chemistry and nuclear physics.

Question

Chapter 18, Problem 44E

Interpretation Introduction

Interpretation: The binding energy per nucleon of 56Fe is to be calculated.

Concept introduction: The sum of masses of the component nucleons and the actual mass of a nucleus is known as the mass defect and it can be used to calculate the nuclear binding energy.

To determine: The binding energy per nucleon of 56Fe

Expert Solution & Answer

Chapter 18 Solutions

Chemistry: An Atoms First Approach

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