Solving Binding Energy Problem of 147N

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SUMMARY

The discussion focuses on calculating the binding energy of the nitrogen isotope 147N, which has a nuclear mass of 13.999234 amu. The mass defect is determined to be 0.007466 amu, which is converted to kilograms as 1.23976 x 10-29 kg. Using the mass-energy equivalence formula E = mc2, the energy calculated is 1.115784 x 10-12 J. However, the expected binding energy per nucleon is 1.19773 x 10-12 J/nucleon, indicating a discrepancy in the calculation process.

PREREQUISITES
  • Nuclear physics concepts, specifically binding energy and mass defect
  • Understanding of mass-energy equivalence (E = mc2)
  • Ability to convert atomic mass units (amu) to kilograms
  • Familiarity with isotopes and their properties
NEXT STEPS
  • Learn about the calculation of binding energy for different isotopes
  • Research the significance of mass defect in nuclear physics
  • Study the periodic table's representation of isotopes and their masses
  • Explore advanced topics in nuclear reactions and energy release
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Students in nuclear physics, educators teaching isotope stability, and researchers interested in binding energy calculations.

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Homework Statement



Problem: Calculate the binding energy of 147N (nuclear mass of 13.999234 amu) in Joules per nucleon. According to periodic table, the mass of N is 14.0067 amu.

Homework Equations


E = mc2


The Attempt at a Solution



Calculate mass defect:

13.999234 - 14.0067 = 0.007466
Convert to kg:

0.007466 * (1.66053886 * 10-27) = 1.23976 * 10-29

Use mass/energy equivalence (E = mc2) to calculate energy of the mass defect:

E = (1.23976 * 10-29)(3 * 108)2 = 1.115784 * 10-12[/EQ]

The result *should* be the binding energy of the entire molecule (I would have thought per nucleon would be just dividing this by 14) - but the answer my book gives is 1.19773*10-12 J/nucleon.

Where have I gone wrong?
 
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Periodic table doesn't contain mass of a nuclide in question.

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