Word Count : 451

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We are given: * Mass defect of uranium-235, $\Delta m(^{235}\text{U}) = 49.899 \, \text{MeV}$ * Mass defect of aluminum-27, $\Delta m(^{27}\text{Al}) = -0.01847 \, u$ We are to calculate the atomic mass of each isotope using the mass defect. --- ### Step 1: Mass Defect and Atomic Mass Relation Mass defect is the difference between the mass of the separated nucleons and the actual atomic mass. $$ \Delta m = Zm_p + Nm_n - M_{\text{nucleus}} $$ Where: * $Z$: number of protons * $N$: number of neutrons * $m_p = 1.007276 \, \text{u}$ * $m_n = 1.008665 \, \text{u}$ * $\Delta m$: mass defect in u (not MeV!) * $M_{\text{nucleus}}$: nuclear mass ______ ____ ____ _____ __________ _______ ______ __________ _____ ____.
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