🤓 Based on our data, we think this question is relevant for Professor Ratliff's class at USF.
First, calculate mass defect:
Li–7 (atomic mass = 7.016003 amu)
Atomic number→ 3 → 3 protons
Mass number → 7
Neutrons → 7-3 = 4
Mass values needed:
Proton = 1.007277 amu
electron = 0.000548597 amu
neutron = 1.008665 amu
Lithium = 7.016003 amu
Calculate mass defect:
Δm = 0.042105 amu
Substitute the equation below:
1 amu c2 = 931.49 MeV
E = 3.92 x 107 eV/nucleus
Convert to kJ/mol:
What is the nuclear binding energy of a lithium-7 nucleus in units of kJ/mol and eV/nucleus? (Mass of a lithium-7 atom = 7.016003 amu.)
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Based on our data, we think this problem is relevant for Professor Ratliff's class at USF.
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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.