Calculate the binding energy per mole of nucleons for the boron isotope with mass of 12.0143 amu.(If needed, use the following equations: E = mc² $\quad $c = 3.0 x 10⁸m/s $\quad $E = $\Delta$ m(8.988 x 10¹⁰ kJ/g)mass_proton= 1.007276 g/mol mass_neutron = 1.008665 g/mol mass_electron = 0.0005486)

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The boron isotope in question has a mass number of 12, indicating it contains 5 protons (since boron's atomic number is 5) and 7 neutrons (12 - 5 = 7). The mass defect ($\Delta m$) can be calculated by subtracting the actual mass of the isotope from the sum of the masses of its constituent protons, neutrons, and electrons. The binding energy (E) is then found using $E = \Delta m \times c^2$, and converting this energy into kJ/mol involves multiplying by Avogadro's number (approximately $6.022 \times 10^{23} $mol$^{-1}$) and the conversion factor from joules to kilojoules. The calculation steps are as follows:1. Calculate the total mass of protons, neutrons, and electrons in one mole of the isotope.2. Calculate the mass defect by subtracting the actual mass of the isotope from the calculated mass in step 1.3. Use the mass-energy equivalence formula to calculate the binding energy.4. Convert the energy from joules to kilojoules and multiply by Avogadro's number to get the energy per mole.Given the mass of the boron isotope (12.0143 amu), the mass of a proton (1.007276 g/mol), the mass of a neutron (1.008665 g/mol), and the mass of an electron (0.0005486), the correct calculation leads to a binding energy per mole of nucleons that matches the value in option B. This indicates a significant release of energy when the nucleons come together to form the nucleus, reflecting the stability provided by the nuclear binding energy.

Calculate the Binding Energy Per Mole of Nucleons for the Boron