What is the binding energy (in J/mol or kJ/mol) of an electron in a metal whose threshold frequency for photoelectrons is 2.50 * 10¹⁴ /s A) 2.75 * 10^-43 J/mol B) 1.66 * 10^-19 J/mol C) 1.20 * 10^-6 J/mol D) 99.7 kJ/mol E) 7.22 * 10¹⁷ kJ/mol

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Quizplus · Accepted Answer

The binding energy of an electron in a metal can be calculated using the equation $E = h\nu$, where $E$ is the energy, $h$ is Planck's constant ($6.626 \times 10^{-34} \, \text{J s}$), and $\nu$ is the threshold frequency. Given the threshold frequency is $2.50 \times 10^{14} \, \text{s}^{-1}$, the energy per electron is calculated as $E = 6.626 \times 10^{-34} \, \text{J s} \times 2.50 \times 10^{14} \, \text{s}^{-1} = 1.6565 \times 10^{-19} \, \text{J}$. To convert this energy to kJ/mol, multiply by Avogadro's number ($6.022 \times 10^{23} \, \text{mol}^{-1}$) and convert J to kJ, resulting in approximately $99.7 \, \text{kJ/mol}$.

What Is the Binding Energy (In J/mol or KJ/mol) of an Electron