What is the wavelength of a photon needed to dissociate an O₃ molecule whose bond energy is 107.2 kJ/mol (h = 6.63 × 10^-34J s; c = 3.0 × 10⁸m/s; and Avogadro's number = 6.022 × 10²³ molecules/mole)?

Question

Quizplus · Accepted Answer

To find the wavelength, first convert the bond energy from kJ/mol to J/photon: (107.2 kJ/mol) × (1000 J/kJ) / (6.022 × 10^23 molecules/mol) = 1.78 × 10^-19 J/photon. Then use the formula E = hc/λ to find the wavelength: λ = hc/E = (6.63 × 10^-34 J s × 3.0 × 10^8 m/s) / 1.78 × 10^-19 J = 1.117 × 10^-6 m = 1117 nm.

What Is the Wavelength of a Photon Needed to Dissociate