The bond energy of N₂ is 160 kJ/mol. What is the wavelength of a photon that can cause the dissociation of a N₂ molecule? (h = 6.63 × 10^-34J s; c = 3.0 × 10⁸m/s and Avogadro's number = 6.022 × 10²³ molecules/mole)

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The energy of a photon is given by E = hc/λ, where h is Planck's constant, c is the speed of light, and λ is the wavelength. The bond energy of N2 is 160 kJ/mol, which is equal to 160 × 10^3 J/mol. To dissociate a N2 molecule, we need to provide energy equal to the bond energy. Therefore, the wavelength of a photon that can cause the dissociation of a N2 molecule is:λ = hc/E = (6.63 × 10^-34 J s)(3.0 × 10^8 m/s) / (160 × 10^3 J/mol) = 749 nm

The Bond Energy of N2 Is 160 KJ/mol

The Bond Energy of N₂ Is 160 KJ/mol