What is the energy per Cl-Cl bond and the wavelength of light that would be required to break this bond?

Question

It has been found that when the chemical bond in a diatomic molecule Cl2, that 328 kJ is released per mole of Cl2 formed. What is the energy per Cl-Cl bond and the wavelength of light that would be required to break this bond?

Answer 1

Let's assume that the energy of the Cl - Cl bond is 328 kJ/mol.
So that's how much energyis needed to break it.

328 kJ/mol = 5.49 x 10^ -19 J/molecule

Use E = hf (E = energy, h = Planck's constant)
to find the frequency (f) of the light with that much energy.

Then, use the universal wave equation v= f(lambda) where v is the speed of light, and lamba is the wavelength, in metres.

Good luck !