A minimum energy of 151 kJ is required to dissociate a mole of iodine molecules, I2. Calculate the wavelength of radiation that supplies this energy, assuming each bond beaks by absorbing one photon.

dE = hc/wavelength

To calculate the wavelength of the radiation that supplies the required energy to dissociate a mole of iodine molecules, we will use the equation relating energy and wavelength:

Energy (E) = hc/λ

Where:
E is the energy in joules,
h is Planck's constant (6.626 x 10^-34 J·s),
c is the speed of light in a vacuum (2.998 x 10^8 m/s), and
λ is the wavelength of the radiation in meters.

First, let's convert the given energy into joules. We know that 1 kJ = 1000 J, so:

151 kJ = 151,000 J

Now we can rearrange the equation to solve for the wavelength:

λ = hc/E

Substituting the given values:

λ = (6.626 x 10^-34 J·s * 2.998 x 10^8 m/s) / 151,000 J

Calculating the numerator:

λ = (1.989148 x 10^-25 J·m/s) / 151,000 J

Simplifying:

λ = 1.319 x 10^-30 m

Thus, the wavelength of the radiation that supplies the required energy is approximately 1.319 x 10^-30 meters.