Upon exposure to sunlight, nitrogen dioxide degrades into nitrogen monoxide and oxygen radicals. Through a very lengthy process, this breakdown leads to the formation of acid rain $($nitric acid$)$ and toxic ozone in the troposphere. The specific frequency of light responsible for the breakdown of nitrogen dioxide is $7\mathrm{.}143$ x $10^14$ Hz$.$

a$)$ What is the wavelength $($in nm$)$ of this frequency of light?

b$)$ With this frequency of light, how much energy $($in kJ$)$ is required to break down $24\mathrm{.}0$ g nitrogen dioxide?