Final answer:
To find the energy and frequency of radiation with a wavelength of 2.0x10^-7 m, use the formulas E = hc/λ for energy and f = c/λ for frequency. Then, convert the photon energy to kJ/mol using Avogadro's number.
Step-by-step explanation:
The student is asking to calculate the energy (in kJ/mol) and frequency of radiation with a given wavelength of 2.0x10-7 meters. To calculate the energy E of a photon, we can use the formula E = hc/λ, where h is Planck's constant (6.626x10-34 J s), c is the speed of light (3x108 m/s), and λ is the wavelength of the radiation. After calculating the energy of one photon in joules, we can then convert this energy to kilojoules per mole (kJ/mol) by multiplying by Avogadro's number (6.022x1023 mol-1) and then dividing by 1000 to convert joules to kilojoules.
To calculate the frequency (f) of the radiation, we can use the formula f = c/λ. Substituting the given values will provide the frequency in hertz (Hz).