Calculate the energy of a photon of electromagnetic radiation?

Question

I have a test today on this and I just need to know how to calculate it step by step the easiest way possible so I can get this conversion down. thanks for the help!

105.9 MHz (typical frequency for FM radio broadcasting) to J

1018 kHz (typical frequency for AM radio broadcasting) to J

834.1 MHz (common frequency used for cell phone communication) to J

Also, How much energy is contained in 1 mol of each?

X-ray photons with a wavelength of 0.110 nm to kJ/mol

γ-ray photons with a wavelength of 2.36 10-5 nm to kJ/mol

Answer 1

Use Planck's equation E = hf for the energy per photon

h = Planck constant (6.625^-34J.s)

f = frequency in Hz (convert the values given in each qu.)



The first 3 are straight forward multiplications



4,5 ..see my previous answer.

Answer 2

The "step-by-step" calculation has only one step. Take the given number and plug it into the formula for energy.



There are two equivalent versions, in terms of frequency or in terms of wavelength.



The energy of a photon of frequency f is E = hf. h = Planck's constant = 6.63 × 10-34 m^2 kg / s, f = frequency in Hz. Answer in Joules.



The energy of a photon of wavelength lambda is E = hc/lambda. c = speed of light = 3.0 x 10^8 m/sec, lambda = wavelength in meters. Answer in Joules.



Oh, and for the ones asking about "a mole", that means compute the energy in Avogadro's Number of photons, which means just multiply E by 6.02 x 10^23.

Answer 3

it rather is a thank you to clean up it: we've: h=6.626*10^-34 j.s (plank consistent) v=102.3 MHz first 102.3 MHz to Hz the end result would be 102.3*10^6 Hz then: locate E=capability E=(h)(v) E=(6.626*10^-34 j.s)(102.3*10^6 Hz) =6.818*10^-26 J