If the energy of a photon is 1.32 x 10-18 J, what is its wavelength in nm?

Answer 1

E= hf
frequency f = speed of light c/wavelength of light lambda
1 nm = 10^-9 m.
1.32*10^-18 J ~ (6.626*10^34 J*s) *c/wavelength (lambda)
Wavelength (lambda) ~ (6.626*10^-34 J*s * 3.00*10^8 m./s.)/(1.32*10^-18 J.)

~ 1.506 *10^-7 m. = 150.6 nm.

Not to nag, but you should probably learn how to do this on your own.

Hope that helps.

Source(s): I am a physics student

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