Establish the relationship of energy and wavelength then calculate the energy of a photon that has a wavelength of 476.4 nm

Recall that the ** energy of a photon (E)** is given by:

$\overline{){\mathbf{E}}{\mathbf{=}}{\mathbf{hv}}}\left(1\right)$

where:

**h** = Planck’s constant (6.626 × 10^{–34} J • s)

**v** = frequency (in s^{–1})

Also, recall that the frequency (v) and wavelength (λ) are related:

$\overline{){\mathbf{\lambda}}{\mathbf{=}}\frac{\mathbf{c}}{\mathbf{v}}}\left(2\right)$

where:

**c** = speed of light (3.0 × 10^{8} m/s)

Visible light has wavelengths of roughly from 400 to 700 nm. If a certain color has a wavelength of 476.4 nm, what is the energy of one of its photons in J? Once you have the value, take it log (base 10) and enter that with three decimal places as your answer. Do not enter units.

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