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)

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm.

A. 4.85x10^{-19} J

B. 2.06x10^{-19} J

C. 8.13x10^{-19} J

D. 1.23x10^{-19} J

E. 5.27x10^{-19} J

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