Color wavelength, nm

Violet 380 – 450 nm

Blue 450 – 495 nm

Green 495 – 570 nm

Yellow 570 – 590 nm

Orange 590 – 620 nm

Red 620 – 750 nm

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

where:

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

**v** = frequency (in s^{–1})

**Solve for ****v****:**

$\frac{\mathbf{E}}{\mathbf{h}}\mathbf{=}\frac{\overline{)\mathbf{h}}\mathbf{v}}{\overline{)\mathbf{h}}}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\mathbf{v}\mathbf{=}\frac{\mathbf{E}}{\mathbf{h}}\mathbf{=}\frac{\mathbf{2}\mathbf{.}\mathbf{961}\mathbf{\times}{\mathbf{10}}^{\mathbf{-}\mathbf{19}}\mathbf{}\overline{)\mathbf{J}}}{\mathbf{6}\mathbf{.}\mathbf{626}\mathbf{\times}{\mathbf{10}}^{\mathbf{-}\mathbf{34}}\mathbf{}\overline{)\mathbf{J}}\mathbf{\xb7}\mathbf{s}}$

Heated lithium atoms emit photons of light with an energy of 2.961 × 10^{−19} J. Calculate the frequency and wavelength of one of these photons. What is the total energy in 1 mole of these photons? What is the color of the emitted light?

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