🤓 Based on our data, we think this question is relevant for Professor Tezcan's class at UCSD.

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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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Particle Nature of Light concept. You can view video lessons to learn The Particle Nature of Light. Or if you need more The Particle Nature of Light practice, you can also practice The Particle Nature of Light practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Tezcan's class at UCSD.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.