Problem: 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?

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

FREE Expert Solution

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

E=hv (1)


where:

h = Planck’s constant (6.626 × 10–34 J • s)

v = frequency (in s–1)


Solve for v:

Eh=hvhv=Eh=2.961×10-19 J6.626×10-34 J·s

View Complete Written Solution
Problem Details

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?

Frequently Asked Questions

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.