Multiple Choice
Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm. Use the formula E = hc/λ, where h = 6.626 x 10^-34 J·s and c = 3.00 x 10^8 m/s.
9. Quantum Mechanics
The Energy of Light
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Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
How many photons are contained in a burst of yellow light (589 nm) from a sodium lamp that contains 609 kJ of energy?
A
4.12 x 10^25 photons
B
3.02 x 10^23 photons
C
7.50 x 10^22 photons
D
1.85 x 10^24 photons
Verified step by step guidance1
First, understand that the energy of a photon can be calculated using the equation: , where is Planck's constant (), is the speed of light (), and is the wavelength of the light.
Convert the wavelength from nanometers to meters. Since 1 nm = meters, the wavelength nm is meters.
Calculate the energy of a single photon using the formula: . Substitute the values for , , and to find the energy of one photon.
Determine the number of photons by dividing the total energy of the burst by the energy of a single photon. Use the formula: , where is the total energy (609 kJ, converted to joules) and is the energy of one photon.
Convert the total energy from kilojoules to joules by multiplying by 1000, since 1 kJ = 1000 J. Then, perform the division to find the number of photons in the burst of yellow light.
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