Question

How much energy (in kj) do 3.0 moles of photons, all with a wavelength of 665 nm, contain?

Answer 1

548kj because The energy in joules of a single photon of wavelength λ in meters is:
E = hc/λ
(6.63x10^-34 J·s) (3x10^8 m/s) / (655 nm) (1x10^-9 m/nm) = 3.03x10^-19 J.
The energy in kilojoules of 3 moles of photons of this wavelength is:
(3.03x10^-19 J) (6.02x10^23 /mol) (3.0 mol) / (1000 J/kJ) = 548 kJ

Answer 2

The energy in kilojoules of a single photon of wavelength λ is 548kJ.

What is wavelength?

The wavelength is the distance between the corresponding crest or trough of the mechanical wave.

The energy of a photon is given by

E = hc/λ

where h is the Planck's constant, c is the speed of light and λ is the wavelength of the wave.

Substitute the values provided in the question, we get

E = (6.63x10⁻³⁴ J·s) (3x10⁸ m/s) / (655 x10⁻⁹ m)

E = 3.03x10⁻¹⁹ J.

The energy of 3 moles of photons of this wavelength in kilojoules is:

3.03x10⁻¹⁹ J x 6.023 x 10²³/mol x  3.0 mol / 1000

E(kJ) = 548 kJ

Thus, the energy in kilojoules of a single photon of wavelength λ is 548kJ.

Learn more about wavelength.

https://brainly.com/question/13533093

#SPJ2