Question

For the wave of light you generated in the Part B, calculate the amount of energy in 1.0 mol of photons with that same frequency (1.2×1010 Hz ) and wavelength (0.026 m ). Recall that the Avogadro constant is 6.022×1023 mol−1.

Answer 1

4.79 J

Step-by-step explanation:

The energy of a single photon is given by

`E=hf`

where

`h=6.63\cdot 10^(-34) Js` is the Planck constant

f is the frequency of the photon

Here we have

`f=1.2\cdot 10^(10) Hz`

so the energy of one photon is

`E_1=(6.63\cdot 10^(-34))(1.2\cdot 10^(10))=7.96\cdot 10^(-24) J`

Here we have 1 mol of photons, which contains

`N=6.022\cdot 10^(23)` photons (Avogadro number). So, the total energy of this mole of photons is:

`E=NE_1 = (6.022\cdot 10^(23))(7.96\cdot 10^(-24))=4.79 J`