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

Answer:

4.79 J

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:

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