Question

A) A red laser pointer emits light with a wavelength of 670 nm. What is the frequency of this light?

Answer 1

Answers:

a) $4.47(10)^{14} Hz$  

b) $178254.16 J$  

c) $2.96(10)^{-19} J$  

Explanation:

a) The following equation states the relation between the wavelength $\lambda$ and the frequency $\nu$ of the light:

$c=\lambda \nu$ (1)

Where:  

$c=3(10)^{8}m/s$ is the speed of light in vacuum

$\lambda=670 nm=670(10)^{-9}m$ is the wavelength of the light emitted by the laser pointer

$\nu$ is the frequency

Finding $\nu$ :

$\nu=\frac{c}{\lambda}$ (2)

$\nu=\frac{3(10)^{8}m/s}{670(10)^{-9}m}$ (3)

$\nu=4.47(10)^{14} Hz$ (4) This is the frequency

b) The energy $E$ of a 670 nm photon is given by:

$E=\frac{hc}{\lambda}$ (5)

Where:  

$h=6.626(10)^{-34}\frac{m^{2}kg}{s}$ is the Planck constant  

Then:

$E=\frac{(6.626(10)^{-34}\frac{m^{2}kg}{s})(3(10)^{8}m/s)}{670(10)^{-9}m}$ (6)

$E=2.96(10)^{-19} J$ (7) This is the energy of one photon

Now we have to find the energy of 1 mole of these 670 nm photons by multiplying (7) by the Avogadro's number ($N_{A}=6.0221(10)^{23}/mol$):

$E N_{A}=(2.96(10)^{-19} \frac{J}{photon})(6.0221(10)^{23}\frac{photon}{mol})$ (8)

$E N_{A}=178254.16 J$ This is the energy of 1 mole of 670 nm photons

c) The ground state of an atom is the point where the energy of the system is zero. This means the ground state energy is $E_{o}=0 J$ and the energy gap $\Delta E$ is:

$\Delta E=E-E_{o}$  

$\Delta E=2.96(10)^{-19} J-0 J=2.96(10)^{-19} J$

Hence, the energy gap has the same value that was already calculated in part b (7), which is the energy of 670 nm photons:

$E=2.96(10)^{-19} J$  

This is the energy of a single 670 nm photon, which is emitted when the excited electrons return to the ground state.  

That is why the wavelength (color) of the light of the laser pointer is 670 nm (red).