the atomic spectrum of lithium has a strong red line at 670.8 nm. what is the energy of each photon of this wave length? What is the energy of 1 mole of these photons??
igfaj
To determine the energy of a photon, you can use the equation:
E = hc/λ
where E is the energy of the photon, h is Planck's constant (6.626 x 10^-34 J·s), c is the speed of light (3.00 x 10^8 m/s), and λ is the wavelength of light.
Let's calculate the energy of each photon with a wavelength of 670.8 nm:
First, convert the wavelength from nanometers (nm) to meters (m):
λ = 670.8 nm = 670.8 x 10^-9 m
Now substitute the values into the equation:
E = (6.626 x 10^-34 J·s) * (3.00 x 10^8 m/s) / (670.8 x 10^-9 m)
Simplifying the equation:
E = 2.960 x 10^-19 J
So, the energy of each photon with a wavelength of 670.8 nm is approximately 2.960 x 10^-19 Joules.
To calculate the energy of 1 mole (Avogadro's number, N_A = 6.022 x 10^23) of these photons, you can multiply the energy of each photon by Avogadro's number:
Energy of 1 mole = (2.960 x 10^-19 J) * (6.022 x 10^23)
Calculating this:
Energy of 1 mole = 1.779 x 10^5 J/mol
Thus, the energy of 1 mole of photons with a wavelength of 670.8 nm is approximately 1.779 x 10^5 Joules per mole.