Calculate the energy in kj/mol of photon in red light of wavelength 656nm
E = hc/wavelength
wavelength = 656E-9 m
E will be in J/photon.
Convert to kJ knowing 1 kJ = 1000 J.
There are 6.02E23 photons in a mole of phonts
Post your work if you get stuck.
To calculate 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)
λ (lambda) is the wavelength of the light in meters
First, let's convert the wavelength from nanometers to meters:
656 nm = 656 x 10^-9 meters = 6.56 x 10^-7 meters
Now, let's substitute the values into the equation:
E = (6.626 x 10^-34 J-s * 3.00 x 10^8 m/s) / (6.56 x 10^-7 meters)
Let's calculate it:
E ≈ 3.02 x 10^-19 J
To convert this energy into kilojoules per mole (kJ/mol), we need to multiply by Avogadro's number, which is approximately 6.022 x 10^23 mol^-1.
E = (3.02 x 10^-19 J) * (1 kJ / 1000 J) * (1 mol / 6.022 x 10^23)
Let's calculate it:
E ≈ 5.02 x 10^-5 kJ/mol
Thus, the energy of a single photon in red light with a wavelength of 656 nm is approximately 5.02 x 10^-5 kilojoules per mole (kJ/mol).