Light that has a frequency of about 4.43 1014 Hz (a wavelength of about 683 nm) appears red to our eyes. What is the energy in joules of the photons associated with this light?
To calculate the energy of the photons associated with this light, we can use the formula:
E = hf
Where E is the energy of the photon, h is Planck's constant (6.626 x 10^-34 J*s), and f is the frequency of the light.
Given that the frequency of the light is 4.43 x 10^14 Hz, we can plug this value into the formula:
E = (6.626 x 10^-34 J*s) * (4.43 x 10^14 Hz)
E = 2.939 x 10^-19 Joules
Therefore, the energy of the photons associated with this light is approximately 2.939 x 10^-19 Joules.