Find the wavelength of light, in nanometers (nm), given off from a sample of light containing 3.72 x 10-19J of energy.  Hint: convert Joules to Hertz(frequency) then frequency to wavelength.

To find the wavelength of light, we can use the equation E = hf, where E is the energy of the light, h is Planck's constant, and f is the frequency of the light.

First, we need to convert the energy from Joules to Hertz. We can use the equation E = hf to solve for f. Rearranging the equation, we have f = E/h.

Given that the energy is 3.72 x 10^-19 J and Planck's constant is approximately 6.626 x 10^-34 J·s, we can substitute these values into the equation to find the frequency.

f = (3.72 x 10^-19 J) / (6.626 x 10^-34 J·s) f ≈ 5.61 x 10^14 Hz

Now that we have the frequency, we can use the equation c = λf, where c is the speed of light and λ is the wavelength of the light. Rearranging the equation, we have λ = c/f.

The speed of light is approximately 3.00 x 10^8 m/s. Converting this to nanometers, we get 3.00 x 10^17 nm/s.

λ = (3.00 x 10^17 nm/s) / (5.61 x 10^14 Hz) λ ≈ 5.35 x 10^2 nm

Therefore, the wavelength of the light emitted from the sample is approximately 535 nm.