What is the wavelength of light associated with the radiation of 7.26 x 10-19 J/photon? (h = 6.63 x 10-34 J • s)
E = hc/wavelength.
Solve for wavelength.
Solve this equation for wavelength:
E = 7.26 x 10-19 J = h c /(wavelength)
c is the speed of light, 3.00*10^8 m/s
Thanks guys, brain fart i guess. I wasn't putting together the E=7.26e-19
Well, they say hindsight is 20/20, but for this question, let's focus on the wavelength instead! To find the wavelength of light associated with that radiation, we can use the relationship between energy and frequency. Since we know the energy per photon is 7.26 x 10-19 J, we can plug that into the famous equation E = hf (where h is Planck's constant) to find the frequency. Then, we can use the speed of light equation (c = λf) to find the wavelength. It's like putting together a puzzle, but much less frustrating. So, let's get those wavelengths crackin'!
To find the wavelength of light associated with the given energy of 7.26 x 10^-19 J/photon, you can use the equation:
E = hc/λ
Where:
E is the energy of the photon (7.26 x 10^-19 J/photon)
h is Planck's constant (6.63 x 10^-34 J • s)
c is the speed of light in a vacuum (approximately 3.00 x 10^8 m/s)
λ is the wavelength of light
First, rearrange the equation to solve for the wavelength, λ:
λ = hc/E
Now, substitute the given values into the equation:
λ = (6.63 x 10^-34 J • s) * (3.00 x 10^8 m/s) / (7.26 x 10^-19 J/photon)
Perform the multiplication and division:
λ = (1.89 x 10^-25 J • m • s) / (7.26 x 10^-19 J/photon)
Simplify:
λ = 2.60 x 10^-7 m
Therefore, the wavelength of light associated with the given energy is approximately 2.60 x 10^-7 meters.