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6.67 x 10^11 Hz
384 nm (apex chemistry 2023)
Ultraviolet radiation has a wavelength between 10 and 400 nanometers. The shorter the wavelength, the more energy each photon contains. To find the frequency, divide the speed of light (299,792,458 metets per second) by the wavelength.
Wavelength = 3 x 108 / 6.9 *1014 lambda = 4.35*10-7 m Almost the colour seems to be violet.
The easiest way would be to find a descriptive article on the internet that shows the visible colors spread out with some wavelengths labeled. There, you can find the approximate wavelengths for light of various colors. If you don't know the color of the light, then in order to find its wavelength, you'd need to know either its frequency or the energy of a photon (quantum). Energy of a photon = h f h = Planck's Konstant = about 6.63 x 10-34 joule-second f = frequency of the light wave or photon But the frequency is (speed of light)/(wavelength) so, Energy = h c/wavelength . If you know either the energy of the photon or its frequency, you can use this stuff to find its wavelength. In this discussion, I've toggled back and forth a few times between the frequency/wavelength of the quantum and the frequency/wavelength of the light wave. Don't worry. They're the same.
6.67 x 10^11 Hz
c = wavelength X frequency, where c is the speed of light, which is 299,792,458 m/s. So you need the wavelength of the photon. Then you divide c/wavelength and the result will be the frequency.
384 nm (apex chemistry 2023)
A photon with energy 3.0 x 10-19 J A photon with wavelength 525 nm A photon with frequency 7.6 x 1014 Hz A photon with frequency 2 x 1015 Hz
For the frequency, first convert the wavelength to meters (divide the number of Angstroms by 1010), then use the formula: wavelength x frequency = speed. Using the speed of light in this case. Solving for frequency: frequency = speed / wavelength. To get the photon's energy, multiply the frequency times Planck's constant, which is 6.63 x 10-34 (joules times seconds).
Ultraviolet radiation has a wavelength between 10 and 400 nanometers. The shorter the wavelength, the more energy each photon contains. To find the frequency, divide the speed of light (299,792,458 metets per second) by the wavelength.
Wavelength = 3 x 108 / 6.9 *1014 lambda = 4.35*10-7 m Almost the colour seems to be violet.
Use this formula to find frequency. Frequency (Hertz) = (3.29 X 10^15 Hz)*Z^2*(1/nf^2 - 1/ni^2) use this to find wavelength Wavelength = speed of light/frequency in Hz Now, you need to know what the Z number (atomic number-Carbon = 6, for instance ) is of the element that generated the photon of light.
The easiest way would be to find a descriptive article on the internet that shows the visible colors spread out with some wavelengths labeled. There, you can find the approximate wavelengths for light of various colors. If you don't know the color of the light, then in order to find its wavelength, you'd need to know either its frequency or the energy of a photon (quantum). Energy of a photon = h f h = Planck's Konstant = about 6.63 x 10-34 joule-second f = frequency of the light wave or photon But the frequency is (speed of light)/(wavelength) so, Energy = h c/wavelength . If you know either the energy of the photon or its frequency, you can use this stuff to find its wavelength. In this discussion, I've toggled back and forth a few times between the frequency/wavelength of the quantum and the frequency/wavelength of the light wave. Don't worry. They're the same.
Use the principle that the wavelength of the photon in meters x the frequency in Hz = the speed of light.Convert nm to m.543nm = 5.43 x 10-7mEquation:c = ƒ•λ, where c is the speed of light in a vacuum, 3.00 x 108 m/s, f is the frequency in Hz, and λ is the wavelength in meters.To solve for frequency, do the following:ƒ = c/λ = (3.00 x 108m/s)/(5.43 x 10-7m) = 5.52 x 1014Hz
The frequency of the photon is 4.92 1014 Hz.
Energy of photon = Plank's ConstantXVelocity of light/Wavelength = h*c/lambda Put the values to get the answer.