2.21x10-18j
The energy of a 500 nm photon is 3.1 eV (electron volts). This is a unit of measure used to represent the energy of a single photon. To put this into perspective, a single photon of visible light has an energy of 1.8 to 3.1 eV, and a single photon of ultraviolet light has an energy of 3.1 to 124 eV. The energy of a 500 nm photon can be calculated by using the following equation: E = hc/ Where: E = energy of the photon (in eV) h = Planck's constant (6.626 * 10-34 Js) c = speed of light (2.998 * 108 m/s) = wavelength of photon (in meters) Therefore, the energy of a 500 nm photon is calculated as follows: Convert the wavelength from nanometers to meters: 500 nm = 0.0005 m Insert the values into the equation: E = (6.626 * 10-34 Js) * (2.998 * 108 m/s) / (0.0005 m) Calculate the energy: E = 3.1 eVTherefore, the energy of a 500 nm photon is 3.1 eV.
Planck's Equation,E = hvWhere E is the energy contained within the photon of light, h is Plank's constant, and v is the frequency of the light.Planck's constant, h, = 6.626068 X 10 ^ -34 J s and frequency of light = speed of light / wavelengththis is not only used in light but also to find energy of all electromagnetic radiation
The relationship between wavelength and energy on the electromagnetic spectrum is inverse: shorter wavelengths correspond to higher energy, while longer wavelengths correspond to lower energy. This means that gamma rays, which have the shortest wavelengths, have the highest energy, while radio waves, which have the longest wavelengths, have the lowest energy.
The energy of a photon is given by the equation E = hc/λ, where h is Planck's constant, c is the speed of light, and λ is the wavelength of the photon. Plugging in the values, a photon with a wavelength of 350 nm would have an energy of approximately 3.56 eV.
The wavelength of a photon can be calculated using the formula: λ = c / f, where λ is the wavelength, c is the speed of light (3.00 x 10^8 m/s), and f is the frequency of the photon. Plugging in the values, we get λ = 3.00 x 10^8 m/s / 6.901014 Hz ≈ 4.350 x 10^7 meters.
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.
The energy of a 500 nm photon is 3.1 eV (electron volts). This is a unit of measure used to represent the energy of a single photon. To put this into perspective, a single photon of visible light has an energy of 1.8 to 3.1 eV, and a single photon of ultraviolet light has an energy of 3.1 to 124 eV. The energy of a 500 nm photon can be calculated by using the following equation: E = hc/ Where: E = energy of the photon (in eV) h = Planck's constant (6.626 * 10-34 Js) c = speed of light (2.998 * 108 m/s) = wavelength of photon (in meters) Therefore, the energy of a 500 nm photon is calculated as follows: Convert the wavelength from nanometers to meters: 500 nm = 0.0005 m Insert the values into the equation: E = (6.626 * 10-34 Js) * (2.998 * 108 m/s) / (0.0005 m) Calculate the energy: E = 3.1 eVTherefore, the energy of a 500 nm photon is 3.1 eV.
The wavelength is 610 nm.
The relationship between wavelength and energy on the electromagnetic spectrum is inverse: shorter wavelengths correspond to higher energy, while longer wavelengths correspond to lower energy. This means that gamma rays, which have the shortest wavelengths, have the highest energy, while radio waves, which have the longest wavelengths, have the lowest energy.
Planck's Equation,E = hvWhere E is the energy contained within the photon of light, h is Plank's constant, and v is the frequency of the light.Planck's constant, h, = 6.626068 X 10 ^ -34 J s and frequency of light = speed of light / wavelengththis is not only used in light but also to find energy of all electromagnetic radiation
The wavelength of a photon can be calculated using the formula: λ = c / f, where λ is the wavelength, c is the speed of light (3.00 x 10^8 m/s), and f is the frequency of the photon. Plugging in the values, we get λ = 3.00 x 10^8 m/s / 6.901014 Hz ≈ 4.350 x 10^7 meters.
The energy per photon of infrared radiation can be calculated using the formula E = hc/λ, where h is the Planck's constant (6.626 x 10^-34 J·s), c is the speed of light (3 x 10^8 m/s), and λ is the wavelength in meters. Converting the wavelength to meters (25 micrometers = 25 x 10^-6 meters), we can plug the values into the formula to calculate the energy per photon. This results in E ≈ 7.95 x 10^-20 Joules per photon.
You know that,E = h*c/λWhereh = Plank's constant = 6,626 x 10-34 J*sc = speed of light = 3*108 m/sλ = greek letter lambda representing the wavelength =624nm => 6,24 *10-7mand therefore [(6.626 X 10^-34 J) X (3 X 10^8 m/s)] / (6.24 x 10^-7) = 3.18 x 10^-19 ... That should be right!
You can use Plank's relation to calculate the energy of the absorbed photon.E = h.f = h.c/LgivenE = Energy of a photon in Joulesf = frequency of the photon in s-1c = speed of light in m/sL = wavelength of the photon in metreh = Planck constant = 6.62606957×10−34 J.s
The energy of a photon can be calculated using the formula E = hc/λ, where 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), and λ is the wavelength. Plugging in the values, we get E = (6.626 x 10^-34 J·s * 3.00 x 10^8 m/s) / (495 x 10^-9 m) ≈ 4.01 x 10^-19 J.
The energy of a photon can be calculated using the formula E = (hc) / λ, where E is energy, h is Planck's constant, c is the speed of light, and λ is wavelength. Plugging in the values gives E = (6.626 x 10^-34 Js * 3 x 10^8 m/s) / (550 x 10^-9 m) = 3.62 x 10^-19 Joules.
As the frequency of photons increases, the energy of the photons increases proportionally. This means that higher frequency photons have higher energy levels. Additionally, higher frequency photons have shorter wavelengths according to the wave-particle duality of light.