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Energy of the photon = Planck's constant x frequency of the ultraviolet radiation
E = h x f
frequency of the ultraviolet radiation = speed of light / wavelength of the ultraviolet radiation
f = c/ lambda
E = 6.63 x 10-34 x 3 x 108 / 3 x 10-7 = 6.63 x 10-19 Joules
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∙ 13y ago
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∙ 9y agoUltraviolet light is a form of radiation that is an invisible part of the electromagnetic spectrum. The energy of a photon of 320 nm ultraviolet light is 6.20764x10-19 Joules.
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∙ 14y agoE_photon=h*f=h*c/wavelength. c =speed of light, h= plank's constant. This gives a value of about 6.2eV
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∙ 14y agoThe energy is E=hc/w= .2E-24/120E-9 = 1.67E-18 Joules.
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∙ 11y agoThe energy is hc/w = 1.25 uevm/,4um =3.125 ev.
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∙ 15y ago1590.24 x 1043 joule
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∙ 10y agoI believe it would be 9.939e-22
Aiyana Garibay
4.44 x 10-19
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When an electron in atom changes energy states a photon is emitted If the photon has a wavelength of 550 nm how did the energy of the electron change?
electron lost 3.6 x 10-19 -barbie=]
What is the wavelength of a photon with an energy of 3.26 10 19 J?
The wavelength is 610 nm.
What colour is light of a wavelength 700nm?
The formula for frequency is f = c/lambda, where c is the speed of light in a vacuum, lambda is the wavelength in meters, and f is frequency in cycles per second. So, if the wavelength is 700.5 nm, the frequency is 4.28 E14 hertz.
A ground-state H atom absorbs a photon of wavelength 94.91 nm and its electron attains a higher energy level?
This will result in the hydrogen atom being in an excited state. The electron must absorb enough energy from the photon to make it into the next energy level. An electron cannot stay 'in between' energy levels. The amount of energy in a photon is given by: E = h*c/lambda [c = speed of light = 3 x 108 m/s; lambda = wavelength in meters; and h = Plancks constant = 4.14 x 10-15 eV*s {eV - electron volt is a unit of energy}] With lambda = 94.91 nm = 94.91 x 10-9 meters; we have E = 13.09 eV From the chart of hydrogen energy levels: 1 -13.61eV 2 -3.4eV 3 -1.51eV 4 -0.85eV 5 -0.54eV it looks like 13.09 eV will be enough to take the electron from level 1 (ground state) up to level 5, but no farther. The exited atom will not stay excited for long and as the electron falls back to it's normal state, it gives off a photon with corresponding energy. I think hydrogen will just go straight back to level 1, but some elements, the electron can jump from level 5 to 4, then 4 to 3, etc. giving off multiple photons with corresponding energy for each photon. See related links.
What is the energy of photon emitted with wavelength of 654 nm?
c = lambda * nunu = c/lambda E = h* nu E = h * c/lambda = 6.626x10^-34 J-sec * 3x10^8 m/sec / 6.54x10^-7 m E = 3.04x10^-27 J
What is the energy of a 500 nm photon?
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.
A photon has a wavelength 628 nm. Calculate the energy of the photon in joules?
The energy of the photon is 3,1631.e-19 joule.
What is the frequency and energy of a photon with a wavelength of 488.3 nm?
89
The energy of a 200 nm photon in eV is?
3.5 I am positive
Transition A produces light with a wavelength of 400 nm Transition B involves twice as much energy as A What wavelenth light does it produce?
Energy per photon is proportional to frequency. That tells us that it's alsoinversely proportional to wavelength.So if Photon-A has wavelength of 400-nm, then wavelength of Photon-Bwith twice as much energy is 200-nm .
How do you calculate the energy in joules of a photon of green light having a wavelength of 529 nm?
The energy of this photon is 3,7351.10e-19 joules.
What is the wavelength of a photon that has three times as much energy as that of a photon whose wavelength is 779 nm?
Photon energy is proportional to frequency ==> inversely proportional to wavelength.3 times the energy ==> 1/3 times the wavelength = 779/3 = 2592/3 nm
What is the wavelength of a photon with an energy of 3.26 10-19?
610 nm
What is the wavelength of a photon with an energy of 4.56 J?
The wavelength is 436 nm.
What is the wavelength of a photon whose energy is twice that of a photon with a 580 nm wavelength?
Twice the energy means twice the frequency, and therefore half the wavelength.
Energy of a photon with the wavelength 425 nm?
4.7*10^-19 j
What is the energy of a photon emitted with a wavelength of NM?
4.44 10-19 j
