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When you talk about the energy of any electromagnetic radiation in terms of its
frequency, you're talking about the energy of a single photon.
8.2 x 1019 J is a bit more than 1,000 times the energy that the Braidwood nuclear
generating station south of Chicago produces in a year.
In order for a single photon to have 8.2 x 1019 J of energy, its frequency would have to be
8.2 x 1019/Planck's Konstant = 8.2 x 1019/6.62608 x 10-34 = 1.2375 x 1053 Hz.
That's about 1034 times the frequency a photon needs in order to be called a
gamma-ray. At that frequency, the wavelength is about 2.422 x 10-45 meter,
and that's something like 10-27 the size of an electron.
Perhaps you meant to type 8.2 x 10minus 19 J.
The frequency of photon with that energy is
8.2 x 10-19/6.62608 x 10-34 = 1.238 x 1015 Hz.
and its wavelength is about 242 nanometers.
That would be a photon in the mid-range ultraviolet.
If you want a beam of light that carries your alleged 8.2 x 10plus 19 J,
you just need more of these photons ... like 1038 of them.
What else can I help you with?
What is the energy of a photon of visible light whose frequency is 8.91x10 to the 14th Hz?
The energy of a photon can be calculated using the formula ( E = h \nu ), where ( E ) is the energy, ( h ) is Planck's constant (( 6.626 \times 10^{-34} , \text{J s} )), and ( \nu ) is the frequency. For a frequency of ( 8.91 \times 10^{14} , \text{Hz} ), the energy ( E ) is approximately ( 5.93 \times 10^{-19} , \text{J} ). This energy falls within the range of visible light, indicating that it corresponds to a color in the visible spectrum.
How are frequency and energy of waves related?
Frequency and energy are related by the following: E = hf where h is Planck's constant, E is the energy in J, and f is the frequency in Hz. Remember that the product of any wavelength and its frequency is equal to the speed of light.
An electron loses 2.5 x 10-15 J of energy and emits a photon What is the frequency of the photon that is emitted?
Photon energy = (Planck's konstant) x (frequency) nu = E / h E = 2.5 x 10-15 J h = 6.626 x 10-34 J-s nu = (2.5 x 10-15 J) / (6.626 x 10-34 J-s) = (2.5 x 10-15 / 6.626 x 10-34) (J / J - s) = 3.773 x 1019 Hz = 3.773 x 1010 GHz
If the photon has a frequency of 4 x 1015 Hz how did the energy of the electron change?
If the change in energy of electron is totally exhibited as a photon then the energy = h times frequency. h = 6.626 x 10 to -34 J s Simply multiply h and frequency you would get the energy in joule
What is the frequency in hertz and the energy in joules of an x-ray photon with a wavelength of 2.32 Å?
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).
What is the frequency of light that has an energy of 2.7 x 10-16 J?
The frequency of light with energy 2.7 x 10^-16 J is f = E/h, where h is Planck's constant (6.626 x 10^-34 J*s). Substituting the values gives a frequency of approximately 4.07 x 10^17 Hz.
What is the energy of a photon the emits a light of frequency 6.42 1014 Hz?
4.25 10-19 j
What is the energy of a photon that emits a light of frequency 4.471014?
The energy of a photon is given by E=hf, where h is Planck's constant (6.626 x 10^-34 J*s) and f is the frequency of light. Thus, the energy of the photon emitting light of frequency 4.471014 Hz is approximately 2.97 x 10^-33 Joules.
What is the energy of a photon that emits a light of frequency 4.47X 1014 Hz?
2.96 x 10^-19 J
What is the energy of a photon that emits a light of frequency 4.47 x 1014 Hz?
2.96 x 10-19 J
What is the energy of a photon that emits a light of frequency energy 7.211014 Hz?
The energy of a photon is given by E = hf, where h is Planck's constant (6.626 x 10^-34 J.s) and f is the frequency of the light. Substituting the given frequency of 7.211014 Hz into the equation, we find that the energy of the photon is approximately 4.79 x 10^-33 J.
How much energy does a 445 nm wave of light have (The speed of light in a vacuum is 3.00 108 ms and Planck's constant is 6.626 10-34 J and bulls.)?
The energy of a photon can be calculated using the formula E = hf, where h is Planck's constant and f is the frequency of the wave. Since frequency = speed of light / wavelength, the energy of a 445 nm wave of light would be approximately 2.79 x 10^-19 J.
What is the energy of a quantum of light with a frequency of 7.39 x 1014 Hz?
The energy of a quantum of light is given by the equation E = hf, where E is the energy, h is Planck's constant (6.626 x 10^-34 J s), and f is the frequency. Substituting the values, the energy of a quantum of light with a frequency of 7.39 x 10^14 Hz would be approximately 4.90 x 10^-19 Joules.
What is the energy of photon that emits a light of frequency (4.47)(10 exponent 14) Hz?
The energy is 2,9619.e-19 J.
What is the energy of a photon that emits a light frequency of 7.21 x 1014 Hz?
The energy of a photon can be calculated using the formula E = hf, where E is the energy, h is Planck's constant (6.626 x 10^-34 J.s), and f is the frequency of the light. Plugging in the values, the energy of a photon emitting a light frequency of 7.21 x 10^14 Hz is approximately 4.85 x 10^-19 J.
What is the energy of a photon of 325nm?
The energy of a photon is determined by the equation E = hf, where E is energy, h is Planck's constant (6.626 x 10^-34 J s), and f is the frequency of the photon. First, calculate the frequency of the photon using the speed of light equation, c = λf. Then, substitute the frequency into the energy equation to find the energy of the photon.
How are frequency and energy of waves related?
Frequency and energy are related by the following: E = hf where h is Planck's constant, E is the energy in J, and f is the frequency in Hz. Remember that the product of any wavelength and its frequency is equal to the speed of light.
