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.
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.
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 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
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).
The energy of the photons released during an atomic emission spectrum can be calculated using the equation (E = h \nu), where (E) is the energy of the photon, (h) is Planck's constant ((6.626 \times 10^{-34} , \text{J s})), and (\nu) is the frequency of the emitted light. The frequency can be related to the wavelength ((\lambda)) of the light using the equation (\nu = \frac{c}{\lambda}), where (c) is the speed of light ((3.00 \times 10^8 , \text{m/s})). By measuring the wavelength of the emitted light, you can determine its frequency and subsequently calculate the energy of the photons.
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.
4.25 10-19 j
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.
2.96 x 10^-19 J
2.96 x 10-19 J
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.
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.
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.
The energy is 2,9619.e-19 J.
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.
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.
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.