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To answer you first question: First we need the energy of one photon. Assuming you are familiar with the two formulae E=hf and c=fl where: c=speed of light /m.s^-1 | h= Planck constant / Js l=wavelength /m | f=frequency / Hz E= Energy / J we can substitute to get E=hc/l l = 320nm = 320 x10^-9 m | E = 6.626 x10^-34 Js | c=3 x10^8 m.s^-1 so E=(6.626 x10^-34 x 3 x10^8)/(320 x10^-9) = 6.211875 x10^-19 [seems believable so far] One mole = 6.02 x10^23 So total energy of a mole of the photons is: 6.02 x10^23 x 6.211875 x10^-9 = 373954.875 J = 374 kJ (3 s.f.) --------- As for the second question: http://en.wikipedia.org/wiki/Ultraviolet#Subtypes there you can see the relative wavelenghts of different types of UV light. UVA = 400-320nm | UVB = 320-200nm Now, looking again at the equation E=hc/l It is clear that to maximise E, we want the smallest l (to divide hc by the smallest number) Therefore shorter wavelength photons have the highest energy, so the answer is UV-B
The energy of a photon can be calculated using the equation 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, the energy of a photon with a wavelength of 300 nm is approximately 6.62 x 10^-19 joules.
We can use the Plank's Law:
E = hf = hc / λWhere
h is Plank's constant (7 x 10-34 J/s)[approx.]
c is the speed of light in a vacuum (3 x 108 m/s)
λ is the wavelength, in meters, of the photon you're measuring
E = [ (7 x 10-34)(3 x 108) ] / 3 x 10-9 m
E = [ 21 x 10-26 ] / 3 x 10-9 m
E = 7 x 10-19 J
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What is the wavelength of a photon whose energy is twice that of a photon with a 580 nm wavelength?
Since the energy of a photon is inversely proportional to its wavelength, for a photon with double the energy of a 580 nm photon, its wavelength would be half that of the 580 nm photon. Therefore, the wavelength of the photon with twice the energy would be 290 nm.
What is the frequency and energy of a photon with a wavelength of 488.3 nm?
The frequency of a photon with a wavelength of 488.3 nm is approximately 6.15 x 10^14 Hz. The energy of this photon is approximately 2.54 eV.
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 energy of a photon of orange light that has a wavelength of NM?
To determine the energy of a photon of orange light with a wavelength of 600 nm, we can use the formula E = hc/λ, where E is the energy of the photon, 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 in meters. Converting the wavelength to meters (600 nm = 600 x 10^-9 m), we can plug the values into the formula to find the energy of the photon. The energy of a photon of orange light with a wavelength of 600 nm is approximately 3.31 x 10^-19 joules.
What is the wavelength of a photon with an energy of 3.26 x 10-19 J?
The wavelength can be calculated using the equation E = hc/λ, where E is the energy of the photon, h is Planck's constant, c is the speed of light, and λ is the wavelength. Plugging the given energy value into the equation and solving for λ gives a wavelength of approximately 608 nm.
What is the wavelength of a photon whose energy is twice that of a photon with a 580 nm wavelength?
Since the energy of a photon is inversely proportional to its wavelength, for a photon with double the energy of a 580 nm photon, its wavelength would be half that of the 580 nm photon. Therefore, the wavelength of the photon with twice the energy would be 290 nm.
What is the frequency and energy of a photon with a wavelength of 488.3 nm?
The frequency of a photon with a wavelength of 488.3 nm is approximately 6.15 x 10^14 Hz. The energy of this photon is approximately 2.54 eV.
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
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?
Transition B produces light with half the wavelength of Transition A, so the wavelength is 200 nm. This is due to the inverse relationship between energy and wavelength in the electromagnetic spectrum.
What is the wavelength of a photon with an energy of 3.26 10-19?
610 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 energy of a photon of orange light that has a wavelength of NM?
To determine the energy of a photon of orange light with a wavelength of 600 nm, we can use the formula E = hc/λ, where E is the energy of the photon, 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 in meters. Converting the wavelength to meters (600 nm = 600 x 10^-9 m), we can plug the values into the formula to find the energy of the photon. The energy of a photon of orange light with a wavelength of 600 nm is approximately 3.31 x 10^-19 joules.
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?
The energy of the electron decreased as it moved to a lower energy state, emitting a photon with a wavelength of 550 nm. This decrease in energy corresponds to the difference in energy levels between the initial and final states of the electron transition. The energy of the photon is inversely proportional to its wavelength, so a longer wavelength photon corresponds to lower energy.
What is the wavelength of a photon that has Energy of 4 x 10 to the -17 power?
4.9695 nm
What is the wavelength of a photon with an energy of 3.26 x 10-19 J?
The wavelength can be calculated using the equation E = hc/λ, where E is the energy of the photon, h is Planck's constant, c is the speed of light, and λ is the wavelength. Plugging the given energy value into the equation and solving for λ gives a wavelength of approximately 608 nm.
What is the energy of a photon emitted with a wavelength of 518 mp?
The energy of a photon can be calculated using the equation E = hc/λ, where h is Planck's constant, c is the speed of light, and λ is the wavelength. Plugging in the values, the energy of a photon with a wavelength of 518 nm is approximately 3.82 eV.
What is the energy of a photon emitted with wavelength of 518 nm?
3.84 x 10-19 joules.
