What in tarnation is a "mole" of photons ???
Don't you have to know the atomic number or the molecular weight of an element or compound
in order to know the size of a mole ?
Do you happen to know the atomic number or the molecular weight of a Photon ???
I don't think Avogadro was talking about photons.
You were going along so nicely there, and it seemed that you were just about to specify a wavelength, when suddenly the circuit went silent. If I want to work with the question, then, I'll have to invent my own plausible wavelength.
You DID mention 'visible' light. Without looking anything up, let's say that the visible wavelength band is 400nm to 750 nm. Then the center of the band is 548 nm, and the corresponding frequency is c/5.48 x 10^-9 Hz.
The energy of each photon is hf .
h = 6.63 x 10^-34 joule-sec.
You want a mol of them, so that's 6.022 x10^23 .
Finally the energy is (6.022 x 10^23) (c/ 5.48 x 10^-9 ) = 3.294 x 10^40 joules.
You asked for the energy in kilojoules, so that's 3.294 x 10^37 kilojoules.
This is, shall we say, a fair amount of energy. In fact, a seriously not-insignificant quantity of the stuff.
I'm reminded of the humble LED, with 1.5 volts of forward bias, conducting 15 mA, and pouring out red light with 75% efficiency. In order to accumulate the above amount of energy in the form of visible light, you would need to collect and energize something like 1.95 million trillion trillion trillion of these LEDs. All I can say to you is: Don't stand in front of them, and if you do, then remember not to look directly at them.
First calculate the frequency: c = wavelength x frequency
3x10^8 m/s = 7x10^-7 m x frequency
frequency = 4.3x10^14 s^-1
Next, calculate the energy: E = planck's constant x frequency
E = 6.63x10^-34 J/s x 4.3x10^14 s^-1
E = 2.85x10^-19 J <---ANSWER
Light of 700 nm has an energy of 171 kj/mol.
The energy of a single photon of red light with a wavelength of 700,0 nm is 1,7712 eV.
1.710x105 J/mol
246kJ
The shorter the wavelength of visible light, the higher the frequency and the greater the energy of the photons.
UV photons have more energy (less wavelength, higher frequency) than visible light photons. It is possible to convert photons to ones with less enery, but not the opposite.
High-energy photons correspond to short-wavelength light while low-energy photons correspond to long-wavelength light. In short, the answer is red. For short-wavelengths (high energy photons) it would appear blue.
Photons do not come in different types like infared-photons etc. they are just the wavelength that the photons are at and nuclear fusion just happens to emit photons at a particular wavelength
To calculate the number of photons, you need the formula E=hf where h is Planck's constant with a value of 6.63*10^-34Js and f should be given. If f isn't given, then use the formula C = f * wavelength. Rearrange this formula by using the wavelength given and the C, speed of light, which is 3*10^8. You should get C/wavelength = f, which will then be placed into E=hf => answer. What you also need is the Intensity. This way you obtain the photon flux as: I/E (i.e. the number of photons per unit area and unit time).
The energy of the photons decreases as the wavelength increases
Photons (energy packets of light)
289nm
... have roughly double the energy of photons of red light, because their frequency is roughly double the frequency of red-light photons. (That also means that their wavelength is roughly half the wavelength of red-light photons, but this fact doesn't help the current discussion at all.)
Energy of light photons is related to frequency as Energy = h(Planck's constant)* frequency Frequency = velocity of wave / wavelength So energy = h * velocity of the wave / wavelength
They are inversely proportional or relationship to each other.
Shortest wavelength means the highest frequency, meaning the photons have the highest energy. That is color violet. The violet light colors the skin brown. Red light with lower energy photons cannot do that.
The shorter the wavelength of visible light, the higher the frequency and the greater the energy of the photons.
Light of is made up of a finite number of photons, or light quanta. The energy of each photon is proportional to the frequency of the light, and hence inversely proportional to the wavelength of the light. Red light has a longer wavelength than blue light, so the quantum of red light has less energy than the quantum of blue light.
UV photons have more energy (less wavelength, higher frequency) than visible light photons. It is possible to convert photons to ones with less enery, but not the opposite.
High-energy photons correspond to short-wavelength light while low-energy photons correspond to long-wavelength light. In short, the answer is red. For short-wavelengths (high energy photons) it would appear blue.
2.012 x 10^(16)