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If the energy of 1.00 mole of photons is 346 kJ what is the wavelength of the light?
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∙ 10y ago
289nm
Wiki User
∙ 10y ago
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What is the numbers of photons of light with a wavelength of 4000 pm that provide 1 j of energy?
If a certain source emits radiation of a wavelength of 400 nm then the energy in a mole of photons of this radiation can be found using E = hc/w. The energy in kJ/mol of a mole of these photons is approximately 300 kJ / mole.
What is the energy difference between orbitals that give rise to the emission of excited rubidium atoms emitting red light with a wavelength of 795 nm?
Use the equation E=(hcNA)/λ Where h is Planck's constant, c is the speed of light, NA is Avogadro's number, and λ is the wavelength given. Also, remember to convert from nm to m. The answer is 151 KJ/mole.
The energy of one photon of light from electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye?
E=hc/l h=plank's constant c=speed of light l=wavelength [(6.626*10^34)(3*10^8)]/(5.50*10^-7)= 3.614*10^-19 for per mole (3.614*10^-19)*(6.022*10^23)= 2.18*10^5 muliply by .001 for kilojoules =2.18*10^2 or just 218 kj/mole
How many kilocalories of energy is released when one mole of fat is oxidized?
one mole of fat releases how much energy
Energy in one mole of glucose in joules?
2870 KJ (per mole)
What is the numbers of photons of light with a wavelength of 4000 pm that provide 1 j of energy?
If a certain source emits radiation of a wavelength of 400 nm then the energy in a mole of photons of this radiation can be found using E = hc/w. The energy in kJ/mol of a mole of these photons is approximately 300 kJ / mole.
How do you calculate the energy content of photons in moles?
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).
How many moles of photons with a wavelength of 660 nm are needed to provide 6 kJ of energy?
The energy carried by a photon is given byE = hfWhere h is Planck's constant (6.626x10^-34 Joule-seconds) and f is the frequency of the photon in Hertz (Hz).We are given the wavelength of the photon in the question in nanometers (nm). First, we need to convert this to (SI) units, because our equations only work with SI units. Then, we will calculate the frequency of the photon from its wavelength. Once we know the frequency of the photon we're interested in, we simply use the equation above to find the energy carried by one of them. Then we divide 6 kJ by that amount of energy, and the quotient will be the number of photons needed to carry 6 kJ. Finally, when we know the number of photons we need, we divide by the number of photons in a mole to get the number of moles.The SI unit of length is the meter (m). 1nanometer (nm) is 10^-9 meters.660 nm = 660 *10^-9 m = 6.6*10^-7 m.Now we will calculate this photon's frequency from its wavelength. These are related by the equationc = fLwhere c is the speed of light (3*10^8 m/s), f is the frequency of the photon and L is the wavelength of the photon.c = fL(3*10^8 m/s) = f * (6.6*10^-7 m)solving for f, we havef = (3*10^8 m/s) / (6.6*10^-7 m) = 4.54*10^15 s^-1Note that the unit of seconds (s) raised to the -1power is defined as 1 Hertz (Hz).f = 4.54*10^15 HzNow we will use the top equation to solve for the energy carried by one photon having this frequency.E = hfE = (6.626*10^-34 Js) * (4.54*10^15 Hz)E = 1.369*10^-17 JThis is how much energy is carried by one photon of wavelength 660 nm (which will also have a frequency of 4.54*10^15 Hz).How many of these do we need to provide 6 kJ? This is solved by simple division. Keeping in mind that 1 kJ = 1000 J, we haveNumber of photons * Energy per photon = 6 kJNumber of photons * (1.369*10^-17 J/photon) = 6 kJNumber of photons * (1.369*10^-17 J/photon) = 6000 JNumber of photons = 6000 J / (1.369*10^-17 J/photon)Number of photons = 4.382*10^20 photonsThis is how many photons (at this frequency) are needed to provide 6 kJ. How many moles of photons is this?Number of photons / number of photons in a mole = number of molesRecall that a mole of something is defined as 6.02*10^23of it. The same way a dozen eggs is defined as 12 eggs, a mole of eggs is 6.02*10^23 eggs. Equivalently, a mole of photons is 6.02*10^23 photons. SoNumber of photons / (6.02*10^23 photons per mole) = number of moles(4.382*10^20 photons) / (6.02*10^23 photons per mole) = number of moles7.279*10^-4 moles = number of molesForgive me if my arithmetic is off, as I don't have a good calculator handy. However, I believe this is the correct method to use.
What is the energy (in joules) of an ultraviolet photon with wavelength 180nm?
1.11 atto Joules.
How do you calculate energy per mole of photons if you know joules per photon?
You have to multiply the joules/photon by Avogadro's Number, i.e., by the number of particles in a mole.
What is the energy difference between orbitals that give rise to the emission of excited rubidium atoms emitting red light with a wavelength of 795 nm?
Use the equation E=(hcNA)/λ Where h is Planck's constant, c is the speed of light, NA is Avogadro's number, and λ is the wavelength given. Also, remember to convert from nm to m. The answer is 151 KJ/mole.
What is the energy content kJ per mol of a mole of photons of red light with a wavelength of 700 nm?
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 compoundin 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.
What is one mole of photon?
A Mole of anything is avogadros number of particles which is 6.022 x 10^23. So a mole of Photos is 6.002 x 10^23 number of photons.
The energy of one photon of light from electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye?
E=hc/l h=plank's constant c=speed of light l=wavelength [(6.626*10^34)(3*10^8)]/(5.50*10^-7)= 3.614*10^-19 for per mole (3.614*10^-19)*(6.022*10^23)= 2.18*10^5 muliply by .001 for kilojoules =2.18*10^2 or just 218 kj/mole
How does the sun give energy to a mole that lives underground?
the food moles eat can give the mole its energy
The amount of energy required to remove one mole of electrons from one mole of sodium atoms is the?
ionization energy
Ionization energy of a helium atom is helium gas per mole?
the first inoization energy is 2372.3 kJ mol-1 there are 6.0221415 × 10^23 in a mole from avagadros number, devide the ionization energy for one mole by the number of atoms in a mole and you get the first ionization energy for one atom.
