0
The energy of one photon can be calculated using the equation E = hc/λ, where h is the Planck's constant, c is the speed of light, and λ is the wavelength. Plugging the values into the equation, we get E = (6.626 x 10^-34 J s * 3 x 10^8 m/s) / (100 x 10^-9 m) = 1.986 x 10^-18 J. Since there are Avogadro's number of photons in a mole, the energy of one mole of photons would be 1.986 x 10^-18 J * 6.022 x 10^23 = 1.195 x 10^6 J/mol.
What else can I help you with?
If the energy of 1.00 mole of photons is 346 kJ what is the wavelength of the light?
To find the wavelength of the light, you can use the energy-wavelength relationship given by E = hc/λ, where E is the energy, h is Planck's constant, c is the speed of light, and λ is the wavelength. Rearrange the formula to solve for λ: λ = hc/E. Substitute the values for h, c, and the energy of 1.00 mole of photons to calculate the wavelength.
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 of a mole of photons of red light with a wavelength of 632nm?
The energy of a photon can be calculated using the formula E = hc/λ, where h is Planck's constant, c is the speed of light, and λ is the wavelength of light. Plugging in the values, we find that the energy of a single photon of red light with a wavelength of 632nm is approximately 3.1 x 10^-19 Joules. To find the energy of a mole of these photons, you simply multiply this value by Avogadro's number (6.022 x 10^23) to get approximately 1.9 x 10^5 Joules.
What is the energy of one photon of violet light?
The energy of one photon of violet light is around 3.1 electronvolts (eV) or equivalently about 500 kilojoules per mole (kJ/mol). Violet light has a shorter wavelength and higher frequency compared to other visible light colors, resulting in higher energy 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
If the energy of 1.00 mole of photons is 346 kJ what is the wavelength of the light?
To find the wavelength of the light, you can use the energy-wavelength relationship given by E = hc/λ, where E is the energy, h is Planck's constant, c is the speed of light, and λ is the wavelength. Rearrange the formula to solve for λ: λ = hc/E. Substitute the values for h, c, and the energy of 1.00 mole of photons to calculate the wavelength.
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 of a mole of photons of red light with a wavelength of 632nm?
The energy of a photon can be calculated using the formula E = hc/λ, where h is Planck's constant, c is the speed of light, and λ is the wavelength of light. Plugging in the values, we find that the energy of a single photon of red light with a wavelength of 632nm is approximately 3.1 x 10^-19 Joules. To find the energy of a mole of these photons, you simply multiply this value by Avogadro's number (6.022 x 10^23) to get approximately 1.9 x 10^5 Joules.
How do you calculate energy per mole of photons if you know joules per photon?
To calculate the energy per mole of photons from the energy per photon, you need to multiply the energy per photon by Avogadro's number (6.022 x 10^23) to account for the number of photons in a mole. The formula is: Energy per mole of photons = Energy per photon x Avogadro's number.
What is the energy (in joules) of an ultraviolet photon with wavelength 180nm?
1.11 atto Joules.
What is one mole of photon?
One mole of photons would contain approximately 6.022 x 10^23 photons. This number is known as Avogadro's number and represents the number of particles in one mole of any substance. Each photon carries energy and has characteristics of both particles and waves.
What is the energy of one photon of violet light?
The energy of one photon of violet light is around 3.1 electronvolts (eV) or equivalently about 500 kilojoules per mole (kJ/mol). Violet light has a shorter wavelength and higher frequency compared to other visible light colors, resulting in higher energy photons.
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.
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 much energy (in kJ) do 3.0 moles of photons all with a wavelength of 675 nm contain?
To calculate the energy of photons, we can use the formula (E = \frac{hc}{\lambda}), where (h) is Planck's constant ((6.626 \times 10^{-34} , \text{J s})), (c) is the speed of light ((3.00 \times 10^8 , \text{m/s})), and (\lambda) is the wavelength in meters (675 nm = (675 \times 10^{-9} , \text{m})). First, calculate the energy of one photon, then multiply by the number of moles (using Avogadro's number, (6.022 \times 10^{23} , \text{photons/mole})). Calculating this gives: Energy of one photon: [ E = \frac{(6.626 \times 10^{-34} , \text{J s})(3.00 \times 10^8 , \text{m/s})}{675 \times 10^{-9} , \text{m}} \approx 2.94 \times 10^{-19} , \text{J} ] Total energy for 3.0 moles of photons: [ \text{Total energy} = 3.0 , \text{moles} \times (6.022 \times 10^{23} , \text{photons/mole}) \times (2.94 \times 10^{-19} , \text{J}) \approx 5.34 \times 10^{5} , \text{J} ] Convert to kJ: [ 5.34 \times 10^{5} , \text{J} \div 1000 \approx 534 , \text{kJ} ] Thus, 3.0 moles of photons at 675 nm contain approximately 534 kJ of energy.
How does the sun give energy to a mole that lives underground?
the food moles eat can give the mole its energy
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
