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What else can I help you with?
What is the wavelength of a photon that has Energy of 4 x 10 to the -17 power?
4.9695 nm
What is 17-4 10 equals 23?
(17-4)+10=23 13+10=23
A-3 plus 17 equals 10?
a - 3 + 17 = 10 Therefore, a - 3 = -7 a = -4
What is the answer for 8 over 17 divided by 4 over 5?
8/17 ÷ 4/5 = 40/68 which can be simplfied to 10/17.
What is 40 multiplied by 170?
40 x 170 = 4 x 10 x 17 x 10 which equals 4 x 17 x 10 x 10 which becomes 4 x 17 x 100 = 68 x 100 = 6800 Or, you can multiply 4x17, then put two zeroes on the end.
What is the wavelength of a photon that has Energy of 4 x 10 to the -17 power?
4.9695 nm
An electron requires 4 x 10-17 J of energy to be removed from its atom What is the wavelength of a photon that has this much energy?
4.8 - 5.2 nm
That An electron requires 4 times 10-17 j of energy to be removed from it's atom what is the wavelength of a photon that has this much energy?
The wavelength is w = hc/E = .2E-24/4E-17 = 5E-9 meters.
What is the frequency associated with the photon of microwave radiation that has a wavelength of 10-4 m?
The frequency of the photon can be calculated using the equation: frequency = speed of light / wavelength. Given that the speed of light is approximately 3 x 10^8 m/s, the frequency for a microwave photon with a wavelength of 10^-4 m would be approximately 3 x 10^12 Hz.
What frequency does a photon of wavelength 4.5 x 10-4m have?
The frequency of a photon is given by the equation f = c/λ, where c is the speed of light (3 x 10^8 m/s) and λ is the wavelength of the photon. Plugging in the values, we find that the frequency of a photon with a wavelength of 4.5 x 10^-4 m is approximately 6.67 x 10^14 Hz.
What frequency does a photon of wavelength 4.5x10-4 m have?
The frequency of a photon can be calculated using the equation: frequency = speed of light / wavelength. Plugging in the speed of light (3 x 10^8 m/s) and the given wavelength (4.5 x 10^-4 m) gives a frequency of 6.67 x 10^14 Hz.
What are the frequency and wavelength of the photon?
c = wavelength X frequency, where c is the speed of light, which is 299,792,458 m/s. So you need the wavelength of the photon. Then you divide c/wavelength and the result will be the frequency.
What is the wavelength of a photon that will induce a transition from the ground state to the n equals 4 state in hydrogen?
The wavelength of the photon can be calculated using the Rydberg formula: 1/λ = R(1/4^2 - 1/n^2), where R is the Rydberg constant. Substituting n=4, the calculation gives a wavelength of approximately 97.2 nm.
What frequency does a photon of wavelength 4.5 10-4 m have?
Frequency = speed/wavelength = 299,792,458/4.5 x 10-4 = 666.21 GHz . (rounded)
An electron requires 3.8 x 10-19 J of energy to be removed from its atom What is the wavelength of a photon that has this much energy?
5.10 x 10^14 hz
What is the approximate energy of a photon having a frequency of 4 107 hz?
The energy of a photon can be calculated using the formula E = hf, where h is Planck's constant (6.626 x 10^-34 J·s) and f is the frequency of the photon. Plugging in the values, the energy of a photon with a frequency of 4 x 10^7 Hz is approximately 2.65 x 10^-26 Joules.
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.
