0
I assume you mean 4 X 10^-17 Joules.
Energy = Planck's constant * speed of light/wavelength in meters
4 X 10^-17 Joules = (6.626 X 10^-34 J*s)(2.998 X 10^8 m/s)/wavelength
wavelength in meters = (6.626 X 10^-34)(2.998 X 10^8)/(4 X 10^-17)
= 4.9662 X 10^-9 meters
or
4.97 nanometers
Add your answer:
Earn +20 pts
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?
To determine the frequency of a photon, you can use the equation E = hf, where E is the energy of the photon, h is Planck's constant (6.626 x 10^-34 Js), and f is the frequency. If the wavelength of the photon is given, you can use the equation c = λf, where c is the speed of light (3.00 x 10^8 m/s), λ is the wavelength, and f is 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
How many moles of photons with a wavelength of 660 nm are needed to provide 6 kJ of energy?
To calculate the number of moles of photons needed, first convert the energy to joules (1 kJ = 1000 J). Then use the energy of a single photon formula (E = hc/λ) to calculate the energy of one photon. Finally, divide the total energy needed by the energy of one photon to find the number of photons, and then convert it to moles.
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.
