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What is the wavelength in nm of a photon whose energy is 4.7 x 10-14 J?
Wiki User
∙ 9y ago
First get the wavelength in meters by multiplying Plancks constant (in units of J-sec) times the speed of light (in m/sec) and divided by the energy. Then change to nanometers by multiplying by 1 billion.
Wiki User
∙ 15y ago
Wiki User
∙ 8y ago0,0042265 nm
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What is the energy per photon of a light source if it has a wavelength of 460 nm?
The standard equation here is E=nhf. E is energy, n is number of photons, h is Planck's Constant, and f is frequency. For a single photon you can get rid of the 'n', so it looks like E=hf. For this problem, you first have to convert the wavelength to frequency. This is done by dividing the speed of the wave per second (i.e., the speed of light), by the wavelength. This is (3*108 m/sec)/(4.60*10-7 m) which simplifies to 6.52*1014/sec. Now all you have to do is multiply the frequency by Planck's constant, which is 6.626068 × 10-34 m2 kg/s. So, (6.626068 × 10-34 m2 kg/s) * (6.52*1014/sec) = 4.3202*10-19 kg m2/s2 or 4.3202*10-19 Joules. If you want proper significant figures, then the answer is 4.3*10-19 Joules. Note: 4.3x10-19 joules equals 2.7 eV (electron volts)
What is the energy of a photon that emits a light of frequency 4.47 10 14 Hz?
The energy is 2,9619.e-19 J.
What is the energy of a photon with a wavelength of 518 nm?
2.8x10-19 JE = hν, and ν = c/λ. λ is wavelength, c is the speed of light (3.0 x 108 meters/second), E is energy, and h is 6.626 x 10-34. 3.0 x 108/715 = 419580.42. 419580.42 x 6.626 x 10-34 = 2.78 x 10-28 joules.
How long is one exameter?
1018 meters = one quintillion meters = 1 billion billion meters = about 110 light yearsAbout 6.2 * 1014 miles
What is 250000000 in scientific notation?
250,000,000 in Scientific Notation is: 2.5*10^8
How to Put these photons in order of increasing energy?
A photon with energy 3.0 x 10-19 J A photon with wavelength 525 nm A photon with frequency 7.6 x 1014 Hz A photon with frequency 2 x 1015 Hz
What the wavelength of a photon with a frequency of 7.81 x 1014 Hz?
384 nm (apex)
What is the frequency of a photon with an energy of 3.26 10 -19 J?
The frequency of the photon is 4.92 1014 Hz.
What is the wavelength of a photon with a frequency of 6.901014 hz?
Wavelength = 3 x 108 / 6.9 *1014 lambda = 4.35*10-7 m Almost the colour seems to be violet.
What is the energy of a photon the emits a light of frequency 6.42 1014 Hz?
4.25 10-19 j
What is the energy of a photon of green light with a frequency of 5.89 1014 s-1?
3.905x10^-19 J
What is the energy of a photon that emits a light of frequency 4.47X 1014 Hz?
2.96 x 10^-19 J
What is the energy of a photon that emits a light frequency of 7.21 x 1014 Hz?
4.78 x 10-19
What are the colors in order of increasing wavelength?
The longest wavelengths of light are the lowest frequencies (and the lowest energy and the longest period, too). These are the reds, and moving up the spectrum, we encounter orange, yellow, green, blue and violet. The violet light has the shortest wavelength (highest frequency), and the highest energy. The infrared (IR) is below the red (longer wavelength and lower frequency), and the ultraviolet (UV) is above the violet (shorter wavelength and higher frequency).
The barium atom has an emission with wavelength 554 nm green Calculate the frequency of this light and the energy of a photon of this light?
- frequency of this light : c=ln, so n=c/l (and remembering that 1 nm = 1 x10-9 m) = (3.00 x 108 m/s)/554x 10-9 m) = 5.42 x 1014 1/s - the energy of a photon of this light: E(photon) = hn = (6.6262 x 10-34 J·s)(5.42 x 1014 1/s) = 3.59 x 10-19 J
What is the wavelength associated with a frequency of 2.06 x 1014 hz?
The wavelength is (speed of the wave) / 2.06 x 1014 .If the wave is an electromagnetic one propagating through vacuum,then the wavelength is3 x 108 / 2.06 x 1014 = 0.001456 millimeter = 1,456 nanometer (rounded)
What is the wavelength of a light of frequency 4.47 X 1014 Hz?
The wavelength is 671 nm.
