The Lyman a line in the hydrogen spectrum has a wavelength of 121.5 nm. Find the change in wavelength of this line in the solar spectrum due to the gravitational shift.
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- When a photon is leaving a gravitational source it will lose energy in the gravitational field. This will shift the frequency of the photon to smaller frequencies.
- The wavelength of such photons will be shifted to a longer wavelength. Such photons are called redshifted.
- The change in wavelength due to gravity is given by,
Here G is the universal gravitational constant, M is the mass of the gravitational source, R is the radius of the gravitational source, and c is the speed of light.
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- Photoelectrons with a maximum kinetic energy of 7.95 eV are emitted from a metal when it is illuminated by ultraviolet radiation with a wavelength of 1.25 × 10-7 m. (i) Calculate the energy of the incident photons in electronvolts. (ii) Calculate the wavelength of the radiation (in nanometres) corresponding to the lowest energy photons that can free electrons from the metal. (iii) How do you explain the fact that, when infrared radiation is shone on this metal, no photoelectrons are emitted?An electron in a Hydrogen atom is in energy level n=5 and drops down into the n=2 level. What is the wavelength of the photon that is emitted in units of nm.In the electrowinning process, a chemical engineer uses an Infrared camera to detect metallurgical Short circuits over the anodes and cathodes. Given that the mass of an electron is 9.109x1031 kg and rydberg's constant is 1.090x107 m-1, determine the energy (in MJ) applied when 5 mol of infrared photons having a wavelength of 32 NM is used in the copper electrolysis process
- The wavelengths for the emission lines observed in the mercury lamp spectra do not match the wavelengths calculated using the Bohr model for the hydrogen atom. Explain why.A hydrogen atom initially in its ground state (n=1) absorbs a photon and ends up in the state for which n = 3. What is the energy of the absorbed photon?The so-called Lyman-a photon is the lowest energy photon in the Lyman series of hydrogen and results from an electron transitioning from the n = 2 to the n = 1 energy level. Determine the energy in eV and the wavelength in nm of a Lyman-a photon. HINT (a) the energy in eV eV (b) the wavelength in nm nm
- For light with a wavelength of 350 nm and with an intensity of /= 10-8 W/m², what is the number of photons/(m²s) in the light beam?H-alpha line is a red visible spectral line in hydrogen atom with a wavelength of 656.3 nm. Consider five distant stars labeled A, B, C, D, and E. The light from these starts was detected on Earth and, after performing spectral analysis, the following H-alpha wavelengths were measured: AA = 667.5 nm, Ag = 650.4 nm, Ac = 653.5 nm, Ap = 660.3 nm, and AE = 664.9 nm. Which star has the slowest speed relative to Earth, in which direction and how fast does it move? The slowest star is? and it moves Select an answer The speed of the slowest star (in km/s), Vslowest = Which star has the fastest speed relative to Earth, in which direction and how fast does it move? The fastest star is? and it moves Select an answer Earth. The speed of the fastest star (in km/s), Vfastest Submit Question = Earth. Units Select an answer ✓ Units Select an answer ✓The wavelength (in nm) of the visible line corresponding to n = 3 in the hydrogen visible spectra (according to Balmer's equation) is:
- Use the following number convention for this question. 1 Red 2 Blue 3 Ultraviolet 4 Violet 5 Infrared 6 Green A student is asked to predict the type of EMR emitted when the electron in a hydrogen atom drops from a higher level to a lower level. The transitions are . n = 8 to n = 5 then the EMR is n = 4 to n = 2 then the EMR is n = 3 to n = 1 then the EMR is n = 3 to n = 2 the the EMR is Which of these students is correct? Student W said 5631 Student X said 3651 Student Y said 1642 Student Z said 4613Energy changes of -1.8167 x 10-19 is recorded when an electron jump from n=6 in an unknown series of hydrogen line spectra. a) calculate the value of nf- [ RH = 2.18 x 10-19]b) identify the line spectra for this radiationIf the energy released by an electron making a transition from one hydrogen atom orbit to another is 4.57 ✕ 10−19 J, what is the wavelength (in nm) of the photon?