Question

calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n=4 to the n=1 principal energy level. E=-2.18x10^-18 J(1/n^2)

Constants (c = 2.9979 | 109 m/s; h = 6.626 | 10 " J[s) 1. What is the energy in joules of a mole of photons with visible light of wavelength 486 nm? (246 kJ) 2. Calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n= 1 principal energy level. E = -2.18 | 10" J(1/n) (97.2 nm)

Answer 1

o Given daveleryth, x = 486 nm. Energy og Enersy a 1 photon = he 1 photon = hc Choplanch constant - ( speedy liget] Enery & 1 photon = 6.626x10²4 + 3x108 486% 10-9 -17 xlo Energo y - 0.041 J I are g photon = 0.041x16" x 6.022x10 23 = 0.246 X 106 J. or 246 kj .

given from transitim from Rydberg en no=4 to na where do wavelength Rut Z Rydberg atomic constant number ] for H, Z=1 to Rype [ <=R* [ da li se & we know t = 91.2 nmt K = 16x 91.2 mm, = 97.2 mm mm