Light emitted by sodium vapor lamps (like those on highway 30 outside BHS) has a

Question

Light emitted by sodium vapor lamps (like those on highway 30 outside BHS) has a wavelength (lambda) of 5.89 times 10^2 nm. Calculate the frequency of this radiation in Hz. Determine the energy in joules (J) of one photon of this radiation. Determine the energy in joules (J) of one mole of photons which have this wavelength. In what region of the light spectrum (IR, UV, visible, x-ray etc.) is this radiation found? Consider the following Bohr diagram for the hydrogen atom in its ground state (Even though the Bohr atom is a classical (not quantum mechanical) model, it very nicely explains the hydrogen atom spectrum). Draw a Bohr picture where the electron has been excited to the third Bohr orbit. Does the original atom absorb or emit energy to create this excited atom (circle one)? Assume that the exited atom in part A returns to the original state (ground state). Would energy be absorbed or emitted by this process (circle one)? Assume that one of the following transitions gives red light and the other gives light in the UV region. Label the appropriate picture with the appropriate "kind" of light and explain how you inferred your answer.

Explanation / Answer

1)
wavelength = 5.89*10^2 nm = 5.89*10^-7 m
a)
f = c/wavelength
= (3*10^8) / (5.89*10^-7)
= 5.09*10^14 Hz

b)
E = h*f
= (6.626*10^-34)*(5.09*10^14)
= 3.37*10^-19 J

c)
E for 1 mol = 3.37*10^-19 * 6.022*10^23
= 2.03*10^5 J/mol

d)
it is in visible region

i am allowed to answer only 1 question at a time. Please ask other as different question

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