Problem: Hydrogen gas absorbs light of wavelength 103nm. Afterward, what wavelengths are seen in the emission spectrum?

FREE Expert Solution

Energy of absorbed photon:

E=hcλ=(6.626×10-34)(3×108)103×10-9

E = 1.93 × 10-18J = (1.93 × 10-18)/(1.6 × 10-19) = 12.06 eV

After absorbing this photon, hydrogen undergoes a transition to a higher state n with energy (-13.6/n2) from the ground state that initially had the energy  (-13.6/12)

To get n:

[(-13.6/n2) -  (-13.6/12)] = 12.06

13.6/n2 = 1.54

n = sqrt (13.6/1.54) = 3.

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Problem Details

Hydrogen gas absorbs light of wavelength 103nm. Afterward, what wavelengths are seen in the emission spectrum?

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