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