Energy of absorbed photon:

$\begin{array}{rcl}\mathbf{E}& \mathbf{=}& \frac{\mathbf{h}\mathbf{c}}{\mathbf{\lambda}}\\ & \mathbf{=}& \frac{\mathbf{(}\mathbf{6}\mathbf{.}\mathbf{626}\mathbf{\times}{\mathbf{10}}^{\mathbf{-}\mathbf{34}}\mathbf{)}\mathbf{(}\mathbf{3}\mathbf{\times}{\mathbf{10}}^{\mathbf{8}}\mathbf{)}}{\mathbf{103}\mathbf{\times}{\mathbf{10}}^{\mathbf{-}\mathbf{9}}}\end{array}$

E = 1.93 × 10^{-18}J = (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/n^{2}) from the ground state that initially had the energy (-13.6/1^{2})

To get n:

[(-13.6/n^{2}) - (-13.6/1^{2})] = 12.06

13.6/n^{2} = 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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