For the first line 1.097 10-2 nm-1 |5? = \\ \: \\ \: \frac{1}{\lambda} =0.000247 \: nm^{-1} \\ \: \\ \: \lambda = 4051 \: nm For the second line \frac{1}{\lambda} = 1.097 \times 10^{-2} \: nm^{-1} \left [ \frac{1}{4^2} -\frac{1}{6^2} ight ] \\ \: \\ \: \frac{1}{\lambda} =0.000381 \: nm^{-1} \\ \: \\ \: \lambda = 2625 \: nm Part B For the first line \\ \: \\ \: E = \frac{hc}{\lambda} \\ \: \\ \: E = 6.626 \times 10^{-34} \: Js \times 3 \times 10^8 \: m/s \times 0.000247 \: nm^{-1} \times 10^9 \: nm/m \\ \: \\ \: E = 4.91 \times 10^{-20} \: J This is for one atom. For one mole of atoms E = 4.91 10-2 J/atom 6.023 1023 atoms/mol E = 29551 J/mol Convert the unit from J to kJ kJ 1 1000 J E = 29551 J/mol E = 29.55 kJ / mol For the second line \\ \: \\ \: E = \frac{hc}{\lambda} \\ \: \\ \: E = 6.626 \times 10^{-34} \: Js \times 3 \times 10^8 \: m/s \times 0.000381 \: nm^{-1} \times 10^9 \: nm/m \\ \: \\ \: E =7.57 \times 10^{-20}