The hydrogen spectrum consists of several spectral lines in Lyman series ( L_1, L_2., L_3 …; L_1 has lowest energy among Lyman series). Similarly it…

The hydrogen spectrum consists of several spectral lines in Lyman series $\displaystyle \left(\mathrm{L}_1, \mathrm{~L}_2\right.$, $\displaystyle \mathrm{L}_3 \ldots ; \mathrm{L}_1$ has lowest energy among Lyman series). Similarly it consists of several spectral lines in Balmer series $\displaystyle \left(\mathrm{B}_1, \mathrm{~B}_2, \mathrm{~B}_3 \ldots ; \mathrm{B}_1\right.$ has lowest energy among Balmer lines). The energy of $\displaystyle \mathrm{L}_1$ is $\displaystyle x$ times the energy of $\displaystyle \mathrm{B}_1$. The value of $\displaystyle x$ is $\displaystyle \_\_\_\_$ $\displaystyle \times 10^{-1}$ . (Nearest integer)