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Calculate the energy emitted when electron of 1.0 gm atom of Hydrogen undergo transition giving the spectrtal lines of lowest energy is visible region of its atomic spectra. Given that, `R_(H)`=`1.1xx10^(7) m^(-1)`,` c=3xx10^8m//sec`,` h=6.625xx10^(-34) Jsec`.

Text Solution

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The transition occurs like Balmer series as spectral line is observed in visible region.
Thus, the line of lowest energy will be observed when transition occurs from 3rd orbit to 2nd orbit, i.e., `n_(1)=2 and n_(2)=3`.
`(1)/(lamda)=R[(1)/(2^(2))-(1)/(3^(2))]=(5)/(36)R`
`E=hv=h*(c)/(lamda)=6.62xx10^(-34)xx3xx10^(8)xx(5)/(36)xx1.1xx10^(7)`
`=3.03xx10^(-19)J` per atom
Energy correspond to 1.0 g atom of hydrogen
`=3.03xx10^(-19)xx`Avogardro's number
`=3.03xx10^(-19)xx6.023xx10^(23)J`
`=18.25xx10^(4)J`.
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