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`.

Calculate the energy emitted when electron of 1.0 gm atom of Hydrogen

1.	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`.
Answer» Correct Answer - `182.5 kJ` `E=13.6[1/n_(1)^(2)-1/n_(2)^(2)]eV//atom rArr E=13.6[(9-4)/36] eV//atom` `E=13.6[(9-4)/(36)]xx6.023xx10^(23)xx1.6xx10^(-19) rArr 182.5 kJ`

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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`.

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