Calculate energy in "KJ" when electrons of "0.05" gram atom of hydrogen undergo transition giving the spectral line of lowest energy in the visible region of its atomic spectrum

Calculate the energy emitted when electrons of 1.0 g atom of hydrogen undergo transition giving the spectral line of largest energy in the visible region of its atomic spectrum. (R_H = 1.1 xx 10^7 m^(-1), c = 3 xx 10^8 m s^(-1), h = 6.62 xx 10^(-34) J s)

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 .

Find the energy released (in erg) when 2.0 g atom of hydrogen undergoes transition giving a spectral line of the lowest energy in the visible region of its atomic spectra

The energy of n^(th) orbit is given by E_(n) = ( -Rhc)/(n^(2)) When electron jumpsfrom one orbit to another orbit then wavelength associated with the radiation is given by (1)/(lambda) = RZ^(2)((1)/(n_(1)^(2)) - (1)/ (n_(2)^(2))) When electron of 1.0 gm atom of Hydrogen undergoes transition giving the spectral line of lowest energy is visible region of its atomic spectra, the wavelength of radiation is

Calculate the energy emitted when electrons of 1.0 g 1 of hydrogen transition giving spectrum lines of the lowest in the visible regain of its atomic spectrum R_(H) = 1.1 xx 10^(7) m^(-1) , c= 3 xx 10^(8) m s^(-1) and h = 6.62 xx 10^(-34) J s

Calculate the energy of the electron in the ground state of the hydrogen atom.

Which of the following series in the spectrum of the hydrogen atom lies in the visible region of the electromagnetic spectrum