356560 For wavelength of visible radiation of hydrogen spectrum Balmer gave an equation as \(\lambda = \frac{{\left( {k{m^2}} \right)}}{{\left( {{m^2} - 4} \right)}}\), where '\(m\)' is principal quantum number of energy level. The value of \(k\) in terms of Rydberg's constant \(R\) is

356561 An electron of stationary hydrogen atom jumps from 4\(th\) energy level to ground level. The velocity that the photon acquired as a result of electron transition will be ( where \(H = \) Planck’s constant, \(R = \) Rydberg’s constant, \(m = \) mass of photons)

356562 The wavelength of the first line of Lyman series for hydrogen atom is equal to that of the second line of Balmer series for a hydrogen like ion. The atomic number Z of hydrogen-like ion is

356563 The radiation emitted when an electron jumps from \({n}=3\) to \({n}=2\) orbit in a hydrogen atom falls on a metal to produce photoelectrons. Find the work function of the metal, when maximum kinetic energy of ejected electron is \(1.376 \times 10^{-19} {~J}\).

356560 For wavelength of visible radiation of hydrogen spectrum Balmer gave an equation as \(\lambda = \frac{{\left( {k{m^2}} \right)}}{{\left( {{m^2} - 4} \right)}}\), where '\(m\)' is principal quantum number of energy level. The value of \(k\) in terms of Rydberg's constant \(R\) is

356561 An electron of stationary hydrogen atom jumps from 4\(th\) energy level to ground level. The velocity that the photon acquired as a result of electron transition will be ( where \(H = \) Planck’s constant, \(R = \) Rydberg’s constant, \(m = \) mass of photons)

356562 The wavelength of the first line of Lyman series for hydrogen atom is equal to that of the second line of Balmer series for a hydrogen like ion. The atomic number Z of hydrogen-like ion is

356563 The radiation emitted when an electron jumps from \({n}=3\) to \({n}=2\) orbit in a hydrogen atom falls on a metal to produce photoelectrons. Find the work function of the metal, when maximum kinetic energy of ejected electron is \(1.376 \times 10^{-19} {~J}\).

356560 For wavelength of visible radiation of hydrogen spectrum Balmer gave an equation as \(\lambda = \frac{{\left( {k{m^2}} \right)}}{{\left( {{m^2} - 4} \right)}}\), where '\(m\)' is principal quantum number of energy level. The value of \(k\) in terms of Rydberg's constant \(R\) is

356561 An electron of stationary hydrogen atom jumps from 4\(th\) energy level to ground level. The velocity that the photon acquired as a result of electron transition will be ( where \(H = \) Planck’s constant, \(R = \) Rydberg’s constant, \(m = \) mass of photons)

356562 The wavelength of the first line of Lyman series for hydrogen atom is equal to that of the second line of Balmer series for a hydrogen like ion. The atomic number Z of hydrogen-like ion is

356563 The radiation emitted when an electron jumps from \({n}=3\) to \({n}=2\) orbit in a hydrogen atom falls on a metal to produce photoelectrons. Find the work function of the metal, when maximum kinetic energy of ejected electron is \(1.376 \times 10^{-19} {~J}\).

356560 For wavelength of visible radiation of hydrogen spectrum Balmer gave an equation as \(\lambda = \frac{{\left( {k{m^2}} \right)}}{{\left( {{m^2} - 4} \right)}}\), where '\(m\)' is principal quantum number of energy level. The value of \(k\) in terms of Rydberg's constant \(R\) is

356561 An electron of stationary hydrogen atom jumps from 4\(th\) energy level to ground level. The velocity that the photon acquired as a result of electron transition will be ( where \(H = \) Planck’s constant, \(R = \) Rydberg’s constant, \(m = \) mass of photons)

356562 The wavelength of the first line of Lyman series for hydrogen atom is equal to that of the second line of Balmer series for a hydrogen like ion. The atomic number Z of hydrogen-like ion is

356563 The radiation emitted when an electron jumps from \({n}=3\) to \({n}=2\) orbit in a hydrogen atom falls on a metal to produce photoelectrons. Find the work function of the metal, when maximum kinetic energy of ejected electron is \(1.376 \times 10^{-19} {~J}\).