Calculate the wavelength of radiation and energy per mol necessary to ionize a hydrogen atom in the ground state.

Open in App

Solution

Ionization energy of hydrogen atom= $- 13.6 Z^{2} = - 13.6 e V E_{i o n i z a t i o n} = \frac{h c}{λ} \frac{6.626 \times 10^{- 34} \times 3 \times 10^{8}}{λ_{i o n i s a t i o n}} = 13.6 \times 1.6 \times 10^{- 19} λ_{i o n i s a t i o n} = 912 \times 10^{- 8} m$
ionization energy for $1$ mole H= $E_{i o n i z a t i o n} \times N_{A} = 13.6 \times 1.6 \times 10^{- 19} \times 6.023 \times 10^{23} = 1310 k J / m o l e = 1313 k J / m o l (a p p r o x)$

Suggest Corrections

Similar questions

An electromagnetic radiation of wavelength 242 nm is just sufficient to ionize a sodium atom. Calculate the ionization energy of sodium in kJ ${m o l}^{- 1}$ .

Q. The ionization energy of the electron in the hydrogen atom in its ground state is

136 e V

. The atoms are excited to higher energy levels too emits radiation of

6

wavelengths. Maximum wavelength of emitted radiation corresponds to the transition between:

Q. Radiation of wavelength

242

nm is sufficient to ionize the sodium atom. Calculate the ionization of energy in kJ mol

^{- 1}

. (

n = 6.625 \times 10^{- 24}

J-s).

Energy of an electron in the ground state of the hydrogen atom is –2.18 × 10^–18 J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol^–1.

An Electromagnetic radiation of wavelength 242 nm is just sufficient to ionize a sodium atom. Calculate the ionization energy of sodium in kJ ${m o l}^{- 1}$ .

Join BYJU'S Learning Program

Calculate the wavelength of radiation and energy per mol necessary to ionize a hydrogen atom in the ground state.

Ionization energy of hydrogen atom=−13.6Z2=−13.6eVEionization=hcλ6.626×10−34×3×108λionisation=13.6×1.6×10−19λionisation=912×10−8mionization energy for 1 mole H=Eionization×NA=13.6×1.6×10−19×6.023×1023=1310kJ/mole=1313kJ/mol(approx)