CameraIcon

SearchIcon

MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Bohr's Model of a Hydrogen Atom

Calculate the...

Question

Calculate the ionisation energy of the hydrogen atom. How much energy will be required to ionise $1$ mole of hydrogen atoms? Given, that the Rydberg constant is $1.0974 \times 10^{7} m^{- 1}$ .

Open in App

Solution

$I E$ per hydrogen atom $= 2.182 \times 10^{- 18} J$
$I E$ per mole $= 1314$ $k J$ ${m o l}^{- 1}$ .

Suggest Corrections

thumbs-up

0

Similar questions

Q. The ionisation potential of hydrogen atoms is

13.6 e V

. How much energy need to be supplied to ionise the hydrogen atom in the first excited state?

Q. If the electron in a hydrogen atom were in the energy level with

n = 3

, how much energy in joule would be required to ionise the atom? (Ionisation energy of

H -

2.18 \times 10^{- 18} J

Q. The ionisation potential of hydrogen atom is

13.6 e V

. The energy required to remove an electron from the second orbit of hydrogen will be

Q. The energy difference and the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from the energy level n = 4 to the energy level n =3, given that value of Rydberg constant is 1.0974

\times

^{- 7}

^{- 1}

Q. The ionisation energy of hydrogen atom is 13.6 eV. What will be the ionisation energy of

L i^{2 +}

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Bohr's Model of a Hydrogen Atom

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Bohr's Model of a Hydrogen Atom

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon