Atomic StructureHard
Question
The energy required by electrons, present in the first Bohr orbit of hydrogen atom to be excited to second Bohr orbit is $\_\_\_\_$ $J{mol}^{- 1}$.
Given : $R_{H} = 2.18 \times 10^{- 11}$ ergs.
Options
A.$1.635 \times 10^{- 18}$
B.$9.835 \times 10^{5}$
C.$9.835 \times 10^{12}$
D.$1.635 \times 10^{- 11}$
Solution
$E_{n} = - R_{H} \times \frac{Z^{2}}{n^{2}}$
$$\Delta E = 2.18 \times 10^{- 11} \times 10^{- 7} \times 1^{2}\left\lbrack \frac{1}{1^{2}} - \frac{1}{2^{2}} \right\rbrack $$$= 1.635 \times 10^{- 18}$ Joule/atom
$= 1.635 \times 10^{- 18} \times 6.02 \times 10^{23}$ Joule $/$ mole
$= 9.835 \times 10^{5}$ Joule $/$ mole
Create a free account to view solution
View Solution FreeMore Atomic Structure Questions
The distance of closest approach of an α-particle fired towards a nucleus with momentum ‘P’ is r. What will be the dista...The amount of energy released when an electron jumps from the seventh excited state to the first excited state in He+ io...Assume that the uncertainty in the position of a particle is equal to its de Broglie wavelength. The minimum uncertainly...In Bohr series of lines of hydrogen spectrum, the third line from the red end corresponds to which one of the following ...No. of visible lines when an electron returns from 5th orbit to ground state in H spectrum -...