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

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