A) \[1.69\times {{10}^{-20}}J\]
B) \[1.69\times {{10}^{-23}}J\]
C) \[1.69\times {{10}^{23}}J\]
D) \[1.69\times {{10}^{25}}J\]
Correct Answer: B
Solution :
\[E=\frac{-13.6}{{{n}^{2}}}=\frac{-13.6}{4}=-3.4\,eV\] We know that energy required for excitation \[\Delta E={{E}_{2}}-{{E}_{1}}\] \[=-3.4-(-13.6)=10.2\,eV\] Therefore energy required for excitation of electron per atom \[=\frac{10.2}{6.02\times {{10}^{23}}}=1.69\times {{10}^{-23}}J\]
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