In the course of developing his model, Bohr arrived at the following formula
for the radius of the electron's orbit: \(r_{n}=\) \(n^{2} h^{2} \varepsilon_{0}
/ \pi m_{0} e^{2},\) where \(m_{c}\) is the electron's mass, \(e\) is its charge,
and \(\varepsilon_{0}\) is a constant related to charge attraction in a vacuum.
Given that \(m_{\mathrm{z}}=9.109 \times 10^{-31} \mathrm{~kg}, e=1.602 \times
10^{-19} \mathrm{C},\) and \(\varepsilon_{0}=8.854 \times 10^{-12}
\mathrm{C}^{2} / \mathrm{J} \cdot \mathrm{m}\)
calculate the following:
(a) The radius of the first \((n=1)\) orbit in the \(\mathrm{H}\) atom
(b) The radius of the tenth \((n=10)\) orbit in the \(\mathrm{H}\) atom