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In a hypothetical Bohr hydrogen atom, if the mass of the electron is doubled then the energy of the electron in the first orbit is
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$-27.2 \mathrm{eV}$
Mass of the electron, $\mathrm{m}=2 \mathrm{~m}$
Energy of electron, $E \propto \frac{\mathrm{m}}{\mathrm{n}^2}$ For first orbit, $\mathrm{n}=1$
$\begin{aligned}
& E=\frac{2 \times(-13.6)}{1} \\
& =-27.2 \mathrm{ev}
\end{aligned}$
Energy of electron, $E \propto \frac{\mathrm{m}}{\mathrm{n}^2}$ For first orbit, $\mathrm{n}=1$
$\begin{aligned}
& E=\frac{2 \times(-13.6)}{1} \\
& =-27.2 \mathrm{ev}
\end{aligned}$
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