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  • If the velocity of the electron in Bohr’s first orbit is 2.19 x 10 ^6 ms -1, calculate the de Broglie wavelength associated with it.

2.59    If the velocity of the electron in Bohr’s first orbit is 2.19\times 10^6 \ \textup{ms}^{-1}, calculate the de Broglie wavelength associated with it.

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Given the velocity of the electron in Bohr's first orbit is 2.19\times 10^6 \ \textup{ms}^{-1}.

And we know the mass of electron which is 9.11\times10^{-31}kg

Hence the de-Broglie's wavelength associated with the electron will be:

\lambda = \frac{h}{mv} = \frac{6.626\times10^{-34}Js}{(9.11\times10^{-31}kg)\times(2.19\times10^6m/s)}

= 3.32\times10^{-10}m = 332\ pm

Posted by

Divya Prakash Singh

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