Question

If the velocity of the electron in Bohrs first orbit is 2.19 × 10 6 m/s, Calculate de Broglie wavelength associated with it .

Answer 1

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Answer 2

$\huge\rm\underline\pink{Solution:-}$

$\large\rm\bold{\boxed{\lambda\:=\:\frac{h}{mv}}}$

$\large\rm{h\rightarrow{\:planck's\:constant}}$

$\large\rm{m\rightarrow{\:mass\:of\:particle}}$

$\large\rm{v\rightarrow{velocity\:of\:particle}}$

Given Velocity (v) = 2.19 × 10⁶m/s

Mass of electron = 9.1 × 10⁻³¹ kg

h = 6.625 × 10⁻³⁴ J.sec

$\large\rm{\implies{\lambda\:=\:\frac{6.625\times\:10^-34}{9.1\times\:10^-31\times\:2.19\times\:10^6}}}$

$\large\rm{\implies{\lambda\:=\:0.332\times\:10^-9}}$

∴ Debriglie wavelength associated with it is 0.332 × 10⁻⁹m = 0.33 nm = 3.3 A⁰