Ncert Exercises & Solutions

2.59 If the velocity of the electron in Bohr’s first orbit is 2.19 × 106 ms–1, calculate the
de Broglie wavelength associated with it.

According to de Broglie’s equation, λ = h/mv
Where, λ = wavelength associated with the
electron h = Planck’s constant
m = mass of electron
v = velocity of electron
Substituting the values in the expression of λ:

λ = \frac{6.626 x 10^{- 34} Js}{(9.10939 x 10^{31} kg) (2.19 x 10^{6} m / s)}

= 3.32 x 10^{- 10} m = 3.32 x 10^{- 10} m x \frac{100}{100}

= 332 x 10^{- 12} m

λ = 332 pm

∴

Wavelength associated with the electron = 332 pm

NEET Information

courses

Company

Botany Questions

Chemistry Questions

Physics Questions

Zoology Questions