Question

Calculate the uncertainty in the position of an electron if the uncertainty in its velocity is 5.7 × 105 m/sec (h = 6.6 × 10–34 kg m2 s–1, mass of the electron = 9.1×10–31 kg).

Solution

Correct option is

±10–10 m

 

Here, we are given  

         

         

         

Substituting these values in the equation for uncertainty principle, ,          

   

                        

                        

i.e., Uncertainty in position = ±10–10 m. 

SIMILAR QUESTIONS

Q1

 

 

Calculate the velocity of electron in the first Bohr orbit of hydrogen atom. Given that

       Bohr radius = 0.529 Å, 

       Planck’s constant, h = 6.626 × 10–34 Js,  

       mass of electron = 9.11 × 10–31 kg and

                        1 J = 1 kg m2s–2.  

Q2

Calculate ionization energy of the hydrogen atom.

Q3

The ionisation energy of He+ is . Calculate the energy of first stationary state of Li2+.

Q4

The ionization energy of hydrogen in excited state is +0.85 eV. What will be the energy of the photon emitted when it returns to the ground state?

Q5

 

Calculate the wavelength associated with an electron

(mass 9.1 × 10–31 kg) moving with a velocity of 103 m sec–1

(h = 6.6 × 10–34 kg m2 sec–1)

Q6

What will be the wavelength of a ball of mass 0.1 kg moving with a velocity of 10 ms–1?

Q7

Calculate the mass of a photon with wavelength 3.6 Å.

Q8

A microscope using suitable photons is employed to locate an electron in an atom within a distance of 0.1 Å. What is the uncertainty involved in the measurement of its velocity?  

Q9

 

Calculate the uncertainty in the velocity of a wagon of mass 3000 kg whose position is known to an accuracy of ±10 pm

(Planck’s constant = 6.63 × 10–34 Js) 

Q10

A golf ball has a mass of 40 g and a speed of 45 m/s. If the speed can be measured within accuracy of 2%, calculate the uncertainty in position.