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).

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.  

Calculate ionization energy of the hydrogen atom.

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

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?

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)

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

Calculate the mass of a photon with wavelength 3.6 Å.

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?  

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) 

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.