An electron microscope uses electrons accelerated by a voltage of 50 kV. Determine the de Broglie wavelength associated with the electrons. If other factors (such as numerical aperture, etc.) are taken to be roughly the same, how does the resolving power of an electron microscope compare with that of an optical microscope which uses yellow light?

The mass of an electron is 1/1840 part of mass of a proton. When they are subjected to a uniform electric field, they start accelerating. If they start from rest and have the same De Broglie wavelength of 1 angstrom unit, then determine the ratio of their kinetic energies

Dual behaviour of matter proposed by de Broglie led to the discovery of electron microscope oftenused for the highly magnified images of biological molecules and othér type of material. If the velocity of the electron in this microscope is '1.6 xx 10^6 ms^(-1)', calculate de Broglie wavelength associated with this electron.

Werner Heisenberg considered the limits of how precisely we can measure the properties of an electron or other microscopic particle. He determined that there is a fundamental limit to how closely we can measure both position and momentum. The more accurately we measure the momentum of a particle, the less accurately we can determine its position. The converse is also true. This is summed up in what we now call the Heisenberg uncertainty principle. The equation is Delta x Delta (mv) ge (h)/(4 pi) The uncertainty in the position or in the momentum of a macroscopic object like a baseball is too small to observe. However, the mass of microscopic object such as an electron is small enough for the uncertainty to be relatively large and significant. If the uncertainty in velocity and position is same, then the uncertainty in momentum will be:

Werner Heisenberg considered the limits of how precisely we can measure the properties of an electron or other microscopic particle. He determined that there is a fundamental limit to how closely we can measure both position and momentum. The more accurately we measure the momentum of a particle, the less accurately we can determine its position. The converse is also true. This is summed up in what we now call the Heisenberg uncertainty principle. The equation is Delta x Delta (mv) ge (h)/(4 pi) The uncertainty in the position or in the momentum of a macroscopic object like a baseball is too small to observe. However, the mass of microscopic object such as an electron is small enough for the uncertainty to be relatively large and significant. If the uncertainties in position and momentum are equal, the uncertainty in the velocity is: