In the lecture , you also learned about the Heisenberg Uncertainty Principle (AEA'H? ;-_=_). 411'\"! According to this principle , there is a limit on the product between the uncertainty in position (a particle -like quality of the object ) and the uncertainty in speed (a wave like quality of the object , since ,as de Broglie showed , speed and wavelength of the object are related ). Let's consider what we can learn from the Heisenberg Uncertainty Principle both qualitatively and quantitatively E. Suppose you did a version of the double -slit experiment in which the electrons are sent out towards the slits one by one . Furthermore ,suppose that you wanted to determine exactly which slit each electron went through .In order to do that one would need to determine the position of the electron to within the width of each slit. In other words , the uncertainty in the position of the electrons would be equal to the width of the slits . In your setup ,the width of each slit is ~60 rim, the same as what the researchers at University of Nebraska -Lincoln experiment used . (i) What would be the minimum uncertainty in the speed of the electrons , given this uncertainty in position ? (ii) Recall that in your double slit experiment the electrons are moving at a speed of l kml's. How does the uncertainty in speed you calculated in part E (i) above compare to the speed of electrons ? Report your answer as a percentage (uncertainty in speed as percentage of the speed )