if uncertainty in momentum is twice the uncertainty in position of an electron, then uncertainty in velocity of electron is `[ħ=l/(2pi)]`

A german physicist gae a principle about the uncertainties in simultaneous measurement of position and momentum of small particles. According to that physicist. It is impossible to measure simultaneously the position and momentum of small particle with absolute accuracy or certainty. if an attempt is made to measure any one of these two quantities with higher accuracy, the other becomes less accurate. The produce of the uncertainty in position (Deltax) and uncertainty momentum (Delta p) is always constant and is equal to or greater than h//4pi , where h is Planck's constant i.e. (Deltax ) (Deltap) ge (h)/(4pi) If uncertainty in momentum is twice the uncertainty in position of an electron then uncertainty in velocity is: [bar(h)=(h)/(2pi)]

If the uncertainty in the position of an electron is zero the uncertainty in its momentum be

If the uncertainty in the position of an electron is zero the uncertainty in its momentum be

When uncertainty in position and momentum are equal, then uncertainty in velocity is

Why uncertainty in position is more when uncertainty in velocity is less for an electron ?