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According to heisenberg's uncertainty principle, the postion and momentum of an electron cannot be determined together. How can we determine the position or velocity of an electron (experimental) and why cannot find it together.

Asked by sureshkalanjoor 30th July 2016, 7:15 PM
Answered by Expert
It is impossible to measure simultaneously the position and momentum of a 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 product of the uncertainty in the position (Δx) and the uncertainty in the momentum (Δp = m.Δv where m is the mass of the particle and Δv is the uncertainty in veloity) is alwyas constant and is equal to or greater than h/4π, where h is Plank's constant, that is
 Δx.Δp ≥ h/4π  .....  (i)
The mathematical expression, 
increment x. increment p space almost equal to space fraction numerator h over denominator 4 straight pi end fraction space space space space.... space left parenthesis i i right parenthesis   
From (i) and (ii), the value of Δp calculated for a given value of Δx is the minimum value for Δp. 
Similarly the value of Δp will be the minimum value for Δx.
Putting Δp = m x Δv , eqn. (i) becomes Δx . (mΔv) ≥ h/4π  or Δ x . Δv ≥ h / 4πm.
This implies that the position and velocity of a particle cannot be measured simultaneously with certainty.
It is important to understand that uncertainty principle applies to position and momentum along the same axis. Thus if Δx is along X-axis, then Δp should also be along X-axis. It is further important to remember that the uncertainty principle is not on accunt of any limitation of the measuring instrument.
Answered by Expert 1st August 2016, 6:15 PM
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