Why Heisenberg uncertainty principle is not applicable for a bigger molecule?
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Solution
Heisenberg's Uncertainty Principle:
By Heisenberg's principle, we know where (for slow-moving particles with respect to the speed of light). is the position, is the momentum, and is Planck's constant.
is the uncertainty in the measurement of the velocity and mass() is assumed to be constant, so the equation is
If is the error in position measurement and is the error in the measurement of momentum, then
Since momentum, , Heisenberg’s uncertainty principle formula can be alternatively written as-
Where, is the error in the measurement of velocity and assuming mass remaining constant during the experiment,
Accurate measurement of position or momentum automatically indicates larger uncertainty (error) in the measurement of the other quantity.
According to his theory, we can't measure the position and the velocity of the object accurately at the same time
From the formula, as the momentum is not low, the uncertainty in the momentum is low.
As Planck's constant is very small, it is very difficult to determine experimentally the uncertainties in the position and momentum of large objects.
A phenomenon like the atomic process and displacement are critically applicable.
Therefore the Heisenberg uncertainty principle is significant only for the smaller particles.
By using the uncertainty principle both the position and momentum of the particle cannot be measured simultaneously.
So Heisenberg's uncertainty principle is not applicable for a bigger molecule.