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The position and the momentum of a particle
It revivals interesting truths for the nature of the particle/wave duality It also affects nuclear decay to a certain extent I belive it is also significant in the mathematical Models
Heisenberg uncertainty principle states that , the momentum and the position of a particle cannot be measured accurately and simultaneously. If you get the position absolutely correct then the momentum can not be exact and vice versa.
They both describe the nature of the wave/particle duality They also both point to the uncertainty of quantum mechanics
The heisenberg uncertainty principle is what you are thinking of. However, the relation you asked about does not exist. Most formalisms claim it as (uncertainty of position)(uncertainty of momentum) >= hbar/2. There is a somewhat more obscure and less useful relation (uncertainty of time)(uncertainty of energy) >= hbar/2. But in this relation the term of uncertainty of time is not so straightforward (but it does have an interesting meaning).
The position and the momentum of a particle
According to uncertainity principle we cannot measure the position of a particle as well as its speed simultaneously at a given time.
It revivals interesting truths for the nature of the particle/wave duality It also affects nuclear decay to a certain extent I belive it is also significant in the mathematical Models
According to the Heisenberg uncertainty principle if the position of a moving particle is known velocity is the other quantity that cannot be known. Heisenberg uncertainty principle states that the impossibility of knowing both velocity and position of a moving particle at the same time.
According to the Heisenberg uncertainty principle if the position of a moving particle is known velocity is the other quantity that cannot be known. Heisenberg uncertainty principle states that the impossibility of knowing both velocity and position of a moving particle at the same time.
Heisenberg uncertainty principle states that , the momentum and the position of a particle cannot be measured accurately and simultaneously. If you get the position absolutely correct then the momentum can not be exact and vice versa.
Werner Karl Heisenberg was a renowned German physicist and philosopher. In 1925 he discovered a way to formulate quantum mechanics with matrices. As a result of his discovery, Heisenberg was awarded the Nobel Prize for Physics in 1932.
They both describe the nature of the wave/particle duality They also both point to the uncertainty of quantum mechanics
Heisenberg's Uncertainty Principle applies only to particles at an atomic scale, and states that we cannot know both the precise location of an electron AND the precise velocity of the electron. To measure one of these, we would change the other in an unknowable way. But this only applies to very tiny particles on the scale of protons or electrons. Once you get up to even a molecular size, the particle is massive enough that the uncertainty effects are less significant than the size of the particle itself.
The heisenberg uncertainty principle is what you are thinking of. However, the relation you asked about does not exist. Most formalisms claim it as (uncertainty of position)(uncertainty of momentum) >= hbar/2. There is a somewhat more obscure and less useful relation (uncertainty of time)(uncertainty of energy) >= hbar/2. But in this relation the term of uncertainty of time is not so straightforward (but it does have an interesting meaning).
Heisenberg's uncertainty principle relates the fundamental uncertainty in the values of certain pairs of properties of a particle (e.g. momentum and position, energy and time) to a fundamental constant of nature known as Planck's Constant. Since Planck's constant is extremely small (~6.62
Heisenberg's Uncertainty Principle is a property of very small (sub-atomic) objects, and states (in effect) that one cannot know both the velocity of a particle and its exact location. This is true of larger objects as well, but at such an infinitely small scale that it is as close to 0 as you can get.