It is impossible to determine simaltanco...

It is impossible to determine simaltancously the position of velocity of small mictroscopic particle such as electron , proton or neutron with accoracy .This is called Heisenberg's uncertainty principal, Malthematically, it is represenites as `Delta x. Delta p ge (h)/(4pi) Delta x` is uncertainty in position `Delta p ` is uncertainty in momentum

`8 xx 10^(12) m s^(-1)`

`6 xx 10^(12) m s^(-1)`

`84xx 10^(12) m s^(-1)`

`2 xx 10^(12) m s^(-1)`

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The correct Answer is:

`Delta x Delta p ge (h)/(4pi) rArr Delta p ge sqrt((h)/(4pi)){:' Delta x = Delta p (given)]`
`rArr Delta x ge (1)/(m) sqrt((h)/(4pi)) = 8 xx 10^(12) ms^(-1)[:' Delta p = m Delta v]`

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It is not possible to determine preciselt both the position and momentum (or velocity) of a small moving particle such as electron, proton etc. This is known as Heisenber uncertainty principle. The mathemactical form of this principle is : Delta x.Delta p ge (h)/(4pi) (constant) However this principle is irrevalent in case of bigger particles such as a cup, ball, car etc., that we come across in our daily life. In case of small microscopic particles, Heisenberg's uncertainty principle rules out simultaneous exact determination of their

It is not possible to determine preciselt both the position and momentum (or velocity) of a small moving particle such as electron, proton etc. This is known as Heisenber uncertainty principle. The mathemactical form of this principle is : Delta x.Delta p ge (h)/(4pi) (constant) However this principle is irrevalent in case of bigger particles such as a cup, ball, car etc., that we come across in our daily life. If the uncertainty in position of the electron is zero, the uncertainty in its momentum would be

It is not possible to determine preciselt both the position and momentum (or velocity) of a small moving particle such as electron, proton etc. This is known as Heisenber uncertainty principle. The mathemactical form of this principle is : Delta x.Delta p ge (h)/(4pi) (constant) However this principle is irrevalent in case of bigger particles such as a cup, ball, car etc., that we come across in our daily life. If uncertainty in position and momentum are equal, the v uncertainty in velocity would be

It is not possible to determine preciselt both the position and momentum (or velocity) of a small moving particle such as electron, proton etc. This is known as Heisenber uncertainty principle. The mathemactical form of this principle is : Delta x.Delta p ge (h)/(4pi) (constant) However this principle is irrevalent in case of bigger particles such as a cup, ball, car etc., that we come across in our daily life. Given that the mass of electron is 9.1 xx 10^(-31) kg and velocity of electron is 2.2 xx 10^(6) ms^(-1) , if uncertainty in its velocity is 0.1% , the uncertainty in position would be

The equation. Delta x. Deltap ge h//4 pi shows

We can pin point an aeroplane moving in the sky, whatever may be its speed i.e., we can locate both its exact position as wellas direction . However, it is not possible to doso in case of a moving microscopic particle such as electron. In fact, we cannot see any such particle without disturbing it. This has been stated by Heisenberg in the form of uncertainty principle. The mathematical form of this principle is : Deltax.DeltaP ge (h)/(4pi) (constant). Since the product of Deltax and Deltap(m Delta upsilon) is constant , if one is very small, the other is bound to be large. The principle as such has no significance in daily life since it applies to those particles which we can not see. If uncertainty in position and momentum are equal , then the uncertainty in velocity is :

We can pin point an aeroplane moving in the sky, whatever may be its speed i.e., we can locate both its exact position as wellas direction . However, it is not possible to doso in case of a moving microscopic particle such as electron. In fact, we cannot see any such particle without disturbing it. This has been stated by Heisenberg in the form of uncertainty principle. The mathematical form of this principle is : Deltax.DeltaP ge (h)/(4pi) (constant). Since the product of Deltax and Deltap(m Delta upsilon) is constant , if one is very small, the other is bound to be large. The principle as such has no significance in daily life since it applies to those particles which we can not see. If the uncertainty in the position of electron is zero , the uncertainty in its momentum would be

We can pin point an aeroplane moving in the sky, whatever may be its speed i.e., we can locate both its exact position as wellas direction . However, it is not possible to doso in case of a moving microscopic particle such as electron. In fact, we cannot see any such particle without disturbing it. This has been stated by Heisenberg in the form of uncertainty principle. The mathematical form of this principle is : Deltax.DeltaP ge (h)/(4pi) (constant). Since the product of Deltax and Deltap(m Delta upsilon) is constant , if one is very small, the other is bound to be large. The principle as such has no significance in daily life since it applies to those particles which we can not see. Heisenberg's uncertainty principle rules out the exact simultaneous measurement of

The French physicist Louis de Broglie in 1924 postulated that matter like radiation , should exhibit a dual behaviour. He proposed the following relationship between the wavelength .lambda of a material particle,its linear momentum P and Planck constant h. lambda=(h)/(p)=(h)/(mv) The de Broglie relaion that the wavelength of a particle should decrease as its velocity increases. It also implies that for a given velocity heavier particles should have shorter wavelength than lighter particles.The waves or de Broglie waves. These waves differ from the electromagnetic waves as they: (i) have lower velocities (ii) have no electrical and magnetic fields and (iii) are not emitted by the particle under consideration. The expermental confirmation of the de Broglie relation was obtained when Davission and Germer in 1927, observed. As diffraction is a characteristic property of waves, hence the beam of electrons behave as a wave as proposed by de Broglie. Werner Heisenberg considered the limits of how precisely we can measure properties of an electron or other microscopic particle like electron . He determined that there is a fundamental limit of how closely we can measure both position and momentum. The more accurately we can determine its position. The converse is also true. This is summed up in what we now call the ''Heisenberg uncertainty principle'' : It is impossible to determine simultaneously and precisely both the momentum and position of a particle. The product of uncertainty in the position, Deltax and the uncertainty in the momentum Delta(mv) must be greater than or equal to (h)/(4pi), i.e., Deltax Delta(mv)ge(h)/(4pi) If the uncertainty in velocity and posititon is same then the uncertainty in momentum will be :

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)]

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