According to Heisenberg's Uncertainty Principle, we cannot simultaneously determine the position and momentum of a particle precisely and that there is always some uncertainty in this. Mathematically, the principle is given as:
`deltaxdeltap>= h/(4pi)`
where, `deltax` is the uncertainty in the position and `deltap` is the uncertainty in momentum of the object, while h is the Planck's constant.
Here, the uncertainty in the position of electron is 0.3 x 10^-10 m. The mass of an electron is 9.12 x 10^-31 kg and the value of Planck's constant is 6.626 x 10^-34 Js.
Thus, the uncertainty in velocity of the electron is
`deltav >= (6.626 xx 10^-34)/(4pi xx 9.12 xx 10^(-31) xx 0.3 xx 10^(-10)) = 0.193 xx 10^7`
Thus, there is a minimum uncertainty of 1.93 x 10^6 m/s in the velocity of the electron.
Hope this helps.
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