Question

In an experiment, an electron is determined to be within 0.1mm of a particular point. If we try to measure the electron's velocity, what will be the minimum uncertainty?​

Answer 1

Answer:

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Answer 2

Given: In an experiment, an electron is determined to be within 0.01 mm of a point.

To find: Minimum uncertainty in measuring electron's velocity

Explanation: Heisenberg’s uncertainty principle states that it is impossible to measure or calculate exactly, both the position and the momentum of an object.

Formula used is:

x.p= h/4π where x is uncertainty in distance and p is uncertainty in measuring the momentum.

=> x.m.v= h/4π where m is the mass of electron and v is uncertainty in measuring velocity

Mass of electron= 1.6* 10^-19

x= 0.01 mm= 10^-5 m

Putting value,

v = h/4πmx

$v = \frac{6.6 \times {10}^{ - 34} }{4 \times 3.14 \times 1.6 \times {10}^{ - 19} \times {10}^{ - 5} }$

v= 0.33 * 10^-10 m/s

Therefore, the uncertainty in measuring electron's velocity is 0.33* 10^-10 m/s.