In: Chemistry
An electron was accelerated through a potential difference of 1.00 ± 0.01 kV. What is the uncertainty of the position of the electron along its line of flight?
If the momentum of a particle is precisely specified, the position is
totally uncertain. This remarkable destruction of one of the fundamentals
of classical mechanics is a special case of the Heisenberg Uncertainty
Principle, It states that if the momentum is known to lie within a range
δp, then the position must be uncertain to an extent δz,
where
δpδz ≥ (ћ/2) (1)
Hece ћ = (ћ / 2π) and h = Planck's constant. Note that z is the line of flight.
The uncertainty of momentum can be calculated from
δp = meδv (2)
where δv = the uncertainty in velocity. This δv can be calculated from
(1/2)mev2 = eV.
For a potential difference of 0.99 kV,
v = √(2eV / me)
= √[{2(1.602 × 10–19 C) (990V)} / {9.110 × 10–31 kg}]
= √[{2(1.602 × 10–19) (990) CV } / {9.110 × 10–31 kg}]
= √[3.482 × 1014 (JV–1V / kg)]
= √[3.482 × 1014 {(kg m2 sec–2) / kg}]
= √[3.482 × 1014 m2 sec–2]
∴ v = 1.866 × 107 m s–1
Similarly, for a potential difference of 1.01 kV,
v = 1.885 × 107 m s–1
Hence δv = (1.885 – 1.866) × 107 m s–1
= 0.019 × 107 m s–1
= 1.9 × 105 m s–1
Solving for δp in equation (2) gives
δp = (9.110 × 10–31 kg) (1.9 × 105 m s–1)
= 17.309 × 10–26 kg m s–1
= 1.7 × 10–25 kg m s–1
Rearranging equation (1) to solve for δz gives
δz ≥ {(ћ/2) / δp} = [{1.054 × 10–34 Js} / {2(1.7 × 10–25 m s–1)}]
= 3.09 × 10–10 (Js/kg) m s–1
= 3.09 × 10–10 (kg m2/s2) (s/kg) m s–1
or δz = 3.09 × 10–10 m = 309 pm = 3.09 Å.
Hope this helps