Post Module #18


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Ashley Chipoletti 1I
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Joined: Fri Sep 29, 2017 7:04 am

Post Module #18

Postby Ashley Chipoletti 1I » Wed Nov 08, 2017 11:31 pm

Can someone help me solve this?

The hydrogen atom has a radius of approximately 0.05 nm. Assume that we know the position of an electron to an accuracy of 1% of the hydrogen radius, calculate the uncertainty in the speed of the electron using the Heisenberg uncertain principle.

Sean Monji 2B
Posts: 66
Joined: Fri Sep 29, 2017 7:06 am

Re: Post Module #18

Postby Sean Monji 2B » Wed Nov 08, 2017 11:47 pm

So we know the equation for uncertainty: ΔpΔx >= h/4π
Given a distance (Δx) and Δp = m * Δv (since velocity is the only thing that is uncertain about a momentum, mass is known) we can derive
1. Δv >= h/( 4π * Δx * m)
2. The Δx of an electron is said to be within 1% of .05 nm, thus .01 * .05 * 10^-9 m is Δx.
3. Plug in variables and solve: 6.626 * 10^-34 / (4π * 5.0 * 10^-13 * 9.109×10^-31)
4. Should give answer in Δv or uncertainty in velocity (m/s)
Last edited by Sean Monji 2B on Wed Nov 08, 2017 11:57 pm, edited 2 times in total.

Ammar Amjad 1L
Posts: 54
Joined: Thu Jul 27, 2017 3:00 am
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Re: Post Module #18

Postby Ammar Amjad 1L » Wed Nov 08, 2017 11:48 pm

This question was previously asked, here's the link for it

viewtopic.php?f=19&t=22876&p=67070&hilit=position+of+an+electron&sid=3d4f4a6923bcfac7b7adf733140188cf#p67070

hope it helps


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