Heisenberg Problem


Moderators: Chem_Mod, Chem_Admin

Lauren Tindall
Posts: 15
Joined: Sat Aug 24, 2019 12:17 am

Heisenberg Problem

Postby Lauren Tindall » Tue Nov 05, 2019 9:53 pm

An e- moving near an atomic nucleus has speed 6x10^61% m/s.
How do you find the uncertainty of its position?

Justin Seok 2A
Posts: 104
Joined: Sat Aug 24, 2019 12:15 am

Re: Heisenberg Problem

Postby Justin Seok 2A » Tue Nov 05, 2019 10:19 pm

So Heisenberg's uncertainty equation is basically (uncertainty in position)*(uncertainty in momentum)=h/4pi. Since we have uncertainty in speed, +- 1 m/s, we can find uncertainty in momentum by multiplying it by the mass of an electron, 9.11*10^-31. Then we can divide that value from both sides to get uncertainty in position = h/(4pi*uncertainty in momentum). Solve for this and you should get the value for uncertainty in position.

Charlene Datu 2E
Posts: 62
Joined: Wed Sep 11, 2019 12:16 am

Re: Heisenberg Problem

Postby Charlene Datu 2E » Tue Nov 05, 2019 10:23 pm

To find the uncertainty of position, you would use the equation ΔpΔx is greater than or equal to h/4pi

1) Rearrange the equation to isolate Δx (uncertainty of position) to get Δx is greater than or equal to h/(4pi Δp)
2) Find Δp. We're given the the speed from which we can calculate Δv and subsequently Δp. Use the equation Δp=mΔv to solve for Δp.
2.5) Δv can be calculated by taking the value after +/- symbol and multiplying it by 2.
3) Plug in your calculated value for Δp to the equation and get Δx

If there's any mistakes, please correct me :)

Victor James 4I
Posts: 50
Joined: Wed Sep 18, 2019 12:20 am

Re: Heisenberg Problem

Postby Victor James 4I » Tue Nov 05, 2019 10:31 pm

the mass of the electron will be given on the midterm, fyi


Return to “Heisenberg Indeterminacy (Uncertainty) Equation”

Who is online

Users browsing this forum: No registered users and 1 guest