Module Question


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Jolie Sukonik 2B
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Joined: Wed Sep 30, 2020 9:44 pm

Module Question

Postby Jolie Sukonik 2B » Mon Oct 26, 2020 4:01 pm

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 uncertainty principle.

How do I find the uncertainty in the position first? I know once I find it I can just calculate the uncertainty in velocity, but I am struggling on how to find deltax.

Quentin Scarborough 1A
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Joined: Wed Sep 30, 2020 9:59 pm
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Re: Module Question

Postby Quentin Scarborough 1A » Mon Oct 26, 2020 4:31 pm

If you know the radius of a Hydrogen atom, you can just find 1% of that to find your uncertainty. In this case it would be .05nm * .01= 5*10^-13, which would be your uncertainty position.

Akshata Kapadne 1C
Posts: 49
Joined: Wed Sep 30, 2020 9:40 pm

Re: Module Question

Postby Akshata Kapadne 1C » Mon Oct 26, 2020 4:31 pm

Since it says that we know the position of an electron to an accuracy of 1 % of the hydrogen radius, and the radius is 0.05 nm, the uncertainty in position is
.01(.05 nm)= 5 x 10^-13 m. From there, you can find delta(v).


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