### post Module Heisenberg

Posted:

**Sun May 06, 2018 11:33 pm**Hey, everyone! I'm not really sure how to do the following problem. I keep getting he wrong answer regardless of how many times I attempt to calculate it:

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.

Comment on your value obtained.

The answer is D. Delta v >= 108 m/s, Delta v is very high. In knowing with certainty the position of the electron to within 1 % of the hydrogen atom radius the resulting uncertainty in the electron's speed is so high that we essentially do not know its speed at the same time that we know its position.

Any help on this problem would be greatly appreciated. Thanks!

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.

Comment on your value obtained.

The answer is D. Delta v >= 108 m/s, Delta v is very high. In knowing with certainty the position of the electron to within 1 % of the hydrogen atom radius the resulting uncertainty in the electron's speed is so high that we essentially do not know its speed at the same time that we know its position.

Any help on this problem would be greatly appreciated. Thanks!