Post-Module Q.18 [ENDORSED]

[Shannee Mak 3F]

I'm having a little trouble mapping out the steps for how to correctly solve this problem. Could someone help me with the steps? Thanks!

The question: 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.

I've converted the radius to diameter and nm to m, which would give the values needed for the position. What should I do after?

[Tanaisha Italia 1B]

You could use the uncertainty equation (delta p * delta x is greater than or equal to h/4pi) to find delta p by plugging in the error in the diameter for delta x. Using the result for delta p, divide that by the mass of the electron to find the uncertainty in the speed.

[Shannee Mak 3F]

I've been calculating again and again, but I keep getting an extremely small number (like x10^-22) ... am I supposed to be using the diameter or the radius in the calculations?

[Shannee Mak 3F]

Nevermind, I solved it!