If an electron has a speed at 8.31 x 106 m/s with 11% uncertainty, calculate the minimum uncertainty of the position of this electron, Δx, in nm.

What are the possible values of ml if n = 5 and l = 3?

calculate the uncertainty in the position of a hydrogen atom when its velocity is known to be within 50.0 m/s. How does the uncertainty in position compare to the radius of the hydrogen atom at approximately 0.040 nm (1 amu = 1.66 * 10^-27 kg).    really struggling on the second part of the question. thank you.

German physicist Werner Heisenberg related the uncertainty of an object's position (Ax) to the uncertainty in its velocity (Av) h Ax 2 4xmAv where h is Planck's constant and m is the mass of the object. The mass of an electron is 9.11 x 10-31 kg. What is the uncertainty in the position of an electron moving at 5.00 x 10° m/s with an uncertainty of Av = 0.01 x 10ʻ m/s? Ax 2 m