### Post Module Question #8/9

Posted:

**Wed Oct 05, 2016 4:42 pm**Question 8 states If one incorrectly assumed that an electron is located inside the nucleus of an atom, then for a hydrogen atom the electron is confined to its nuclear diameter of 1.7 x 10-15 m which would be the electron's uncertainty in position. Use the Heisenberg uncertainty equation to calculate the electron's uncertainty in momentum. Then use the mass of electron (9.1 x 10-31 kg) to calculate its uncertainty in velocity.

Comment on your value.

I got that Delta p <= 3.1 x 10-20kg.m.s-1, Delta v = 3.4 x 1010m.s-1

For question 9, it says use the above uncertainty in velocity to calculate the electron's uncertainty in kinetic energy. Then calculate the uncertainty in kinetic energy per mole of electrons (that is, per mole of hydrogen atoms). Comment on your value.

I used the velocity I got to determine the wavelength then used the wavelength to determine the energy; but, my answer didn't match any of the options. What am I doing wrong?

Comment on your value.

I got that Delta p <= 3.1 x 10-20kg.m.s-1, Delta v = 3.4 x 1010m.s-1

For question 9, it says use the above uncertainty in velocity to calculate the electron's uncertainty in kinetic energy. Then calculate the uncertainty in kinetic energy per mole of electrons (that is, per mole of hydrogen atoms). Comment on your value.

I used the velocity I got to determine the wavelength then used the wavelength to determine the energy; but, my answer didn't match any of the options. What am I doing wrong?