In problem 7, chapter 7, how do you find the energy used in 1 mol of atoms (the 2nd part of the problem)? I used the formula E = (n)(h)(wavelength)

But the answer I come up with (4.94e-20) is wrong. How do you do this part?

-- Anonymous, April 12, 2000

Answers

All you have to do is take the energy (the energy required to excite the hydrogen electron from one state to the other) you used to calculate the wavelength in part 1 and multiply it by avagadro's # (6.022 x 10^23) and you should get the energy used in 1 mol of atoms.

-- Anonymous, April 12, 2000