delta E = 2.180E-18 J(1/a^2 - 1/b^2) where a = 2 and b= 4) so
dE = 2.180E-18 J (1/2^2 - 1/4^2)
Solve for dE. Then dE = hc/wavelength. h is Planck's constant, c is speed of light. Solve for wavelength (in meters) and convert to nanometers. Post your work if you get stuck.
The lines in the visible portion of the hydrogen spectrum are called the Balmer series, for which m=2 in the Rydberg equation. Calculate the wavelength in nanometers of the spectral line in this series for which n=4.
2 answers
So for dE I got 4.0875 × 10-19 joules
Over
(6.62607004 × 10-34 m2 kg / s)(299 792 458 m / s)
Do I have to then covert into nm?
Over
(6.62607004 × 10-34 m2 kg / s)(299 792 458 m / s)
Do I have to then covert into nm?