Question

The wavelength of the violet light emitted from a hydrogen atom is 410.1 nm. This light is a result of electronic transitions between the n = 5 and n = 2 energy levels. How much higher in energy is the n = 5 energy level than the n = 2 energy level?

Select one:

a. 3.000 x 108 J

b. 1.114 x 10-14 J

c. 2.436 x 10-18 J

d. 1.616 x 10-36 J

e. 4.847 x 10-19 J

Answer 1

e. 4.847 x 10-19 J

Step-by-step explanation:

From the given information:

The equation connecting the photon energy and the wavelength is:

`E_(photon ) = \frac {hc}{\lambda}`

where;

`planck's \ constant \ (h)`= 6.626 * 10 ^{-34} J.s

`velocity \ of \ light \ (c)` = 3.00 * 10^8 m/s

wavelength
`\lambda = 410.1 \ nm * (10^(-9) \ m)/(1 \ nm)`

`\lambda = 4.101 * 10^(-7) \ m`

To determine the photon energy of violet light

`E_(photon ) = \frac {(6.626 * 10^(-34) J/s ) * (3.00 * 10^8 \ m/s) }{4.101 * 10^(-7) \ m}`

= 4.847 × 10⁻¹⁹ J