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

Answer:

e. 4.847 x 10-19 J

Explanation:

From the given information:

The equation connecting the photon energy and the wavelength is:

$E_{photon } = \dfrac {hc}{\lambda}$

where;

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

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

wavelength $\lambda = 410.1 \ nm \times \dfrac{10^{-9} \ m}{1 \ nm}$

$\lambda = 4.101 \times 10^{-7} \ m$

To determine the photon energy of violet light

$E_{photon } = \dfrac {(6.626 \times 10^{-34} J/s ) \times (3.00 \times 10^8 \ m/s) }{4.101 \times 10^{-7} \ m}$

= 4.847 × 10⁻¹⁹ J