An atom emits a photon of wavelength 1.08 meters. What is the energy change occurring in the atom due to this emission? (Planck's constant is
6.626 × 10-34 joule seconds, the speed of light is 2.998 × 108 m/s)

7.1560 × 10-34 joules

1.8393 × 10-25 joules

2.3869 × 10-42 joules

1.9864 × 10-25 joules

Question

An atom emits a photon of wavelength 1.08 meters. What is the energy change occurring in the atom due to this emission? (Planck's constant is
6.626 × 10-34 joule seconds, the speed of light is 2.998 × 108 m/s)

7.1560 × 10-34 joules

1.8393 × 10-25 joules

2.3869 × 10-42 joules

1.9864 × 10-25 joules

anonymous · Answer

you can get the energy multiplying the frequency of the emitted light by Planck's constant:
$E=h\nu$
since you are given the wavelength, $\lambda$,  you will have to calculate the frequency, $\nu$, first using:
$\lambda=c\nu$
where $c$ is the speed of light...

anonymous · Answer

give it a try and see if you can get the result!

anonymous · Answer

idk how to do it