Question

Certain atoms emit photons of light with an energy of 4.893 x 10^-19 J. Calculate the frequency (in Hz) and wavelength (in nm) of one of these photons. frequency Hz wavelength nm What is the total energy (in kJ) in 1 mole of these photons? kJ What is the color of the emitted light? violet blue green yellow orange red

          Certain atoms emit photons of light with an energy of 4.893 x 10^-19 J. Calculate the frequency (in Hz) and wavelength (in nm) of one of these photons.
frequency Hz
wavelength nm
What is the total energy (in kJ) in 1 mole of these photons?
kJ
What is the color of the emitted light?
violet
blue
green
yellow
orange
red

Certain atoms emit photons of light with an energy of 4.893 x 10^-19 J. Calculate the frequency (in Hz) and wavelength (in nm) of one of these photons.
frequency Hz
wavelength nm
What is the total energy (in kJ) in 1 mole of these photons?
kJ
What is the color of the emitted light?
violet
blue
green
yellow
orange
red

Added by John P.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Certain atoms emit photons of light with an energy of 4.893 x 10^-19 J. Calculate the frequency (in Hz) and wavelength (in nm) of one of these photons: frequency Hz wavelength nm What is the total energy (in kJ) in 1 mole of these photons? kJ What is the color of the emitted light? violet blue green yellow orange red