What is the energy of a photon with a wavelength of 8.45 102 nm? (The speed of light in a vacuum is 2.998 108 m/s. Planck's constant is 6.626 10-34 J · s.)
See above.
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)
To find the energy of a photon, you can use the equation:
E = (h * c) / λ
Where:
E is the energy of the photon
h is Planck's constant (6.626 x 10^-34 J · s)
c is the speed of light in a vacuum (2.998 x 10^8 m/s)
λ is the wavelength of the photon
First, let's convert the given wavelength from nanometers (nm) to meters (m):
8.45 x 10^2 nm = 8.45 x 10^(-7) m (since 1 nm = 10^(-9) m)
Now, we can substitute the values into the equation:
E = (6.626 x 10^-34 J · s * 2.998 x 10^8 m/s) / (8.45 x 10^(-7) m)
Calculating this expression will give you the energy of the photon in joules (J).