An atom radiates 1.5 × 10-19J when an electron jumps from one level to another. What is the wavelength of the emitted radiation? (Planck’s constant 6.6 × l0-34Js ; Speed of light in vacuum = 3.0 × 108ms-1)
a
1.32 × 10-6m
b
2.97 × 10-6m
c
3.30 × 10-6m
d
6.82 × 10-6m
e
8.01 × 10m-6
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daadudaniel
3 years ago
We can use the formula relating the energy of a photon to its wavelength:
E = hc/λ
where E is the energy of the photon, h is Planck's constant, c is the speed of light, and λ is the wavelength of the photon.
In this case, we are given the energy of the emitted radiation (1.5 × 10^-19 J), and we can use the values of h and c to solve for the wavelength:
E = hc/λ
λ = hc/E
λ = (6.6 × 10^-34 J s)(3.0 × 10^8 m/s)/(1.5 × 10^-19 J)
λ =1.32 × 10^
-6m
