Given:
Wavelength, λ = 337.1 nm = 337.1 × 10−9 m
Number of photons emitted per second, n = 5.6 × 1024 s−1
Speed of light, c = 3 × 108 m s−1
Planck’s constant, h = 6.626 × 10−34 J s
Step 1: Calculate frequency of radiation
ν = c / λ
ν = (3 × 108) / (337.1 × 10−9)
ν = 8.90 × 1014 s−1
Step 2: Calculate energy of one photon
E = hν
E = (6.626 × 10−34) × (8.90 × 1014)
E = 5.90 × 10−19 J
Step 3: Calculate power of the laser
Power = Energy per second
Power = n × E
Power = (5.6 × 1024) × (5.90 × 10−19)
Power = 3.30 × 106 W
Final Answer:
Power of the nitrogen laser,
P = 3.3 × 106 W
Considering Bohr’s atomic model for hydrogen atom :
(A) the energy of H atom in ground state is same as energy of He+ ion in its first excited state.
(B) the energy of H atom in ground state is same as that for Li++ ion in its second excited state.
(C) the energy of H atom in its ground state is same as that of He+ ion for its ground state.
(D) the energy of He+ ion in its first excited state is same as that for Li++ ion in its ground state.