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The wavelength of the bright red line in the spectrum of atomic

hydrogen is 652 nm. What is the energy of the photon generated in
the transition?

User Shawn Chen
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1 Answer

6 votes

Answer:

The energy of the photon generated in the transition is 3.14*10⁻¹⁹ J

Step-by-step explanation:

There are two equation that we need to use in order to solve this problem:

The first one is Planck's equation, which describes the relationship between energy and frequency:

E = h*v eq. 1)

Where E is energy, h is Planck's constant (6.626 * 10⁻³⁴ J*s) and v is the radiation frequency.

In order to know the frequency, we use the second equation, which is the wave equation:

c = λ*v eq. 2)

Where c is the speed of light in vacuum (aprx 3 * 10⁸ m/s), and λ is the wavelength. If we solve that equation for v we're left with

v=c/λ eq. 3)

We replace v in eq. 1):

E= c*h/λ

Lastly we put the data we know and solve the equation, keeping in mind the correct use of units (converting 652 nm into m):


E=(3*10^(8)ms^(-1) *6.626*10^(-34)Js)/(633*10^(-9)m )=3.14*10^(-19)J

User JonMinton
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