Use the Rydberg equation to calculate the wavelength of the photon emitted when

Question

Use the Rydberg equation to calculate the wavelength of the photon emitted when a hydrogen atom undergoes a transition from n = 5 to n = 1. Be careful when working with the reciprocal term in the Rydberg equation, and watch your unit. Submit Answer Answer Submitted: Your final submission will be graded when the time limit is reached. Tries 1/3 Previous Tries Now calculate the energy difference (delta E) for the transition in the previous problem for 1 mol H atoms. (Enter your answer in J/mol.) (in)/mol)

Explanation / Answer

Apply Rydberg Formula

E = R*(1/nf^2 – 1/ni ^2)

R = -2.178*10^-18 J

Nf = final stage/level

Ni = initial stage/level

E = Energy per unit (i.e. J/photon)

E = (2.178*10^-18)*(1/5^2 – 1/1 ^2)

E = -2.09088 *10^-18

For the wavelength:

WL = h c / E

h = Planck Constant = 6.626*10^-34 J s

c = speed of particle (i.e. light) = 3*10^8 m/s

E = energy per particle J/photon

WL = (6.626*10^-34)(3*10^8)/( -2.09088 *10^-18)

WL = 9.50 *10^-8 m

to nanometers:

WL = (9.50*10^-8)(10^9) = 95 nm

Q2

energy difference between 1 mol of H atoms...

E n5 = 2.09088 *10^-18 J/particle

E n1 = 2.178*10^-18 J/particle

dE =  2.178*10^-19-2.09088 *10^-18 = 1.87308*10^-18 J/particle

1 mol = 6.022*10^3 particles

1.87308*10^-18)(6.022*10^23) = 1127968.776 --> 1.12*10^6

nearest answer is A

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