Fill in the following table. What are the frequency and energy of a photon with

Question

Fill in the following table.

What are the frequency and energy of a photon with a wavelength of 920 nm. Report your answers to three significant digits.

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Use the equation for the energy of the electron in the Bohr model of the atom and the fact that hxR = 2.180e-18 J to calculate the energy of an electron in the given level of each of the following ions. This is equation 2.5 in the paper textbook and can be found by browsing the e-book. Use 'e' notation with two decimal places. For example, 2.34e-22.

Hint: Each of the ions has a different number of protons, but all have one electron.

(nm) v (s-1) E/photon (J) E/mol photons
(kJ/mol) 701 9.00 1014 9.10 10-20 331

Explanation / Answer

ANSWER

Dear candidate you have asked many questions. As per guidelines one question one time. Here we answer first question . All othe questions can be solved by same precedure

For better understanding we have not answerd in tabular form.

(A) wavwlength = 701nm = 701 X 10-9m

frequency = velcity of light / wavelength = c/ = 3 X 108 / 701 X 10-9m = 4.28 X 1014s-1

E/photon (J) = planks constant X frequency = hv = 6.626 X 10-34 X 4.28 X 1014 = 28.36 X 10-20J

E/mol photons (kJ/mol) = Avagadroes No. X energy of one photon

E/mol photons (kJ/mol) = 6.022 X 1023 X 28.36 X 10-20 = 170.78 X 103 = 170.78KJ/mol

(B) frequency is given. v = 9.00 X 1014s-1

= 3 X 108 / 9.00 X 1014s-1 0.333 X 10-6m = 333.33 X 10-9m = 333.33nm

E/photon (J) = 6.626 X 10-34 X 9.00 X 1014 = 59.63 X 10-20J

E/mol photons (kJ/mol) = 6.022 X 1023 X 59.63 X 10-20 = 359.09KJ/mol

(C) E/photon (J) = hv = 9.10 10-20J

v =   9.10 10-20 / h= 9.10 10-20 / 6.626 X 10-34 = 1.3733 X 1014 s-1

wavelength = 3 X 108 / 1.3733 X 1014 = 2.184 X 10-6m

E/mol photons (kJ/mol) = 6.022 X 1023 X 9.10 10-20J = 54.80KJ/mol

(D) E/mol photons (kJ/mol) = 331KJ/mol

E/photon (J) = 331 / 6.022 X 1023 = 54.97 X 10-23KJ/mol = 54.97 X 10-20J/mol

frequency = 54.97 X 10-20J / 6.626 X 10-34 = 8.296 X 1014S-1

wavelength = 3 X 108 / 8.296 X 1014 = 0.3628 X 10-6 = 362.8nm

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