Consider the second spectral emission line in the ultraviolet series of the hydr

Question

Consider the second spectral emission line in the ultraviolet series of the hydrogen atom. What is the frequency in hertz and wavelength in nanometers of this emission line? What is the total energy in kilojoules of 1 mol. of photons radiated at this frequency? Consider the second spectral emission line in the ultraviolet series of the hydrogen atom. What is the frequency in hertz and wavelength in nanometers of this emission line? What is the total energy in kilojoules of 1 mol. of photons radiated at this frequency?

Explanation / Answer

wavelength calculated by rydberg formula , since its 2nd line , n1 =3 , n2 =infinity ,

1/wavelength = 1.097*107 ( (1/n1^2) - (1/n2^2) )

wavelenght = 9 / 1.097*107  = 820.4nm

frequency = 3*108  / 820.4nm = 3.66*1014 Hz

energy of 1mole of particles = planck's constant * frequency * avagadro's number

energy = (6.626 *10-34   ) * (3.66*1014 ) * (6*1023)

energy = 145.5 * 103 J

energy = 145.5 KJ

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