Question

How much energy in kJ is needed to excite 1 mol of H atoms to the...

How much energy in kJ is needed to excite 1 mol of H atoms to the stationary state with quantum number n = 6 from their ground state? B) Calculate the frequency in Hz of emitted light when electrons fall back to their grounds state from their state in part A.

Homework Answers

Answer #1

(A)

Energy required for this transition

E = -13.6 [(1/n12)-(1/n22)] eV

= -13.6 [(1/12)-(1/62)] eV

= -13.6 [1-(1/36)] eV

= -13.6 [35/36)] eV

= -13.22 eV

So, 13.22 eV energy required for transition of electron from ground state to n=6 stationary state for one atom.

for one mole of H atom the energy required = 6.023 x 1023 x 13.22 eV

= 7.96 x 1024 eV

Now, we know that 1 eV = 1.6 x 10-19J

So, 7.96 x 1024 eV = 7.96 x 1024 x 1.6 x 10-19J

= 1.2736 x 106J

= 1273.6 kJ energy is required for the required transition.

(B)

Energy per transition, E = 13.22 x 1.6 x 10-19 J

h = 211.52 x 10-19 J, where h = Planck's constant = 6.63 x 10-34Js

= 211.52 x 10-19/ 6.63 x 10-34 Hz

= 3.19 x 1016 Hz is the frequency of light emitted when electron falls back to grond state.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The energy of a vibrating molecule is quantized much like the energy of an electron in...
The energy of a vibrating molecule is quantized much like the energy of an electron in the hydrogen atom. The energy levels of a vibrating molecule are given by the equation En=(n+12)hν where n is a quantum number with possible values of 1,2,…, and ν is the frequency of vibration. The vibration frequency of HCl is approximately 8.85×1013s−1 Part A: starting with a "stationary" molecule, what minimum energy is required to excite a vibration in HCl? Part B: What wavelength...
The H–Br bond energy is 142 kJ/mol. Therefore the formation of a single bond between atoms...
The H–Br bond energy is 142 kJ/mol. Therefore the formation of a single bond between atoms The H–Br bond energy is 142 kJ/mol. Therefore the formation of a single bond between atoms should require the absorption of 284 kJ per mole of H–Br formed. should result in the release of 142 kJ per mole of H–Br formed. should require the absorption of 142 kJ per mole of H–Br formed. should result in the release of 284 kJ per mole of...
1. Calculate the energy (in kJ/mol) of the Lyman series line for hydrogen that is, the...
1. Calculate the energy (in kJ/mol) of the Lyman series line for hydrogen that is, the transition from n=2 to n=1 (1 kJ/mol= 8.6 cm^-1) 2. Would you expect the energy of the same transition as in the first problem to be greater or less for the helium ion, He^+? Why? Make a sketch to relative scale the energy levels that give rise to the Lyman bands in H-atoms and He^+.
In addition to thermal energy, one can also use photons to impart energy to Si so...
In addition to thermal energy, one can also use photons to impart energy to Si so that some electrons from the valence band can jump over to the conduction band. What is the maximum wavelength of the light that can be used to excite an electron from the valence band to the conduction band of Si at 300K? The same electrons can fall back to the valence band giving out the energy as radiation. Calculate the wavelength of the light...
The ionization energy of gold is 8.90x10^2 kJ/mol. How much energy, in kilojoules, is required to...
The ionization energy of gold is 8.90x10^2 kJ/mol. How much energy, in kilojoules, is required to ionize 79 atoms of gold?
how to calculate ground state for N and N+1 electrons quantum dot and plot grap between...
how to calculate ground state for N and N+1 electrons quantum dot and plot grap between number of electrons vs energy. if you can comsider electrons are parabolic simple harmonic oscillator quantum confirment.
1. We can observe the wavelengths emitted from Hydrogen. When Hydrogen electrons transition between states, they...
1. We can observe the wavelengths emitted from Hydrogen. When Hydrogen electrons transition between states, they absorb or emit a particle of light called a photon with energy E=hf. Here f is the frequency of light and h is a constant. a. How much energy does an electron in the n=1 (lowest-energy) state of Hydrogen have? Repeat for n=2 and n=3. b. How much energy is emitted if an electron in the n=3 state transitions to the n=2 state? c....
1. The work-function of rubidium metal is 208 kJ/mol, which means that it takes 208 kJ...
1. The work-function of rubidium metal is 208 kJ/mol, which means that it takes 208 kJ to remove 1 mol of electrons from the surface of solid rubidium metal. a) What is the maximum wavelength of light needed to cause photoeffect with Rb(s)? (575 nm) b) What color is the light in part a? c) In a different photoeffect experiment with Rb(s), electrons with the de Broglie wavelength of 0.744 nm are generated. What is the wavelength of radiation used...
A certain photochemical reaction requires an excitation energy of 126 kJ mol^-1 . To what values...
A certain photochemical reaction requires an excitation energy of 126 kJ mol^-1 . To what values does this correspond in the following units: (A) frequency of light, (B) wave number, (C) wavelength in nanometers, and (D) electron volts?
(1) Part A: If a electron in a hydrogen atom makes a transition from ground state...
(1) Part A: If a electron in a hydrogen atom makes a transition from ground state to n = 8 level what wavelength of light in (nm) would be needed for the abosorbed photon to cause the transition? Part B: If the same electron falls to a lower level by emmitting a photon of light in the Paschen series what is the frequncy of light in (Hz) thats emitted? (2) When a photon have a wavelength of 195nm strikes the...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT