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anonymous

  • one year ago

What is the wavelength (in nm) of radiation that has an energy content of 7.67 x 10^3 kJ/mol? I got myself confused on how to set it up.

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  1. aaronq
    • one year ago
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    you have to get the value in energy terms (per photon, not per mole of photons)

  2. anonymous
    • one year ago
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    How do you set that up? Do you use the E = hv formula?

  3. aaronq
    • one year ago
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    yeah, but you need to divide by avogadro's number first

  4. anonymous
    • one year ago
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    For which part?

  5. anonymous
    • one year ago
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    \[\frac{ 7.67 \times 10^3 kJ }{ mol } \times \frac{ 1000J }{ 1kJ } \times \frac{ 1mol }{6.022 \times 10^{23}photons }\]. You would use this dimensional analysis to find energy per photon (J/photon). This would be E Next use E=hv h is a Planck constant Find v which is frequency Then use \[c=\lambda v\] where c is speed of light. It has a constant of 3.00 x 10^8m/s You are to find lambda which is wavelength. It would be in meters. 1m=1.0 x 10^9nm Good luck solving it.

  6. anonymous
    • one year ago
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    1.56 x 10^11. Would that be right?

  7. anonymous
    • one year ago
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    You mean 1.56 x 10^1 Because thats what I got.

  8. anonymous
    • one year ago
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    Yeah. Meant that.

  9. anonymous
    • one year ago
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    How do you tell where it is on the electromagnetic spectrum?

  10. anonymous
    • one year ago
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    Alright. Thank you.

  11. anonymous
    • one year ago
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    You write the answer in meters Then you would use this chart. http://www2.lbl.gov/MicroWorlds/ALSTool/EMSpec/EMSpec2.html

  12. anonymous
    • one year ago
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    No problem! It can be challenging at first. Good luck on your work.

  13. anonymous
    • one year ago
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    Thanks!

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