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jennilalala Group Title

Calculate the energy in J of 0.32 moles of photons whose frequency is 2.6 x 10^15 ?

  • 2 years ago
  • 2 years ago

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  1. SheldonEinstein Group Title
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    You must know the formula for calculating the energy... in this situation. Do you know the formula?

    • 2 years ago
  2. aaronq Group Title
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    E=hv h is planks constant v= frequency this gives you the energy of 1 photon so multiply this by the amount of photons you have: amount of photons = avogadros constant x number of moles

    • 2 years ago
  3. SheldonEinstein Group Title
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    that v is actually "new (pronounced as new)"

    • 2 years ago
  4. SheldonEinstein Group Title
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    So @jennilalala with the help of : E = hv formula, can you find the energy by putting the values given ?

    • 2 years ago
  5. SheldonEinstein Group Title
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    "v" --> \(\large{\color{blue}{\nu}}\) .... right @aaronq ?

    • 2 years ago
  6. jennilalala Group Title
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    I am back sorry ahaah. yes i know the formulas. i just dont know what to do if it says ".32 moles of photon.."

    • 2 years ago
  7. SheldonEinstein Group Title
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    Do you the planck's constant ?

    • 2 years ago
  8. jennilalala Group Title
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    6.626x10^23 ?? not by heart...yet...

    • 2 years ago
  9. aaronq Group Title
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    haha yep, v= "new"

    • 2 years ago
  10. jennilalala Group Title
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    10^-34

    • 2 years ago
  11. SheldonEinstein Group Title
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    OK so it is \[\large { h = 6.626 \times 10^{-34} m^{-1}}\]

    • 2 years ago
  12. SheldonEinstein Group Title
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    oh wait it is m^2 kg/s

    • 2 years ago
  13. SheldonEinstein Group Title
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    So right, now solve this : \[\large{E = 6.626 \times 10^{-34} \times 2.6 \times 10^{15}}\] What do you get?

    • 2 years ago
  14. jennilalala Group Title
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    1.73x10^-18

    • 2 years ago
  15. SheldonEinstein Group Title
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    My calculator says it as : \(\large{\color{blue}{ 17.2276 * 10^{-19}}}\) that is 1.72276 * 10^{-18}

    • 2 years ago
  16. SheldonEinstein Group Title
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    OK so now .. this is the energy for \(1\) photon ... now we to calculate for 0.32 moles of photons.

    • 2 years ago
  17. SheldonEinstein Group Title
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    See ... no. of photons = Avogadros's constant * no. of moles of photons...

    • 2 years ago
  18. SheldonEinstein Group Title
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    You know avogadro's constant?

    • 2 years ago
  19. jennilalala Group Title
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    6.022x10^23

    • 2 years ago
  20. SheldonEinstein Group Title
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    Good! So now, solve this one : \[\large{\color{red}{\mathbb{No. of Photons}} = \color{blue}{6.022 * {10}^{23}} \times \color{green}{0.32}}\]

    • 2 years ago
  21. jennilalala Group Title
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    1.93x10^23

    • 2 years ago
  22. jennilalala Group Title
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    then i multiply the two calculations?

    • 2 years ago
  23. SheldonEinstein Group Title
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    Correct! So this is your No. of photons. Now multiply this result with "1.73 * 10^{-18} "

    • 2 years ago
  24. jennilalala Group Title
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    3.3x10^-5

    • 2 years ago
  25. SheldonEinstein Group Title
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    Right!

    • 2 years ago
  26. jennilalala Group Title
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    not negative typo lol

    • 2 years ago
  27. SheldonEinstein Group Title
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    No problem.

    • 2 years ago
  28. SheldonEinstein Group Title
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    So finally you have your correct way, I hope you got it ?

    • 2 years ago
  29. jennilalala Group Title
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    Yes thank you so much!

    • 2 years ago
  30. SheldonEinstein Group Title
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    You're welcome @jennilalala . keep up the good work.

    • 2 years ago
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