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I struggled on this question also, but now looking back at it, I think you would calculate the energy per photon required, using the equation E=hv or E=hc/lambda. And once you find that, I believe you would divide the energy that was given to you (in Joules) by the calculated energy you just found (joules/photon), canceling out the Joules, leaving you with the number of photons. This could be wrong though. I'm not for sure.
I also was confused on this question. I believe you were suppose to use the energy found in the previous problem, and relate this to the number of photons using Avogadro's number. Then once you had the photons convert to moles of Hydrogen atoms using the grams per mole of hydrogen.
AngieGarcia_4F wrote:Emily_4B wrote:Do you guys know if we’ll get the midterm back or be able to look at it in office hours to review this question?
My TA went over the midterm during discussion so maybe yours will too.
That sounds really helpful, thanks!
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