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

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anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0You must know the formula for calculating the energy... in this situation. Do you know the formula?

aaronq
 4 years ago
Best ResponseYou've already chosen the best response.1E=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

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0that v is actually "new (pronounced as new)"

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0So @jennilalala with the help of : E = hv formula, can you find the energy by putting the values given ?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0"v" > \(\large{\color{blue}{\nu}}\) .... right @aaronq ?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0I am back sorry ahaah. yes i know the formulas. i just dont know what to do if it says ".32 moles of photon.."

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Do you the planck's constant ?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.06.626x10^23 ?? not by heart...yet...

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0OK so it is \[\large { h = 6.626 \times 10^{34} m^{1}}\]

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0oh wait it is m^2 kg/s

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0So right, now solve this : \[\large{E = 6.626 \times 10^{34} \times 2.6 \times 10^{15}}\] What do you get?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0My calculator says it as : \(\large{\color{blue}{ 17.2276 * 10^{19}}}\) that is 1.72276 * 10^{18}

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0OK so now .. this is the energy for \(1\) photon ... now we to calculate for 0.32 moles of photons.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0See ... no. of photons = Avogadros's constant * no. of moles of photons...

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0You know avogadro's constant?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Good! So now, solve this one : \[\large{\color{red}{\mathbb{No. of Photons}} = \color{blue}{6.022 * {10}^{23}} \times \color{green}{0.32}}\]

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0then i multiply the two calculations?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Correct! So this is your No. of photons. Now multiply this result with "1.73 * 10^{18} "

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0not negative typo lol

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0So finally you have your correct way, I hope you got it ?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Yes thank you so much!

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0You're welcome @jennilalala . keep up the good work.
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