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

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

Chemistry
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You must know the formula for calculating the energy... in this situation. Do you know the formula?
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
that v is actually "new (pronounced as new)"

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So @jennilalala with the help of : E = hv formula, can you find the energy by putting the values given ?
"v" --> \(\large{\color{blue}{\nu}}\) .... right @aaronq ?
I am back sorry ahaah. yes i know the formulas. i just dont know what to do if it says ".32 moles of photon.."
Do you the planck's constant ?
6.626x10^23 ?? not by heart...yet...
haha yep, v= "new"
10^-34
OK so it is \[\large { h = 6.626 \times 10^{-34} m^{-1}}\]
oh wait it is m^2 kg/s
So right, now solve this : \[\large{E = 6.626 \times 10^{-34} \times 2.6 \times 10^{15}}\] What do you get?
1.73x10^-18
My calculator says it as : \(\large{\color{blue}{ 17.2276 * 10^{-19}}}\) that is 1.72276 * 10^{-18}
OK so now .. this is the energy for \(1\) photon ... now we to calculate for 0.32 moles of photons.
See ... no. of photons = Avogadros's constant * no. of moles of photons...
You know avogadro's constant?
6.022x10^23
Good! So now, solve this one : \[\large{\color{red}{\mathbb{No. of Photons}} = \color{blue}{6.022 * {10}^{23}} \times \color{green}{0.32}}\]
1.93x10^23
then i multiply the two calculations?
Correct! So this is your No. of photons. Now multiply this result with "1.73 * 10^{-18} "
3.3x10^-5
Right!
not negative typo lol
No problem.
So finally you have your correct way, I hope you got it ?
Yes thank you so much!
You're welcome @jennilalala . keep up the good work.

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