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

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SheldonEinsteinBest ResponseYou've already chosen the best response.2
You must know the formula for calculating the energy... in this situation. Do you know the formula?
 one year ago

aaronqBest ResponseYou've already chosen the best response.1
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
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
that v is actually "new (pronounced as new)"
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
So @jennilalala with the help of : E = hv formula, can you find the energy by putting the values given ?
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
"v" > \(\large{\color{blue}{\nu}}\) .... right @aaronq ?
 one year ago

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

SheldonEinsteinBest ResponseYou've already chosen the best response.2
Do you the planck's constant ?
 one year ago

jennilalalaBest ResponseYou've already chosen the best response.0
6.626x10^23 ?? not by heart...yet...
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
OK so it is \[\large { h = 6.626 \times 10^{34} m^{1}}\]
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
oh wait it is m^2 kg/s
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
So right, now solve this : \[\large{E = 6.626 \times 10^{34} \times 2.6 \times 10^{15}}\] What do you get?
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
My calculator says it as : \(\large{\color{blue}{ 17.2276 * 10^{19}}}\) that is 1.72276 * 10^{18}
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
OK so now .. this is the energy for \(1\) photon ... now we to calculate for 0.32 moles of photons.
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
See ... no. of photons = Avogadros's constant * no. of moles of photons...
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
You know avogadro's constant?
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
Good! So now, solve this one : \[\large{\color{red}{\mathbb{No. of Photons}} = \color{blue}{6.022 * {10}^{23}} \times \color{green}{0.32}}\]
 one year ago

jennilalalaBest ResponseYou've already chosen the best response.0
then i multiply the two calculations?
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
Correct! So this is your No. of photons. Now multiply this result with "1.73 * 10^{18} "
 one year ago

jennilalalaBest ResponseYou've already chosen the best response.0
not negative typo lol
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
So finally you have your correct way, I hope you got it ?
 one year ago

jennilalalaBest ResponseYou've already chosen the best response.0
Yes thank you so much!
 one year ago

SheldonEinsteinBest ResponseYou've already chosen the best response.2
You're welcome @jennilalala . keep up the good work.
 one year ago
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