Simple energy with photons problem help

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To calculate the energy of 1.7 mol of photons with a wavelength of 0.28 μm, the formula E = HC/W is used, yielding an energy value of approximately 7.1 x 10^-21 J for a single photon. To find the total energy for 1.7 mol, multiply the energy of one photon by Avogadro's number (6.022 x 10^23). This results in a total energy calculation of 1.7 x (7.1 x 10^-21 J) x (6.022 x 10^23), which provides the correct total energy. The confusion arises from how to incorporate the mole quantity, but multiplying by Avogadro's number is the correct approach. The final energy value reflects the total energy of the specified number of photons.
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Simple energy with photons problem...help!

Homework Statement


What is the energy of 1.7 mol of photons that have a wavelength of 0.28 μm?


Homework Equations





The Attempt at a Solution


E = HC/W = (6.63e^34)*(3e^8)/0.00000028 = 7.10357e^-21
what do I do with the mol part? I know 1 mol = 6.022e^23 so I tried multiplying it by that but its wrong...do I divide. Or is there something else I have to do?
 
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your approach looks ok. you have 1.7 mol of photons so you have 1.7*(6.022*10^23)
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