Simple energy with photons problem help

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SUMMARY

The energy of 1.7 moles of photons with a wavelength of 0.28 μm can be calculated using the formula E = HC/W, where H is Planck's constant (6.63e-34 J·s), C is the speed of light (3e8 m/s), and W is the wavelength in meters (0.00000028 m). The initial calculation yields an energy per photon of approximately 7.10357e-21 J. To find the total energy for 1.7 moles, multiply the energy per photon by Avogadro's number (6.022e23), resulting in a total energy of approximately 7.10357e-21 J * (1.7 * 6.022e23).

PREREQUISITES
  • Understanding of Planck's constant (H)
  • Knowledge of the speed of light (C)
  • Familiarity with Avogadro's number (6.022e23)
  • Basic grasp of wavelength and energy relationships in physics
NEXT STEPS
  • Research the relationship between energy and wavelength in electromagnetic radiation
  • Learn about the concept of moles in chemistry and its application to photons
  • Explore the implications of Planck's constant in quantum mechanics
  • Study the calculation of energy in different contexts, such as chemical reactions and photon interactions
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Students in physics or chemistry, educators teaching quantum mechanics, and anyone interested in the energy calculations 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)
photons
 

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