Use ν = c / λ to get the frequency:
x = (3.00 x 108 m s¯1) / (655 x 10¯9 m) = .004580* x 1017 s¯1.Now use E = hν to get the energy:
x = (6.6260755 x 10¯34 J s) (.004580* x 1017 s¯1.) = .030348 x 10¯17 JThis is the energy for one photonThe next step is to find the kilojoules for one mole and for this we use Avogadro's Number (.030348 x 10¯17 J/photon) (6.022 x 1023 photon mol¯1)= .182755 * 106Dividing the answer by 1000 to make the change to kilojoules, we get 182.755 kJ/mol.The last step is to find the kilojoules for 3 moles ,that is 3 x 182.755 = 548.265 KJSo the correct answer is D: 548KJPlease let me know if it is helpful and best me if you are satisfactory.
Now use E = hν to get the energy:
x = (6.6260755 x 10¯34 J s) (.004580* x 1017 s¯1.) = .030348 x 10¯17 JThis is the energy for one photon
Please let me know if you have any other questions
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