x = (3.00 x 10^{8} m s¯^{1}) / (655 x 10¯^{9} m) = .004580* x 10^{17} s¯^{1}.

Now use E = hν to get the energy:

x = (6.6260755 x 10¯^{34} J s) (.004580* x 10^{17} s¯^{1}.^{}) = .030348 x 10¯^{17 J}

This is the energy for one photon

The 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 10^{23} photon mol¯^{1})

= .182755 * 10^{6}

Dividing 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 KJ

So the correct answer is D: 548KJ

Please let me know if it is helpful and best me if you are satisfactory.

Apr 6th, 2015

hi,

Please let me know if you have any other questions