Question

What is the wavelength (in meters) of photons with the following energies?

93.0 kJ/mol

8.25×10^{−4} kJ/mol

1860 kJ/mol

Answer #1

Use the following equation:

E = h*c / so: = h*c / E

Where:

h = planck constant = 6.63x10^{-34} J s

c = speed of light = 3x10^{8} m/s

With these values and the energies given, calculate wavelenght for every energy, but first, let's neglect the moles:

93,000 J/mol * 1 mol / 6.022x10^23 atoms = 1.52x10^{-19}
J

1
= 6.63x10^{-34} * 3x10^{8} / 1.54x10^{-19}
= 1.29x10^{-6} m

0.825 / 6.022x10^{23} = 1.37x10^{-24} J

2
= 6.63x10^{-34} * 3x10^{8} / 1.37x10^{-24}
= 0.1452 m

1860000 / 6.02x10^{23} = 3.09x10^{-18}

3
= 6.63x10^{-34} * 3x10^{8} / 3.09x10^{-18}
= 6.44x10^{-8} m

Hope this helps.

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