Calculating Spectroscopic Dissociation Energy for 127-I2 Molecule

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SUMMARY

The spectroscopic dissociation energy for the 127-I2 molecule is established at 1.542 eV, equating to approximately 2.47 x 10-19 joules. To calculate the necessary wavelength of light for dissociation while achieving atomic velocities of 1000 m/s, one must consider both the dissociation energy and the kinetic energy required. The correct approach involves using the equation wavelength = hc/E, where E must account for both the dissociation energy and the kinetic energy derived from KE = 1/2 mv2.

PREREQUISITES
  • Understanding of spectroscopic dissociation energy
  • Familiarity with energy conversion between electronvolts and joules
  • Knowledge of the Planck constant (h) and speed of light (c)
  • Basic principles of kinetic energy calculations
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  • Study the conversion of electronvolts to joules in detail
  • Learn about the Planck constant and its application in spectroscopy
  • Explore kinetic energy calculations and their implications in molecular dissociation
  • Research the relationship between energy, wavelength, and frequency in light
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Chemistry students, physicists, and researchers involved in molecular spectroscopy and energy calculations will benefit from this discussion.

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Homework Statement



The spectroscopic dissociation energy of 127-I2 is 1.542eV. What wavelength of light would be needed to dissociate the molecule and have the atoms move apart at velocities of 1000 m/s?

Homework Equations





The Attempt at a Solution



What I did was convert 1.542eV to joules which became 2.47x10^-19 joules/mol. After that I found the total energy per bond by dividing the energy be avagadro's number = 4.1x10^-43. Then plugged it into wavelength = hc/E = 4.8x10^17m. But this didn't look right. Am I going about it the wrong way? Or should I just go straight to wavelength = hc/E using the 1.542eV to find the wavelength. Or work backwards using KE=1/2 mv^2?

Thanks in advance
 
Physics news on Phys.org
1.542 eV is energy required for 1 molecule to be dissociated. However, your light must carry more energy, as the atoms need kinetic energy.
 

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