Calculating Spectroscopic Dissociation Energy for 127-I2 Molecule

AI Thread Summary
The spectroscopic dissociation energy for the 127-I2 molecule is 1.542 eV, which translates to approximately 2.47 x 10^-19 joules. To find the wavelength of light needed for dissociation while achieving a velocity of 1000 m/s for the atoms, it's essential to account for the additional kinetic energy required. The correct approach involves using the equation wavelength = hc/E, where E must include both the dissociation energy and the kinetic energy calculated from KE = 1/2 mv^2. The initial calculation of energy per bond appears to be incorrect, suggesting a need to directly apply the energy values without unnecessary conversions. Ultimately, the light's energy must exceed the dissociation energy to provide the necessary kinetic energy for the atoms.
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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
 
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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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