The C- Cl and C- F bond dissociation energies in CF₃Cl are 339 kJ/mol and 482 kJ/mol, respectively. The maximum wavelengths of electromagnetic radiation required to rupture these bonds are
And , respectively.

Question

Quizplus · Accepted Answer

The energy required to break a bond can be found using the equation E = hc/λ, where E is the energy in J/mol, h is Planck's constant (6.626 x 10^-34 J s), c is the speed of light (2.998 x 10^8 m/s), and λ is the wavelength in meters. To convert kJ/mol to J/mol, we need to multiply by 1000.

For C-Cl bond dissociation: 
E = (339 x 1000) / (6.626 x 10^-34 x 2.998 x 10^8) 
E = 1.59 x 10^-18 J 
λ = hc/E 
λ = (6.626 x 10^-34) (2.998 x 10^8) / 1.59 x 10^-18 
λ = 1.25 x 10^-6 m 
λ = 1250 nm

For C-F bond dissociation: 
E = (482 x 1000) / (6.626 x 10^-34 x 2.998 x 10^8) 
E = 2.26 x 10^-18 J 
λ = hc/E 
λ = (6.626 x 10^-34) (2.998 x 10^8) / 2.26 x 10^-18 
λ = 8.76 x 10^-8 m 
λ = 87.6 nm

Therefore, the maximum wavelengths of electromagnetic radiation required to rupture these bonds are 1250 nm and 87.6 nm, which correspond to choice B.

The C- Cl and C- F Bond Dissociation Energies in CF3Cl

The C- Cl and C- F Bond Dissociation Energies in CF₃Cl