Question

) The C O bond dissociation energy in CO2 is 799 kJ/mol. The maximum wavelength of electromagnetic radiation required to rupture this bond is ________.

Answer 1

Answer:

λ = 150 nm

Explanation:

For C-O bond rupture:

The required energy to rupture C-O bond = bond energy of C-O bond

= 799 kJ/mol

$\mathsf{= 799 \ kJ/mol \times ( \dfrac{1 \ mol }{6.023 \times 10^{23} \ C-O \ bonds })}$

$\mathsf{= 1.3265 \times 10^{-21} \ kJ/ C-O \ bond}$

$\mathsf{= 1.33 \times 10^{-18} \ J/C-O \ bond}$

Recall that the wavelength associated with energy and frequency is expressed as:

$E = \dfrac{hc}{\lambda}$

$\lambda = \dfrac{hc}{E}$

$\lambda = \dfrac{(6.626 \times 10^{-34} \ J.s^{-1}) \times (3.0 \times 10^8 \ ms^{-1})}{ 1.33 \times 10^{-18} \ J/C-O \ bond}}$

$\mathsf{\lambda = 1.50 \times 10^{-7} \ m}$

λ = 150 nm