Respuesta :
This is a incomplete question. The complete question is:
It takes 348 kJ/mol to break a carbon-carbon single bond. Calculate the maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon. Round your answer to correct number of significant digits
Answer: 344 nm
Explanation:
[tex]E=\frac{Nhc}{\lambda}[/tex]
E= energy = 348kJ= 348000 J (1kJ=1000J)
N = avogadro's number = [tex]6.023\times 10^{23}[/tex]
h = Planck's constant = [tex]6.626\times 10^{-34}Js [/tex]
c = speed of light = [tex]3\times 10^8ms^{-1}[/tex]
[tex]348000=\frac{6.023\times 10^{23}\times 6.626\times 10^{-34}\times 3\times 10^8}{\lambda}[/tex]
[tex]\lambda=\frac{6.023\times 10^{23}\times 6.626\times 10^{-34}\times 3\times 10^8}{348000}[/tex]
[tex]\lambda=3.44\times 10^{-7}m=344nm[/tex] [tex]1nm=10^{-9}m[/tex]
Thus the maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon is 344 nm
