343.9 nm wavelength of light is required to break carbon-carbon single bond by absorbing a single photon.
Given,
To break 1 mol of carbon-carbon single bond energy required= 348kj
To break 6.023×10^23 molecules of carbon-carbon single bond energy required = 348kj
To break 1 molecules of carbon-carbon single bond energy required= 348 ×1000 j / 6.023×10^23
= 57.77 ×10^-20 j
As we know,
Energy(E) = hc / λ
Where, E = energy required
h = Planck's constant = 6.623×10^-34 js
c = speed of light =3×10^8 m/s
λ = lambda = wavelength
Now, putting all the values we will get,
57.77×10^-20 j =[ (6.623×10^-34js )×( 3×10^8 m/s) ]/ λ
57.77×10^-20 j =( 19.869 ×10^-26jm) / λ
λ = 19.869×10^-26 jm / 57.77×10^-20 j
λ = 0.3439× 10^-6 m
λ = 343.9 × 10^-9 m
λ = 343.9 nm
Hence, 343.9 nm wavelength of light is required to break carbon-carbon single bond by absorbing a single photon.
Learn more about wavelength here :
brainly.com/question/10728818
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