To calculate the maximum wavelength of light required to break a carbon-hydrogen single bond, we need to use the equation:
E = hc/λ
where E is the energy of the photon, h is the 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 of light.
First, let's convert the given energy of 412 kJ/mol to joules per molecule:
E = (412 kJ/mol) x (1000 J/1 kJ) / (6.022 x 10^23 mol^-1)
E = 6.834 x 10^-19 J
Now, we can rearrange the equation to solve for λ:
λ = hc/E
Substituting the values:
λ = (6.626 x 10^-34 J·s) * (2.998 x 10^8 m/s) / (6.834 x 10^-19 J)
λ = 2.911 x 10^-7 m
Since the question asks for the answer in nanometers (nm), let's convert the wavelength to nm:
λ = (2.911 x 10^-7 m) * (10^9 nm/1 m)
λ = 291.1 nm
Therefore, the maximum wavelength of light for which a carbon-hydrogen single bond could be broken by absorbing a single photon is 291.1 nm.
It takes 412kJ/mol to break a carbon hydrogen single bond calculate the maximum wavelength of light for which a carbon hydrogen single bond could be broken by absorbing a single photon
Be sure your answer has correct number of significant digits in nm
1 answer