It takes 614./kJmol to break a carbon-carbon double bond. Calculate the maximum wavelength of light for which a carbon-carbon double bond could be broken by absorbing a single photon.Be sure your answer has the correct number of significant digits.nm

To solve this problem, we need to use the equation that relates energy, wavelength and Planck's constant:

E = h * c / λ

where: E is the energy per mole of photons, h is Planck's constant (6.626 x 10^-34 J*s), c is the speed of light (3.00 x 10^8 m/s), and λ is the wavelength.

We are given E in kJ/mol, but we need it in J/photon for the equation. To convert from kJ/mol to J/photon, we use Avogadro's number (6.022 x 10^23 mol^-1):

E = 614.4 kJ/mol * (10^3 J/kJ) / (6.022 x 10^23 mol^-1) = 1.02 x 10^-19 J/photon

Now we can solve for λ:

λ = h * c / E λ = (6.626 x 10^-34 J*s) * (3.00 x 10^8 m/s) / (1.02 x 10^-19 J/photon) λ = 1.94 x 10^-7 m

Since the question asks for the answer in nm, we convert from m to nm:

λ = 1.94 x 10^-7 m * (10^9 nm/m) = 194 nm

So, the maximum wavelength of light for which a carbon-carbon double bond could be broken by absorbing a single photon is 194 nm.