Photon to break C=C bond

Question

The C= C bond is very strong with a large bond energy of 962 kJ/mol. Calculate the frequency of the photon required to break this bond. Calculate the wavelength of the photon required to break a C=C bond in nm.

Answer 1

E for mole of C=C bonds: 962 kJ/mol * 1000 J / 1 kJ = 962,000 J / mol

Divide by Avogadro's for a single bond:

(962,000 J/mol)/6.02*10^23 = 1.598 * 10^-18 J / bond

Wavelength = Planck's * speed of light / energy to break bond

= hc / E = (6.63 * 10^-34)(3*10^8) / (1.598 * 10^-18 J / bond) = 1.24*10^-7 m

Finally, convert from m to nm:

1.24*10^-7 m * 10^9 nm/1m = 124 nm